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S  6 `P   P*    6 `   R*  H  0޽h ? ̙3380___PPT10.0 0X(   $+ X X 0 P    X*  X 0     Z*  X 6 `P   X*  X 6 `   Z* H X 0޽h ? ̙3380___PPT10.= v 0L0 }P*(     0!~ /ACIDS, BASES & SALTS A guide for GCSE students b/(28(26f<fff  0%(H OKNOCKHARDY PUBLISHING(2 fJ  C "A KTRE: . " <̙? x @ 0 0 ( <̙? x @L 0 0T ) C ,Agcselogo2 * 0-"`>B 2010 SPECIFICATIONSH0 G$G  B  s *޽h ? ̙33y___PPT10Y+D=' = @B +; 0L0 JB@0(  0 0 0H@} PACIDS, BASES & SALTS (2 f= 0 04pg  INTRODUCTION This Powerpoint show is one of several produced to help students understand selected GCSE Chemistry topics. It is based on the requirements of the AQA specification but is suitable for other examination boards. Individual students may use the material at home for revision purposes and it can also prove useful for classroom teaching with an interactive white board. Accompanying notes on this, and the full range of AS and A2 Chemistry topics, are available from the KNOCKHARDY WEBSITE at... www.knockhardy.org.uk~ (2 2(2 ! , dB 0 <D?  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Permission must be obtained for their use in any commercial work.$CH$   &  C z 0 bA޽h @ ?Parchment ̙33y___PPT10Y+D=' = @B + 0L0   H (    0C"?0 b CONTENTS Acidity and alkalinity Indicators pH Acids General methods for making salts Making salts from metal oxides Making salts from metal carbonates Making salts from metals Making salts from alkalis  by titration Making insoluble salts  by precipitation Questionsb 202 2!!}   0C"? n@ 0 0  6C"? y@ 0 0   6C"?@  0 0   6C"?P@ 0 0   6C"? @d 0 0   6C"?   @X 0 0   6C"? p @R 0 0  0\+H@} PACIDS, BASES & SALTS (2 f  6C"?  @^ 0 0  6C"?   @L 0 0  6C"?@@ 0 0  6C"? @j 0 0B  s *޽h ? ̙33y___PPT10Y+D=' = @B + 0 v(    0@ ^ACIDITY AND ALKALINITY,(2ff  0(s " water is a neutral substance " when substances dissolve in water, the solution may become& ACIDIC or ALKALINE or stay NEUTRAL |c  3! @`T  C ,Agcselogo2H  0޽h ? ̙33y___PPT10Y+D=' = @B +y 0  0(    0` ^ACIDITY AND ALKALINITY,(2ff  0$Ύ(s  vX" water is a neutral substance " when substances dissolve in water, the solution may become& ACIDIC or ALKALINE or stay NEUTRAL " hydrogen ions H+(aq) make solutions acidic " hydroxide ions OH(aq) make solutions alkaline " solutions with equal numbers of H+(aq) and OH(aq) are neutral l-c 3!!!f/fff 3   3!x + # @`T  C ,Agcselogo2H  0޽h ? ̙33y___PPT10Y+D=' = @B +y 0 p <0(  < < 0h R INDICATORS, (2 ff < T s_ж_ж?"`&s` |" show by a colour change if a solution is acidic, alkaline or neutral " some can even show how acidic or how alkaline a solution is  v @` < n_ж_жA3ParchmentS" ?X`  < n_ж_жA3ParchmentS" ? `  < n_ж_жA3ParchmentS" ?`  < n_ж_жA3ParchmentS" ? X  < n_ж_жA3ParchmentS" ?  T  < C ,Agcselogo2H < 0޽h ? ̙33y___PPT10Y+D=' = @B + 0   (    0s R INDICATORS, (2 ffT  T_ж_ж?"`&s V" show by a colour change if a solution is acidic, alkaline or neutral " some can even show how acidic or how alkaline a solution is " well known indicators include&   @`T   C ,Agcselogo2H  0޽h ? ̙33y___PPT10Y+D=' = @B +- 0 TL @(  @ @ 0s R INDICATORS, (2 ffJ @ T$s_ж_ж?"`&s  " show by a colour change if a solution is acidic, alkaline or neutral " some can even show how acidic or how alkaline a solution is " well known indicators include& LITMUS acidic RED alkaline BLUE neutral PURPLE    @` @ n_ж_жA3ParchmentS" ?X`  @ n_ж_жA3ParchmentS" ? `  @ n_ж_жA3ParchmentS" ?` T  @ C ,Agcselogo2H @ 0޽h ? ̙33y___PPT10Y+D=' = @B + 0   (    07s R INDICATORS, (2 ffL  T:s_ж_ж?"`&s  " show by a colour change if a solution is acidic, alkaline or neutral " some can even show how acidic or how alkaline a solution is " well known indicators include& LITMUS acidic RED alkaline BLUE neutral PURPLE    @`T   C ,Agcselogo2H  0޽h ? ̙33y___PPT10Y+D=' = @B +  0 6. (    0p8s R INDICATORS, (2 ff,  TTs_ж_ж?"`&s  \" show by a colour change if a solution is acidic, alkaline or neutral " some can even show how acidic or how alkaline a solution is " well known indicators include& LITMUS acidic RED alkaline BLUE neutral PURPLE UNIVERSAL acidic RED alkaline VIOLET neutral GREEN/  f3  @`T   C ,Agcselogo2   n_ж_жA3ParchmentS" ? H    n_ж_жA3ParchmentS" ?    n_ж_жA3ParchmentS" ?  H  0޽h ? ̙33y___PPT10Y+D=' = @B + 0 Hz(  H H 0|as R INDICATORS, (2 ff, H Tus_ж_ж?"`&s  \" show by a colour change if a solution is acidic, alkaline or neutral " some can even show how acidic or how alkaline a solution is " well known indicators include& LITMUS acidic RED alkaline BLUE neutral PURPLE UNIVERSAL acidic RED alkaline VIOLET neutral GREEN/  f3  @`T H C ,Agcselogo2H H 0޽h ? ̙33y___PPT10Y+D=' = @B + 0 PD(  P P 0ws PpH SCALE, (2ffT P C ,Agcselogo2H P 0޽h ? ̙33y___PPT10Y+D=' = @B + 0 91L(  L L 0s PpH SCALE, (2ff} L 0$s(s  Used to compare the relative acidity (and alkalinity) of solutions. The value is related to the concentration of H+ions, in solution. Br r @`T L C ,Agcselogo2H L 0޽h ? ̙33y___PPT10Y+D=' = @B +S 0 zrX (  X X 0Ps PpH SCALE, (2ff X 0s(s ^ Used to compare the relative acidity (and alkalinity) of solutions. The value is related to the concentration of H+ions, in solution.  The greater the concentration of hydrogen ions in solution, the lower the pH ^Or O!r_ @`T X C ,Agcselogo2H X 0޽h ? ̙33y___PPT10Y+D=' = @B +  0 D<(    0s PpH SCALE, (2ff  0|u(s  (` Used to compare the relative acidity (and alkalinity) of solutions. The value is related to the concentration of H+ions, in solution.  The greater the concentration of hydrogen ions in solution, the lower the pH < 0 1 2 3 4 5 6 7 8 9 10 11 12 13 14  > strongly weakly neutral weakly strongly acidic acidic alkaline alkaline POrO   3  f 3 f    f f>r   @`T  C ,Agcselogo2H  0޽h ? ̙33y___PPT10Y+D=' = @B +;  0 b Z  (    0u PpH SCALE, (2ff  0u(s  F Used to compare the relative acidity (and alkalinity) of solutions. The value is related to the concentration of H+ions, in solution.  The greater the concentration of hydrogen ions in solution, the lower the pH < 0 1 2 3 4 5 6 7 8 9 10 11 12 13 14  > strongly weakly neutral weakly strongly acidic acidic alkaline alkaline HCl CH3COOH H2O NH3 NaOH HYDROCHLORIC ETHANOIC AMMONIA SODIUM ACID ACID HYDROXIDE OrO   3  f 3 f    f f       ~ vr  #  @`T  C ,Agcselogo2H  0޽h ? ̙33y___PPT10Y+D=' = @B +A  0 h `  (    0"u PpH SCALE, (2ff  0vu(s5 L | Used to compare the relative acidity (and alkalinity) of solutions. The value is related to the concentration of H+ions, in solution.  The greater the concentration of hydrogen ions in solution, the lower the pH < 0 1 2 3 4 5 6 7 8 9 10 11 12 13 14  > strongly weakly neutral weakly strongly acidic acidic alkaline alkaline HCl CH3COOH H2O NH3 NaOH HYDROCHLORIC ETHANOIC AMMONIA SODIUM ACID ACID HYDROXIDE Acidic solutions pH < 7 Alkaline solutions pH > 7 Neutral solutions pH = 7OrO   3  f 3 f    f f        3r  #m W @`T  C ,Agcselogo2H  0޽h ? ̙33y___PPT10Y+D=' = @B + 0 T(  T T 0]u PpH SCALE, (2ffD T 0s(so  Despite what some people think, the pH scale is not restricted to between 0 and 14. It extends beyond those values, but is not as relevant; e.g. the pH of the dilute HCl and H2SO4 found on the laboratory shelves is -0.3 and -0.6 respectively.  2!W  BL @`T T C ,Agcselogo2H T 0޽h ? ̙33y___PPT10Y+D=' = @B += 0 d\(    0nu PpH SCALE, (2ff  0$u(s/  H Despite what some people think, the pH scale is not restricted to between 0 and 14. It extends beyond those values, but is not as relevant; e.g. the pH of the dilute HCl and H2SO4 found on the laboratory shelves is -0.3 and -0.6 respectively. Weak acids have higher pH values than stronger ones of the same concentration. Ethanoic acid CH3COOH has a larger pH than hydrochloric acid HCl of the same concentration. G\BP!!.!!!b  5    @`T  C ,Agcselogo2H  0޽h ? ̙33y___PPT10Y+D=' = @B + 0 \D(  \ \ 0u T MEASURING pH, (2 ff \ 0u(sb Indicator Add a few drops of universal (full-range) indicator to the solution and compare the colour against a chart. The colour you  see depends not only on how many drops of indicator you add but also on your perception of colour. Rah  @`T \ C ,Agcselogo2H \ 0޽h ? ̙33y___PPT10Y+D=' = @B + 0  `(    0u T MEASURING pH, (2 ff  04u(s  Indicator Add a few drops of universal (full-range) indicator to the solution and compare the colour against a chart. The colour you  see depends not only on how many drops of indicator you add but also on your perception of colour. pH meters Electrical/electronic devices which measure the conductivity of the solution. Having calibrated the apparatus against a solution of known pH, you place the probe in any solution and read off the pH value on a scale or digital read-out.*Rah  @`T  C ,Agcselogo2H  0޽h ? ̙33y___PPT10Y+D=' = @B + 0 XA(  X X 0u MACIDS,(2ffT X C ,Agcselogo2H X 0޽h ? ̙33y___PPT10Y+D=' = @B +e 0 0(    0u MACIDS,(2ff  0u(s sDefinition ACIDS ARE PROTON (H+ ion) DONORS Categories Acids can be arranged into groups according to how many H+ ions they produce from each molecule @ !  != , @`T  C ,Agcselogo2H  0޽h ? ̙33y___PPT10Y+D=' = @B +< 0 c[`(    0u MACIDS,(2ff  0D4w(s'  JxDefinition ACIDS ARE PROTON (H+ ion) DONORS Categories Acids can be arranged into groups according to how many H+ ions they produce from each molecule ACID SALTS ION EXAMPLE hydrochloric HCl chloride Cl NaCl nitric HNO3 nitrate NO3 NaNO3 ethanoic CH3COOH ethanoate CH3COO CH3COONa THE ABOVE ARE MONOPROTIC (MONOBASIC) ACIDS"@+H !  != 1)ff ffff   ffff fff+v $ +  @`T  C ,Agcselogo2H  0޽h ? ̙33y___PPT10Y+D=' = @B +  0   p= (    0#w MACIDS,(2ff|  0̂w(s  zDefinition ACIDS ARE PROTON (H+ ion) DONORS Categories Acids can be arranged into groups according to how many H+ ions they produce from each molecule ACID SALTS ION EXAMPLE hydrochloric HCl chloride Cl NaCl nitric HNO3 nitrate NO3 NaNO3 ethanoic CH3COOH ethanoate CH3COO CH3COONa THE ABOVE ARE MONOPROTIC (MONOBASIC)ACIDS sulphuric H2SO4 hydrogensulphate HSO4 NaHSO4 sulphate SO42- Na2SO4  carbonic H2CO3 hydrogencarbonate HCO3 NaHCO3 carbonate CO32- Na2CO3 THE ABOVE ARE DIPROTIC (DIBASIC)ACIDS@*H @& !  != 1)     + 33333333 3333333 fffffffffffffff& $ +   "-%  @`pB  H_ж_жDo  T  C ,Agcselogo2H  0޽h ? ̙33y___PPT10Y+D=' = @B +* 0 QI@(    0hw MACIDS,(2ff  0|mw(sb 8Definition ACIDS ARE PROTON (H+ ion) DONORS Categories Acids can also arranged into groups according to the extent they split into ions when put in water.h !  !h @`T  C ,Agcselogo2H  0޽h ? ̙33y___PPT10Y+D=' = @B + 0 $`(  ` ` 0XZw MACIDS,(2ffk ` 0\w(s"  Definition ACIDS ARE PROTON (H+ ion) DONORS Categories Acids can also arranged into groups according to the extent they split into ions when put in water. STRONG ACIDS COMPLETELY dissociate (split up) into ions e.g. sulphuric, hydrochloric, nitric  !  !i f M&   @`T ` C ,Agcselogo2H ` 0޽h ? ̙33y___PPT10Y+D=' = @B +s 0 \*(  \ \ 0w MACIDS,(2ff \ 0w(sb  _Definition ACIDS ARE PROTON (H+ ion) DONORS Categories Acids can also arranged into groups according to the extent they split into ions when put in water. STRONG ACIDS COMPLETELY dissociate (split up) into ions e.g. sulphuric, hydrochloric, nitric WEAK ACIDS PARTIALLY dissociate (split up) into ions e.g. ethanoic, citric, carbonic` !  !ic F@  A @`T \ C ,Agcselogo2H \ 0޽h ? ̙33y___PPT10Y+D=' = @B + 0 $(    0w MACIDS,(2ffk  0z(s ODefinition ACIDS ARE PROTON (H+ ion) DONORS Categories Acids can also arranged into groups according to the extent they split into ions when put in water. STRONG ACIDS COMPLETELY dissociate (split up) into ions e.g. sulphuric, hydrochloric, nitric WEAK ACIDS PARTIALLY dissociate (split up) into ions e.g. ethanoic, citric, carbonic This means that if you take similar concentrations of HCl and CH3COOH, the concentration of H+ ions in the solution of CH3COOH will be less as only a few of its molecules will have split up into ions. Its pH will consequently be higher.P !  !i9   O"!f  A 6 @`T  C ,Agcselogo2H  0޽h ? ̙33y___PPT10Y+D=' = @B +' 0 NF(    0w MACIDS,(2ff  0$z(s 5Reactions The hydrogen ions produced by acids can be replaced by other positive ions (metal ions or ammonium ions) to produce salts. This occurs when dilute acids react with metals, oxides of metals, hydroxides of metals, carbonates, hydrogencarbonates and ammonia.  !ff3 ff3 @`T  C ,Agcselogo2H  0޽h ? ̙33y___PPT10Y+D=' = @B + 0 '" (    0(z MACIDS,(2ff  06z(s 4Reactions The hydrogen ions produced by acids can be replaced by other positive ions (metal ions or ammonium ions) to produce salts. This occurs when dilute acids react with metals, oxides of metals, hydroxides of metals, carbonates, hydrogen carbonates and ammonia. HYDROCHLORIC ACIDN5  @`T  C ,Agcselogo2  0z  Y ZINC CHLORIDE @`  0Pz} ]r7  [SODIUM CHLORIDE @`  0$Zz e [COPPER CHLORIDE @`vB @ N_ж_жD>8 vB @ N_ж_жD>=h vB  N_ж_жD>=)    0Hz} -7  ]AMMONIUM CHLORIDE @`vB  N_ж_жD> -   0mz! `}  TZINC @`  0vzf3MW   SODIUM HYDROXIDE>  @`  0Gzf |  | COPPER OXIDE>  @`  0wz3M z  WAMMONIA @`vB   N_ж_жD>M  ! 0`z =  ^MAGNESIUM CHLORIDE @` " 0ezff^ )  cMAGNESIUM CARBONATE @`H  0޽h ? ̙33y___PPT10Y+D=' = @B + 0 80" (    0z MACIDS,(2ff%  0w(s 7Reactions The hydrogen ions produced by acids can be replaced by other positive ions (metal ions or ammonium ions) to produce salts. This occurs when dilute acids react with metals, oxides of metals, hydroxides of metals, carbonates, hydrogen carbonates and ammonia. SULPHURIC ACID\8  @`T  C ,Agcselogo2  00z  Y ZINC SULPHATE @`  0 z} ]r7  [SODIUM SULPHATE @`  0z e [COPPER SULPHATE @`vB @ N_ж_жD>8 vB @ N_ж_жD>=h vB  N_ж_жD>=)    0`z} -7  ]AMMONIUM SULPHATE @`vB  N_ж_жD> -   0z! `}  TZINC @`  0zf3MW   SODIUM HYDROXIDE>  @`  0{f |  | COPPER OXIDE>  @`  0{3M z  WAMMONIA @`vB   N_ж_жD>M  ! 0x{ =  ^MAGNESIUM SULPHATE @` " 0{ff^ )  cMAGNESIUM CARBONATE @`H  0޽h ? ̙33y___PPT10Y+D=' = @B + 0 "!#d(  d d 0z dMAKING SALTS - POSSIBILITIES,(2ffT d C ,Agcselogo2 d H,{_ж_ж" x v u!IS THE SALT SOLUBLE OR INSOLUBLE?"(2" !  d H ){_ж_ж" }r  {'DOES THE METAL REACT WITH DILUTE ACIDS?((2( '  d H4{_ж_ж"   _ IS IT SAFE? (2      d H9{_ж_ж"  p2 1IS THE METAL OXIDE OR CARBONATE SOLUBLE IN WATER?2(22 1 vB  d N_ж_жDff) vB  d N_ж_жDff)UvB  d N_ж_жDff)O a |B  d T_ж_жDff)'@*vB  d@ N_ж_жDff) QT vB d N_ж_жDff)' Y '@ d H`?{_ж_ж" Y   FMIX SOLUTIONS OF TWO SUITABLE SALTS TO PRECIPITATE THE INSOLUBLE SALT<G(2(  ! F 7 d H0F{_ж_ж" !Y -  =ADD EXCESS METAL TO THE ACID THEN FILTER OFF THE EXCESS METAL<>(2"  ! =  d HL{_ж_ж" 2Y  %TITRATE THE METAL HYDROXIDE WITH ACID.&(2 ! % vB d N_ж_жDff) 1 F vB d N_ж_жDff)F  vB d N_ж_жDff):x d HT{_ж_ж" , yFILTER OFF THE SALT.(2 !  vB d N_ж_жDff)>= L d H]{_ж_ж" k Y   RADD EXCESS METAL OXIDE OR METAL CARBONATE TO ACID THEN FILTER OFF THE EXCESS SOLID<S(27  ! R vB d N_ж_жDff) ={ vB d N_ж_жDff) : d HTb{_ж_ж"  ,  &CRYSTALLISE THE SALT FROM THE FILTRATE.'(2  ! &  d Hi{_ж_ж!"  ~=  ZNO (2  d Hl{_ж_ж!"    ZNO (2  d H8q{_ж_жf3" F3 _SOLUBLE (2  d HQ{_ж_ж!"  Q  ZNO (2   d Hy{_ж_ж"  Q  [YES (2  !d H|{_ж_ж"   [YES (2  "d H8{_ж_ж" x [YES (2  #d Hx{_ж_ж" *p  ] INSOLUBLE (2   H d 0޽h ? ̙33y___PPT10Y+D=' = @B +s 0 P0*(  0 0 0{ dPREPARATION OF SOLUBLE SALTS,(2ff 0 0ԓ{C"?(s JSalts can be made by NEUTRALISATION of acids; " acidic solutions contain aqueous hydrogen ions H+(aq) " sulphuric acid produces a sulphate " hydrochloric acid produces a chloride " nitric acid produces a nitrateA  f3  f3    >c O @`T 0 C ,Agcselogo2H 0 0޽h ? ̙33y___PPT10Y+D=' = @B +[  0 z (    0{C"?(s  2Salts can be made by NEUTRALISATION of acids; " acidic solutions contain aqueous hydrogen ions H+(aq) " sulphuric acid produces a sulphate " hydrochloric acid produces a chloride " nitric acid produces a nitrate Other chemicals are formed, it depends on what is neutralising the acid. OXIDES SALT + WATER HYDROXIDES SALT + WATER CARBONATES SALT + CARBON DIOXIDE + WATER METALS SALT + HYDROGEN (not all metals are suitable; some are too reactive; others are not reactive enough)*@dzI   3 f3TPc   @`T  C ,Agcselogo2  0{ dPREPARATION OF SOLUBLE SALTS,(2ffH  0޽h ? ̙33y___PPT10Y+D=' = @B + 0  b(    0{( n&PREPARATION OF SALTS BY NEUTRALISATION,'(2&ffT  C ,Agcselogo2H  0޽h ? ̙33y___PPT10Y+D=' = @B +% 0 LD !!(  vB  N_ж_жD)F    0ܒ{ FMAKING SALTS  FROM INSOLUBLE BASES,$(2#ffT  C ,Agcselogo2  HL{_ж_ж" x v u!IS THE SALT SOLUBLE OR INSOLUBLE?"(2" !   H{_ж_ж" }r  {'DOES THE METAL REACT WITH DILUTE ACIDS?((2( '   H{_ж_ж"   _ IS IT SAFE? (2       H{_ж_ж"  p2 1IS THE METAL OXIDE OR CARBONATE SOLUBLE IN WATER?2(22 1 vB  N_ж_жD) vB   N_ж_жDff)UvB   N_ж_жDff)O a |B   T_ж_жD)'@*vB  @ N_ж_жD) QT vB   N_ж_жD)' Y '@  H}_ж_ж" Y   FMIX SOLUTIONS OF TWO SUITABLE SALTS TO PRECIPITATE THE INSOLUBLE SALT<G(2(  ! F 7  H}_ж_ж" !Y -  =ADD EXCESS METAL TO THE ACID THEN FILTER OFF THE EXCESS METAL<>(2"  ! =   H }_ж_ж" 2Y  %TITRATE THE METAL HYDROXIDE WITH ACID.&(2 ! % vB  N_ж_жDff) 1 F vB  N_ж_жDff):x  H}_ж_ж" , yFILTER OFF THE SALT.(2 !  vB  N_ж_жD)>= L  Hp{_ж_ж" k Y   RADD EXCESS METAL OXIDE OR METAL CARBONATE TO ACID THEN FILTER OFF THE EXCESS SOLID<S(27  ! R vB  N_ж_жDff) ={ vB  N_ж_жD) :  H }_ж_ж"  ,  &CRYSTALLISE THE SALT FROM THE FILTRATE.'(2  ! &   H\&}_ж_ж"  ~=  ZNO (2   H*}_ж_ж!"    ZNO (2   H<}_ж_жf3" F3 _SOLUBLE (2   H(}_ж_ж!"  Q  ZNO (2   HL2}_ж_ж"  Q  [YES (2   H`6}_ж_ж"   [YES (2    H9}_ж_ж" x [YES (2  ! H=}_ж_ж" *p  ] INSOLUBLE (2   H  0޽h ? ̙33y___PPT10Y+D=' = @B + 0  P:(  P P 0HD}s p Acid with excess insoluble oxide!! @`T P C ,Agcselogo2 P 0N}( n&PREPARATION OF SALTS BY NEUTRALISATION,'(2&ffH P 0޽h ? ̙33y___PPT10Y+D=' = @B + 0  L](  L L 0O}s `XP___PPT92* {1 Place dilute acid in a beaker and warm it gently without letting it boil (reactions are faster at higher temperatures) Nzz @`P L C (Acuso41g&T.  L 0f}s p Acid with excess insoluble oxide!! @`T L C ,Agcselogo2 L 0Z}( n&PREPARATION OF SALTS BY NEUTRALISATION,'(2&ffH L 0޽h ? ̙33y___PPT10Y+D=' = @B +D 0 kc  (    0}s `XP___PPT92* 1 Place dilute acid in a beaker and warm it gently without letting it boil (reactions are faster at higher temperatures) Remove the heat Rzz @`P  C (Acuso41g&T.   0<}s p Acid with excess insoluble oxide!! @`T  C ,Agcselogo2F @ p  PH   TF0_ж_ж!" @ p B TF0_ж_ж!" @ p   0}( n&PREPARATION OF SALTS BY NEUTRALISATION,'(2&ffH  0޽h ? ̙33y___PPT10Y+D=' = @B + 0 D<  (    0x}s  `XP___PPT92* R1 Place dilute acid in a beaker and warm it gently without letting it boil (reactions are faster at higher temperatures) Remove the heat 3. Carefully and slowly add small amounts of the solid while stirring (most reactions of this type are exothermic i.e. they give off energy - the energy released would make the solution boil over) dzzF @`P  C (Acuso41g&T.   0l}s p Acid with excess insoluble oxide!! @`T  C ,Agcselogo2F @ p  PH   TF0_ж_ж!" @ p  B TF0_ж_ж!" @ p   0}( n&PREPARATION OF SALTS BY NEUTRALISATION,'(2&ffH  0޽h ? ̙33y___PPT10Y+D=' = @B + 0 P  (  P  C (Acuso44g&T. s  04}s `XP___PPT92* 1 Place dilute acid in a beaker and warm it gently without letting it boil (reactions are faster at higher temperatures) Remove the heat 3. Carefully and slowly add small amounts of the solid while stirring (most reactions of this type are exothermic i.e. they give off energy - the energy released would make the solution boil over) 4. Continue adding the solid until no more dissolves (this ensures all the acid has been used - it is easier to filter off excess solid than extract excess acid).zkz5l @`  0}s p Acid with excess insoluble oxide!! @`T  C ,Agcselogo2F @ p  PH   TF0_ж_ж!" @ p  B TF0_ж_ж!" @ p   0<}( n&PREPARATION OF SALTS BY NEUTRALISATION,'(2&ffH  0޽h ? ̙33y___PPT10Y+D=' }= @B + 0 ` (    04}s O G5. Filter the solution into an evaporating dish to remove excess solidHH @`P  C (Acuso42g>   0 }s p Acid with excess insoluble oxide!! @`T  C ,Agcselogo2  0( n&PREPARATION OF SALTS BY NEUTRALISATION,'(2&ffH  0޽h ? ̙33y___PPT10Y+D=' }= @B + 0 91 (  /  0 s ] TLD___PPT9& s5. Filter the solution into an evaporating dish to remove excess solid Transfer the dish to a tripod and carefully warm the mixture to remove some of the water. Too much heat will drive off any water of crystallisation. @II @`  0s p Acid with excess insoluble oxide!! @`P  C (Acuso43gT T  C ,Agcselogo2  0!( n&PREPARATION OF SALTS BY NEUTRALISATION,'(2&ffH  0޽h ? ̙33y___PPT10Y+D=' }= @B +@ 0 g_  (      09s d f^V___PPT980 K5. Filter the solution into an evaporating dish to remove excess solid Transfer the dish to a tripod and carefully warm the mixture to remove some of the water. Too much heat will drive off any water of crystallisation. When some of the water has been evaporated, let the solution to cool; (allows crystallisation takes place)TIlIl,R @`   07s p Acid with excess insoluble oxide!! @`P   C (Acuso43gT T   C ,Agcselogo2F @ p   P8    TF0_ж_ж!" @ p  B TF0_ж_ж!" @ p   0xD( n&PREPARATION OF SALTS BY NEUTRALISATION,'(2&ffH   0޽h ? ̙33y___PPT10Y+D=' }= @B += 0 d\ (    0Ls d f^V___PPT980 K5. Filter the solution into an evaporating dish to remove excess solid Transfer the dish to a tripod and carefully warm the mixture to remove some of the water. Too much heat will drive off any water of crystallisation. When some of the water has been evaporated, let the solution to cool; (allows crystallisation takes place)XIlIl,R @`  0@es p Acid with excess insoluble oxide!! @`  0q sRH@8___PPT9 #When sufficient crystals have appeared, filter them off, wash with a little cold water and transfer them to a filter paper. Place another filter paper over the top and press gently to help remove some of the water. @`T  C ,Agcselogo2  0t( n&PREPARATION OF SALTS BY NEUTRALISATION,'(2&ffH  0޽h ? ̙33y___PPT10Y+D=' = @B +  0 =5 T(  T T 0s d f^V___PPT980 K5. Filter the solution into an evaporating dish to remove excess solid Transfer the dish to a tripod and carefully warm the mixture to remove some of the water. Too much heat will drive off any water of crystallisation. When some of the water has been evaporated, let the solution to cool; (allows crystallisation takes place)XIlIl,R @` T 0s p Acid with excess insoluble oxide!! @` T 0p sYTLD___PPT9& ZWhen sufficient crystals have appeared, filter them off, wash with a little cold water and transfer them to a filter paper. Place another filter paper over the top and press gently to help remove some of the water. 9. Allow the crystals to dry naturally in air. (heat can cause the crystals to decompose and lose their water of crystallisation)H/S1*  @`T T C ,Agcselogo2 T 0( n&PREPARATION OF SALTS BY NEUTRALISATION,'(2&ffH T 0޽h ? ̙33y___PPT10Y+D=' = @B + 0  \s(  \ \ 0H( n&PREPARATION OF SALTS BY NEUTRALISATION,'(2&ff  \ 0ts %Acid with excess insoluble carbonate 6%%%  @`T \ C ,Agcselogo2H \ 0޽h ? ̙33y___PPT10Y+D=' = @B + 0  X(  X X 0tρ( n&PREPARATION OF SALTS BY NEUTRALISATION,'(2&ff" X 0tҁs 6Acid with excess insoluble carbonate The method used is similar to that used with acids and metal oxides. The main differences is that it is not necessary to use heat and that carbon dioxide gas is given off so you have to make sure the solution doesn t effervesce (fizz) too much. 6%%%  @`T X C ,Agcselogo2H X 0޽h ? ̙33y___PPT10Y+D=' = @B +{ 0 @  2(    0с( n&PREPARATION OF SALTS BY NEUTRALISATION,'(2&ffB  0|s 6Acid with excess insoluble carbonate The method used is similar to that used with acids and metal oxides. The main differences is that it is not necessary to use heat and that carbon dioxide gas is given off so you have to make sure the solution doesn t effervesce (fizz) too much. V%%%  @`T  C ,Agcselogo2$  0G.s H@8___PPT9  tPlace dilute acid in a beaker $ @`R  C *A carbsalt}' H  0޽h ? ̙33y___PPT10Y+D=' = @B + 0 P 4t(  4T 4 C ,Acarbsalt2}'  4 0( n&PREPARATION OF SALTS BY NEUTRALISATION,'(2&ffB 4 0h.s 6Acid with excess insoluble carbonate The method used is similar to that used with acids and metal oxides. The main differences is that it is not necessary to use heat and that carbon dioxide gas is given off so you have to make sure the solution doesn t effervesce (fizz) too much. V%%%  @`T 4 C ,Agcselogo2d 4 0'.s ZRJ___PPT9,$  8Place dilute acid in a beaker Carefully and slowly add small amounts of the solid carbonate while stirring  make sure there is not too much effervescence.8~~ @`H 4 0޽h ? ̙33y___PPT10Y+D=' = @B +  0   @ 0d (  0 0 0@( n&PREPARATION OF SALTS BY NEUTRALISATION,'(2&ff4 0 00Fs 6Acid with excess insoluble carbonate The method used is similar to that used with acids and metal oxides. The main differences is that it is not necessary to use heat and that carbon dioxide gas is given off so you have to make sure the solution doesn t effervesce (fizz) too much. H%%%  @`T 0 C ,Agcselogo2 0 0LG.s *f^V___PPT980  :Place dilute acid in a beaker Carefully and slowly add small amounts of the solid carbonate while stirring  make sure there is not too much effervescence. 3. Continue adding the solid carbonate until no more dissolves (this ensures all the acid has been used - it is easier to filter off excess solid than extract excess acid).t?l @`R 0 C *A carbsalt}' T 0 C ,Acarbsalt2}' H 0 0޽h ? ̙33y___PPT10Y+D=' = @B + 0 0  ,(  ,T  , C ,Acarbsalt3  , 0ts  H4. Filter the solution into an evaporating dish to remove excess solid II @` , 0vs t$Acid with excess insoluble carbonate%% @`T , C ,Agcselogo2 , 0_ж_ж"  p2 1IS THE METAL OXIDE OR CARBONATE SOLUBLE IN WATER?2(22 1 vB  N_ж_жD) vB   N_ж_жDff)UvB   N_ж_жDff)O a |B   T_ж_жDff)'@*vB  @ N_ж_жD) QT vB   N_ж_жDff)' Y '@  HD_ж_ж" Y   FMIX SOLUTIONS OF TWO SUITABLE SALTS TO PRECIPITATE THE INSOLUBLE SALT<G(2(  ! F 7  HK_ж_ж" !Y -  =ADD EXCESS METAL TO THE ACID THEN FILTER OFF THE EXCESS METAL<>(2"  ! =   H8R_ж_ж" 2Y  %TITRATE THE METAL HYDROXIDE WITH ACID.&(2 ! % vB  N_ж_жD) 1 F vB  N_ж_жD)F  vB  N_ж_жD):x  HN_ж_ж" , yFILTER OFF THE SALT.(2 !  vB  N_ж_жDff)>= L  HT&_ж_ж" k Y   RADD EXCESS METAL OXIDE OR METAL CARBONATE TO ACID THEN FILTER OFF THE EXCESS SOLID<S(27  ! R vB  N_ж_жD) ={ vB  N_ж_жD) :  Hd_ж_ж"  ,  &CRYSTALLISE THE SALT FROM THE FILTRATE.'(2  ! &   H`]_ж_ж"  ~=  ZNO (2   H(_ж_ж"    ZNO (2   HPq_ж_жf3" F3 _SOLUBLE (2   Hu_ж_ж"  Q  ZNO (2   Hls_ж_ж"  Q  [YES (2   H@~_ж_ж"   [YES (2    H_ж_ж" x [YES (2  ! H_ж_ж" *p  ] INSOLUBLE (2   H  0޽h ? ̙33y___PPT10Y+D=' = @B + 0  `e(  ` ` 0( n&PREPARATION OF SALTS BY NEUTRALISATION,'(2&ff ` 0s Acid with excess metal 6  @`T ` C ,Agcselogo2H ` 0޽h ? ̙33y___PPT10Y+D=' = @B +G 0 nf (    0( n&PREPARATION OF SALTS BY NEUTRALISATION,'(2&ff  0s 4Acid with excess metal The method used is similar to that used with acids and metal oxides or metal carbonates. However, because hydrogen is produced during the experiment, Bunsen burners must not be used while the chemical reaction is taking place. Not all metals are suitable: some are too reactive K, Na, Ca some don t react Cu6BBB  @`T  C ,Agcselogo2H  0޽h ? ̙33y___PPT10Y+D=' = @B +9 0 `X (  R  C *A carbsalt M   0( n&PREPARATION OF SALTS BY NEUTRALISATION,'(2&ff  0< s FAcid with excess metal The method used is similar to that used with acids and metal oxides or metal carbonates. However, because hydrogen is produced during the experiment, Bunsen burners must not be used while the chemical reaction is taking place. Not all metals are suitable: some are too reactive K, Na, Ca some don t react CuHBAB  @`T  C ,Agcselogo2$  0$ s  H@8___PPT9  tPlace dilute acid in a beaker $ @`R  C *A carbsalt M H  0޽h ? ̙33y___PPT10Y+D=' = @B +%  0 LD (  R  C *A carbsalt M   0)( n&PREPARATION OF SALTS BY NEUTRALISATION,'(2&ff  0<s TAcid with excess metal The method used is similar to that used with acids and metal oxides or metal carbonates. However, because hydrogen is produced during the experiment, Bunsen burners must not be used while the chemical reaction is taking place. Not all metals are suitable: some are too reactive K, Na, Ca some don t react CuVB\B  @`T  C ,Agcselogo2\  0I s ZRJ___PPT9,$  &Place dilute acid in a beaker Carefully and slowly add small amounts of the metal while stirring  make sure there is not too much effervescence. Btu @`H  0޽h ? ̙33y___PPT10Y+D=' = @B +  0   \ (  N  C &Aznso4g M   08M( n&PREPARATION OF SALTS BY NEUTRALISATION,'(2&ff  0 [s TAcid with excess metal The method used is similar to that used with acids and metal oxides or metal carbonates. However, because hydrogen is produced during the experiment, Bunsen burners must not be used while the chemical reaction is taking place. Not all metals are suitable: some are too reactive K, Na, Ca some don t react CuVB_B  @`T  C ,Agcselogo2  0hV s {f^V___PPT980  lPlace dilute acid in a beaker Carefully and slowly add small amounts of the metal while stirring  make sure there is not too much effervescence. 3. Continue adding the metal until no more dissolves (this ensures all the acid has been used - it is easier to filter off excess metal than extract excess acid).tuu5l @`H  0޽h ? ̙33y___PPT10Y+D=' = @B + 0 P t(  tP t C (Aznso42g  t 0Ds  H4. Filter the solution into an evaporating dish to remove excess metal II @` t 0ws fAcid with excess metal @`T t C ,Agcselogo2 t 0( n&PREPARATION OF SALTS BY NEUTRALISATION,'(2&ffH t 0޽h ? ̙33y___PPT10Y+D=' = @B + 0 6.` x(  xP x C (Aznso43gd 6 x 0ps ] TLD___PPT9& z4. Filter the solution into an evaporating dish to remove excess metal 5. Transfer the dish to a tripod and carefully warm the mixture to remove some of the water. Too much heat will drive off any water of crystallisation. DI @` x 0s fAcid with excess metal @`T x C ,Agcselogo2 x 0( n&PREPARATION OF SALTS BY NEUTRALISATION,'(2&ffH x 0޽h ? ̙33y___PPT10Y+D=' = @B + 0 p  |m(  |P  | C (Aznso43gd S | 0s d  Q4. Filter the solution into an evaporating dish to remove excess metal 5. Transfer the dish to a tripod and carefully warm the mixture to remove some of the water. Too much heat will drive off any water of crystallisation. 6. When some of the water has been evaporated, let the solution to cool; (allows crystallisation takes place)<Ro,U @` | 0s fAcid with excess metal @`T | C ,Agcselogo2 | 0%( n&PREPARATION OF SALTS BY NEUTRALISATION,'(2&ffF @ p | S  | TF0_ж_ж!" @ p  |B TF0_ж_ж!" @ pH | 0޽h ? ̙33y___PPT10Y+D=' = @B +@ 0 g_ (  3  0,s d  Q4. Filter the solution into an evaporating dish to remove excess metal 5. Transfer the dish to a tripod and carefully warm the mixture to remove some of the water. Too much heat will drive off any water of crystallisation. 6. When some of the water has been evaporated, let the solution to cool; (allows crystallisation takes place)RR,U @`  0<s fAcid with excess metal @`  0E sR $7. When sufficient crystals have appeared, filter them off, wash with a little cold water and transfer them to a filter paper. Place another filter paper over the top and press gently to help remove some of the water. @`T  C ,Agcselogo2  0hP( n&PREPARATION OF SALTS BY NEUTRALISATION,'(2&ffH  0޽h ? ̙33y___PPT10Y+D=' = @B + 0  J(  3  0Ws d  Q4. Filter the solution into an evaporating dish to remove excess metal 5. Transfer the dish to a tripod and carefully warm the mixture to remove some of the water. Too much heat will drive off any water of crystallisation. 6. When some of the water has been evaporated, let the solution to cool; (allows crystallisation takes place)RR,U @`  0es fAcid with excess metal @`  0f sY`XP___PPT92* ]7. When sufficient crystals have appeared, filter them off, wash with a little cold water and transfer them to a filter paper. Place another filter paper over the top and press gently to help remove some of the water. 8. Allow the crystals to dry naturally in air. (heat can cause the crystals to decompose and lose their water of crystallisation)d/S4*  @`T  C ,Agcselogo2  0s( n&PREPARATION OF SALTS BY NEUTRALISATION,'(2&ffH  0޽h ? ̙33y___PPT10Y+D=' = @B +5 0 \T !!(    0TH VMAKING SALTS  FROM SOLUBLE BASES (ALKALIS),,(2+ffT  C ,Agcselogo2  Hdy_ж_ж" x v u!IS THE SALT SOLUBLE OR INSOLUBLE?"(2" !   H_ж_ж" }r  {'DOES THE METAL REACT WITH DILUTE ACIDS?((2( '   H_ж_ж"   _ IS IT SAFE? (2       H_ж_ж"  p2 1IS THE METAL OXIDE OR CARBONATE SOLUBLE IN WATER?2(22 1 vB  N_ж_жD) vB   N_ж_жDff)UvB   N_ж_жDff)O a |B   T_ж_жD)'@*vB  @ N_ж_жD) QT vB   N_ж_жD)' Y '@  Hh_ж_ж" Y   FMIX SOLUTIONS OF TWO SUITABLE SALTS TO PRECIPITATE THE INSOLUBLE SALT<G(2(  ! F 7  H_ж_ж" !Y -  =ADD EXCESS METAL TO THE ACID THEN FILTER OFF THE EXCESS METAL<>(2"  ! =   H_ж_ж" 2Y  %TITRATE THE METAL HYDROXIDE WITH ACID.&(2 ! % vB  N_ж_жD) 1 F vB  N_ж_жDff)F  vB  N_ж_жD):x  H_ж_ж" , yFILTER OFF THE SALT.(2 !  vB  N_ж_жD)>= L  H_ж_ж" k Y   RADD EXCESS METAL OXIDE OR METAL CARBONATE TO ACID THEN FILTER OFF THE EXCESS SOLID<S(27  ! R vB  N_ж_жD) ={ vB  N_ж_жDff) :  H_ж_ж"  ,  &CRYSTALLISE THE SALT FROM THE FILTRATE.'(2  ! &   HD_ж_ж"  ~=  ZNO (2   H_ж_ж!"    ZNO (2   H_ж_жf3" F3 _SOLUBLE (2   H_ж_ж"  Q  ZNO (2   H8_ж_ж"  Q  [YES (2   HP_ж_ж"   [YES (2    H_ж_ж" x [YES (2  ! H_ж_ж" *p  ] INSOLUBLE (2   H  0޽h ? ̙33y___PPT10Y+D=' = @B + 0  C(    0t OALKALIS,(2ffT  C ,Agcselogo2H  0޽h ? ̙33y___PPT10Y+D=' = @B + 0 p (    0t OALKALIS,(2ffU  0 (s YDefinition ALKALIS ARE SOLUBLE BASES Their solutions contain hydroxide ions, OH(aq) HZ !I#Q @`T  C ,Agcselogo2H  0޽h ? ̙33y___PPT10Y+D=' = @B + 0 +#` (    0 OALKALIS,(2ffp  0 (s Definition ALKALIS ARE SOLUBLE BASES Their solutions contain hydroxide ions, OH(aq) STRONG ALKALIS sodium hydroxide (NaOH) potassium hydroxide (KOH) WEAK ALKALIS ammonia solution (ammonium hydroxide) (NH4OH)S'!8 ! @Q$ < @`T  C ,Agcselogo2H  0޽h ? ̙33y___PPT10Y+D=' = @B + 0 C;P (    0  OALKALIS,(2ffN  0,4(s Definition ALKALIS ARE SOLUBLE BASES Their solutions contain hydroxide ions, OH(aq) STRONG ALKALIS sodium hydroxide (NaOH) potassium hydroxide (KOH) WEAK ALKALIS ammonia solution (ammonium hydroxide) (NH4OH)S'f@Q$ < @`T  C ,Agcselogo22  0T+cs  bMaking salts using alkalis cannot be done by the methods used for insoluble bases because you cannot tell when all the acid has been neutralised  the excess alkali is soluble. ! " @`H  0޽h ? ̙33y___PPT10Y+D=' = @B + 0 @ w(    0xD OALKALIS,(2ffN  0H(s Definition ALKALIS ARE SOLUBLE BASES Their solutions contain hydroxide ions, OH(aq) STRONG ALKALIS sodium hydroxide (NaOH) potassium hydroxide (KOH) WEAK ALKALIS ammonia solution (ammonium hydroxide) (NH4OH)S'f@Q$ < @`T  C ,Agcselogo2  0Ncs] vMaking salts using alkalis cannot be done by the methods used for insoluble bases because you cannot tell when all the acid has been neutralised  the excess alkali is soluble. The salts are made by titration using an indicator ACID + ALKALINE HYDROXIDE   > NEUTRAL SALT + WATER SOLUTION SOLUTION `Y4%!3F!,  @`H  0޽h ? ̙33y___PPT10Y+D=' = @B +2  0 YQ0 (    0o OALKALIS,(2ffN  0r(s Definition ALKALIS ARE SOLUBLE BASES Their solutions contain hydroxide ions, OH(aq) STRONG ALKALIS sodium hydroxide (NaOH) potassium hydroxide (KOH) WEAK ALKALIS ammonia solution (ammonium hydroxide) (NH4OH)S'f@Q$ < @`T  C ,Agcselogo2H  0wcs &Making salts using alkalis cannot be done by the methods used for insoluble bases because you cannot tell when all the acid has been neutralised  the excess alkali is soluble. The salts are made by titration using an indicator ACID + ALKALINE HYDROXIDE   > NEUTRAL SALT + WATER SOLUTION SOLUTION The indicator tells you when the acid has been neutralisedHY;;!@ ;  @`H  0޽h ? ̙33y___PPT10Y+D=' = @B + 0 F>0,(  , , 0ԙ VAMMONIUM SALTS,(2ff , 0h(s $Ammonia is very soluble in water giving an alkaline solution which can be neutralised by acids to produce AMMONIUM SALTS e.g. AMMONIA + HYDROCHLORIC  > AMMONIUM SOLUTION ACID CHLORIDE *Nf&J x  @`T , C ,Agcselogo2H , 0޽h ? ̙33y___PPT10Y+D=' = @B +! 0 H@<(  < < 0 VAMMONIUM SALTS,(2ff < 0̱(sp  &:Ammonia is very soluble in water giving an alkaline solution which can be neutralised by acids to produce AMMONIUM SALTS e.g. AMMONIA + HYDROCHLORIC  > AMMONIUM SOLUTION ACID CHLORIDE If ammonium hydroxide is specified you can write the equation AMMONIUM + HYDROCHLORIC  > AMMONIUM + WATER HYDROXIDE ACID CHLORIDE Ammonium salts make very important fertilisers pl/?!_f/BJ x@ ]0  @`T < C ,Agcselogo2H < 0޽h ? ̙33y___PPT10Y+D=' = @B + 0 :2P(  P P 0ļ aMAKING SALTS BY TITRATION,(2ffm P 0(s This method is limited to the soluble salts of ammonia or alkali metals e.g. ammonium chloride NH4Cl sodium chloride NaCl potassium sulphate K2SO4 sodium nitrate NaNO3 !D    ,' @`T P C ,Agcselogo2H P 0޽h ? ̙33y___PPT10Y+D=' = @B + 0 ` (    0 aMAKING SALTS BY TITRATION,(2ff#  0(s"  7This method is limited to the soluble salts of ammonia or alkali metals e.g. ammonium chloride NH4Cl sodium chloride NaCl potassium sulphate K2SO4 sodium nitrate NaNO3 Method React an acid with an alkali (hydroxides of Group I metals and ammonia). The method involves TITRATION. &8ih !, @`T  C ,Agcselogo2H  0޽h ? ̙33y___PPT10Y+D=' = @B + 0 P t(    0 aMAKING SALTS BY TITRATION,(2ff  0&(s" This method is limited to the soluble salts of ammonia or alkali metals e.g. ammonium chloride NH4Cl sodium chloride NaCl potassium sulphate K2SO4 sodium nitrate NaNO3 Method React an acid with an alkali (hydroxides of Group I metals and ammonia). The method involves TITRATION. 1 Place a measured quantity of acid in a conical flask. 2 Add three or four drops of a suitable indicator. 3 Place the alkali in a burette. Note the level of the liquid. 4 Add the alkali to the acid until the indicator just changes colour Note the new level of liquid. 5 Repeat experiment with exactly the same volumes but no indicator. 6 Evaporate a small amount of the water in an evaporating basin and let the solution cool to allow crystals to form.*it;!> @`T  C ,Agcselogo2H  0޽h ? ̙33y___PPT10Y+D=' = @B + 0 @ (    0* aMAKING SALTS BY TITRATION,(2ff)  0 R(s" This method is limited to the soluble salts of ammonia or alkali metals e.g. ammonium chloride NH4Cl sodium chloride NaCl potassium sulphate K2SO4 sodium nitrate NaNO3 Method React an acid with an alkali (hydroxides of Group I metals and ammonia). The method involves TITRATION. 1 Place a measured quantity of acid in a conical flask. 2 Add three or four drops of a suitable indicator. 3 Place the alkali in a burette. Note the level of the liquid. 4 Add the alkali to the acid until the indicator just changes colour Note the new level of liquid. 5 Repeat experiment with exactly the same volumes but no indicator. 6 Evaporate a small amount of the water in an evaporating basin and let the solution cool to allow crystals to form.<it;6!m> @`T  C ,Agcselogo2H  0޽h ? ̙33y___PPT10Y+D=' = @B + 0 p (    0? aMAKING SALTS BY TITRATION,(2ff7  0x(s" This method is limited to the soluble salts of ammonia or alkali metals e.g. ammonium chloride NH4Cl sodium chloride NaCl potassium sulphate K2SO4 sodium nitrate NaNO3 Method React an acid with an alkali (hydroxides of Group I metals and ammonia). The method involves TITRATION. 1 Place a measured quantity of acid in a conical flask. 2 Add three or four drops of a suitable indicator. 3 Place the alkali in a burette. Note the level of the liquid. 4 Add the alkali to the acid until the indicator just changes colour Note the new level of liquid. 5 Repeat experiment with exactly the same volumes but no indicator. 6 Evaporate a small amount of the water in an evaporating basin and let the solution cool to allow crystals to form.Jitq@!+> @`T  C ,Agcselogo2H  0޽h ? ̙33y___PPT10Y+D=' = @B + 0  (    0b aMAKING SALTS BY TITRATION,(2ff)  0(s" This method is limited to the soluble salts of ammonia or alkali metals e.g. ammonium chloride NH4Cl sodium chloride NaCl potassium sulphate K2SO4 sodium nitrate NaNO3 Method React an acid with an alkali (hydroxides of Group I metals and ammonia). The method involves TITRATION. 1 Place a measured quantity of acid in a conical flask. 2 Add three or four drops of a suitable indicator. 3 Place the alkali in a burette. Note the level of the liquid. 4 Add the alkali to the acid until the indicator just changes colour Note the new level of liquid. 5 Repeat experiment with exactly the same volumes but no indicator. 6 Evaporate a small amount of the water in an evaporating basin and let the solution cool to allow crystals to form.<itl!> @`T  C ,Agcselogo2H  0޽h ? ̙33y___PPT10Y+D=' = @B + 0  (    0h aMAKING SALTS BY TITRATION,(2ff)  0(s" This method is limited to the soluble salts of ammonia or alkali metals e.g. ammonium chloride NH4Cl sodium chloride NaCl potassium sulphate K2SO4 sodium nitrate NaNO3 Method React an acid with an alkali (hydroxides of Group I metals and ammonia). The method involves TITRATION. 1 Place a measured quantity of acid in a conical flask. 2 Add three or four drops of a suitable indicator. 3 Place the alkali in a burette. Note the level of the liquid. 4 Add the alkali to the acid until the indicator just changes colour Note the new level of liquid. 5 Repeat experiment with exactly the same volumes but no indicator. 6 Evaporate a small amount of the water in an evaporating basin and let the solution cool to allow crystals to form.<itD!{> @`T  C ,Agcselogo2H  0޽h ? ̙33y___PPT10Y+D=' = @B + 0  (    0 aMAKING SALTS BY TITRATION,(2ff%  0(s" This method is limited to the soluble salts of ammonia or alkali metals e.g. ammonium chloride NH4Cl sodium chloride NaCl potassium sulphate K2SO4 sodium nitrate NaNO3 Method React an acid with an alkali (hydroxides of Group I metals and ammonia). The method involves TITRATION. 1 Place a measured quantity of acid in a conical flask. 2 Add three or four drops of a suitable indicator. 3 Place the alkali in a burette. Note the level of the liquid. 4 Add the alkali to the acid until the indicator just changes colour Note the new level of liquid. 5 Repeat experiment with exactly the same volumes but no indicator. 6 Evaporate a small amount of the water in an evaporating basin and let the solution cool to allow crystals to form.8ita{!> @`T  C ,Agcselogo2H  0޽h ? ̙33y___PPT10Y+D=' = @B + 0 0 P(    0l aMAKING SALTS BY TITRATION,(2ff  0 (s" This method is limited to the soluble salts of ammonia or alkali metals e.g. ammonium chloride NH4Cl sodium chloride NaCl potassium sulphate K2SO4 sodium nitrate NaNO3 Method React an acid with an alkali (hydroxides of Group I metals and ammonia). The method involves TITRATION. 1 Place a measured quantity of acid in a conical flask. 2 Add three or four drops of a suitable indicator. 3 Place the alkali in a burette. Note the level of the liquid. 4 Add the alkali to the acid until the indicator just changes colour Note the new level of liquid. 5 Repeat experiment with exactly the same volumes but no indicator. 6 Evaporate a small amount of the water in an evaporating basin and let the solution cool to allow crystals to form.iR> @`T  C ,Agcselogo2H  0޽h ? ̙33y___PPT10Y+D=' = @B +x 0L0   (      0 aMAKING SALTS BY TITRATION,(2ff   0(s  ZExample word equations:- sodium hydroxide + hydrochloric acid  > sodium chloride + water sodium hydroxide + sulphuric acid  > sodium sulphate + water potassium hydroxide + nitric acid  > potassium nitrate + water ammonium hydroxide + nitric acid  > ammonium nitrate + water &^D@|   @`T   C ,Agcselogo2H   0޽h ? ̙33y___PPT10Y+D=' = @B + 0L0  E(    0 - aMAKING SALTS BY TITRATION,(2ff  01(s  Example word equations:- sodium hydroxide + hydrochloric acid  > sodium chloride + water sodium hydroxide + sulphuric acid  > sodium sulphate + water potassium hydroxide + nitric acid  > potassium nitrate + water ammonium hydroxide + nitric acid  > ammonium nitrate + water Now complete these:- &u[@|   @`T  C ,Agcselogo2H  0޽h ? ̙33y___PPT10Y+D=' = @B +$  0L0 3 + (    0HD aMAKING SALTS BY TITRATION,(2ff  0I(s VExample word equations:- sodium hydroxide + hydrochloric acid  > sodium chloride + water sodium hydroxide + sulphuric acid  > sodium sulphate + water potassium hydroxide + nitric acid  > potassium nitrate + water ammonium hydroxide + nitric acid  > ammonium nitrate + water Now complete these:- potassium hydroxide + hydrochloric acid  > potassium chloride + water &@|   @`T  C ,Agcselogo2  n_ж_жAParchment"  `    n_ж_жAParchment"  sp   n_ж_жAParchment"  s    n_ж_жAParchment"   H  0޽h ? ̙33y___PPT10Y+D=' = @B +  0L0 P4E(  4 4 00] aMAKING SALTS BY TITRATION,(2ff 4 0Pb(s 0DExample word equations:- sodium hydroxide + hydrochloric acid  > sodium chloride + water sodium hydroxide + sulphuric acid  > sodium sulphate + water potassium hydroxide + nitric acid  > potassium nitrate + water ammonium hydroxide + nitric acid  > ammonium nitrate + water Now complete these:- potassium hydroxide + hydrochloric acid  > potassium chloride + water sodium hydroxide + nitric acid  > sodium nitrate + water f#!!aL|    @`T 4 C ,Agcselogo2 4 n_ж_жAParchment"  `  4 n_ж_жAParchment"  tqH 4 0޽h ? ̙33y___PPT10Y+D=' = @B +  0L0   @0% (  0 0 0z aMAKING SALTS BY TITRATION,(2ffp 0 0}(s  Example word equations:- sodium hydroxide + hydrochloric acid  > sodium chloride + water sodium hydroxide + sulphuric acid  > sodium sulphate + water potassium hydroxide + nitric acid  > potassium nitrate + water ammonium hydroxide + nitric acid  > ammonium nitrate + water Now complete these:- potassium hydroxide + hydrochloric acid  > potassium chloride + water sodium hydroxide + nitric acid  > sodium nitrate + water ammonium hydroxide + hydrochloric acid  > ammonium chloride + water o! !.!!T|   L @`T 0 C ,Agcselogo2 0 n_ж_жAParchment" }` } 0 n_ж_жAParchment" }}H 0 0޽h ? ̙33y___PPT10Y+D=' = @B + 0L0  (    0P aMAKING SALTS BY TITRATION,(2ff0  0؞(s  Example word equations:- sodium hydroxide + hydrochloric acid  > sodium chloride + water sodium hydroxide + sulphuric acid  > sodium sulphate + water potassium hydroxide + nitric acid  > potassium nitrate + water ammonium hydroxide + nitric acid  > ammonium nitrate + water Now complete these:- potassium hydroxide + hydrochloric acid  > potassium chloride + water sodium hydroxide + nitric acid  > sodium nitrate + water ammonium hydroxide + hydrochloric acid  > ammonium chloride + water fo7!!T|   L @`T  C ,Agcselogo2H  0޽h ? ̙33y___PPT10Y+D=' = @B + 0L0 #` t(  t t 0d gNEUTRALISATION - IONIC EQUATION, (2ffP t 0(s In all alkali  acid reactions, the same ionic reaction takes place& FFE  @`T t C ,Agcselogo2H t 0޽h ? ̙33y___PPT10Y+D=' = @B + 0L0   !(    0 gNEUTRALISATION - IONIC EQUATION, (2ff  0`(sV ^In all alkali  acid reactions, the same ionic reaction takes place& sodium hydroxide + dil. nitric acid  > sodium nitrate + water NaOH(aq) + HNO3 (aq)  > NaNO3 (aq) + H2O (l) FO! ! !  !LE 8K  @`T  C ,Agcselogo2H  0޽h ? ̙33y___PPT10Y+D=' = @B +  0L0    y (    0< gNEUTRALISATION - IONIC EQUATION, (2ff"  0(s  In all alkali  acid reactions, the same ionic reaction takes place& sodium hydroxide + dil. nitric acid  > sodium nitrate + water NaOH(aq) + HNO3 (aq)  > NaNO3 (aq) + H2O (l) Na+(aq) + OH(aq) + H+(aq) + NO3(aq)  > Na+(aq) + NO3(aq) + H2O(l) \CFO! ! !  ! !! ! !  ! ! !E 8K   @`T  C ,Agcselogo2vB @ N_ж_жDf>vB  N_ж_жDf>vB  @ N_ж_жDf> vB   N_ж_жDf>_} vB  @ N_ж_жDf> vB   N_ж_жDf>:XH  0޽h ? ̙33y___PPT10Y+D=' = @B + 0L0    u (    0x gNEUTRALISATION - IONIC EQUATION, (2ff"  0 X(sX  In all alkali  acid reactions, the same ionic reaction takes place& sodium hydroxide + dil. nitric acid  > sodium nitrate + water NaOH(aq) + HNO3 (aq)  > NaNO3 (aq) + H2O (l) Na+(aq) + OH(aq) + H+(aq) + NO3(aq)  > Na+(aq) + NO3(aq) + H2O(l) cancel ions H+(aq) + OH(aq)  > H2O(l) from from acid alkaliFO! ! ! ! !  !;E 8K    %  @`T  C ,Agcselogo2vB  N_ж_жDf>   vB  N_ж_жDf> # # vB @ N_ж_жD>vB  N_ж_жD>vB  @ N_ж_жD> vB   N_ж_жD>_} vB  @ N_ж_жD> vB   N_ж_жD>:XH  0޽h ? ̙33y___PPT10Y+D=' = @B +1 0 XP !!(    0D dMAKING SALTS - POSSIBILITIES,(2ffT  C ,Agcselogo2  H`J_ж_ж" x v u!IS THE SALT SOLUBLE OR INSOLUBLE?"(2" !   HT _ж_ж" }r  {'DOES THE METAL REACT WITH DILUTE ACIDS?((2( '   H|_ж_ж"   _ IS IT SAFE? (2       H_ж_ж"  p2 1IS THE METAL OXIDE OR CARBONATE SOLUBLE IN WATER?2(22 1 vB  N_ж_жDff) vB   N_ж_жD)U|B   T_ж_жD)O a B   Z_ж_жD)'@*|B  @ T_ж_жD) QT |B   T_ж_жD)' Y '@  H_ж_ж" Y   FMIX SOLUTIONS OF TWO SUITABLE SALTS TO PRECIPITATE THE INSOLUBLE SALT<G(2(  ! F 7  H_ж_ж" !Y -  =ADD EXCESS METAL TO THE ACID THEN FILTER OFF THE EXCESS METAL<>(2"  ! =   H _ж_ж" 2Y  %TITRATE THE METAL HYDROXIDE WITH ACID.&(2 ! % |B  T_ж_жD) 1 F |B  T_ж_жD)F  vB  N_ж_жDff):x  Hȏ_ж_ж" , yFILTER OFF THE SALT.(2 !  |B  T_ж_жD)>= L  Hܔ_ж_ж" k Y   RADD EXCESS METAL OXIDE OR METAL CARBONATE TO ACID THEN FILTER OFF THE EXCESS SOLID<S(27  ! R |B  T_ж_жD) ={ |B  T_ж_жD) :  H_ж_ж"  ,  &CRYSTALLISE THE SALT FROM THE FILTRATE.'(2  ! &   H_ж_ж"  ~=  ZNO (2   H|_ж_ж"    ZNO (2   HH_ж_ж" F3 _SOLUBLE (2   Hp_ж_ж"  Q  ZNO (2   Hd_ж_ж"  Q  [YES (2   H_ж_ж"   [YES (2    H_ж_ж" x [YES (2  ! H_ж_ж" *p  ] INSOLUBLE (2   H  0޽h ? ̙33y___PPT10Y+D=' = @B + 0 @Z(    04 fPREPARATION OF INSOLUBLE SALTS,(2ffT  C ,Agcselogo2H  0޽h ? ̙33y___PPT10Y+D=' = @B + 0  0(    0` fPREPARATION OF INSOLUBLE SALTS,(2ff9  0"`(s oMETHOD Insoluble salts can be made by mixing appropriate solutions of ions so that a precipitate is formed. *p!j @`T  C ,Agcselogo2H  0޽h ? ̙33y___PPT10Y+D=' = @B + 0 /' Rh(  h h 0( fPREPARATION OF INSOLUBLE SALTS,(2ff] h 0L"`(s 1METHOD Insoluble salts can be made by mixing appropriate solutions of ions so that a precipitate is formed. EXAMPLES silver chloride silver nitrate and sodium chloride barium sulphate barium chloride and sodium sulphate lead iodide lead nitrate and potassium iodideX2!j!,&< @`T h C ,Agcselogo2H h 0޽h ? ̙33y___PPT10Y+D=' = @B + 0 `r(    0D fPREPARATION OF INSOLUBLE SALTS,(2ff  0"`(s 2METHOD Insoluble salts can be made by mixing appropriate solutions of ions so that a precipitate is formed. PREPARATION OF SILVER CHLORIDE To make silver chloride you need& (i) a soluble silver salt silver nitrate plus (ii) a soluble chloride sodium chloride.p H!i f.!! ff  @`T  C ,Agcselogo2H  0޽h ? ̙33y___PPT10Y+D=' = @B +h  0   0Nl (  l l 0 fPREPARATION OF INSOLUBLE SALTS,(2ff l 0 -"`(s 0METHOD Insoluble salts can be made by mixing appropriate solutions of ions so that a precipitate is formed. PREPARATION OF SILVER CHLORIDE To make silver chloride you need& (i) a soluble silver salt silver nitrate plus (ii) a soluble chloride sodium chloride.pHofT0  @`T l C ,Agcselogo2F  D l : j xB  l H_ж_жDo DxB  l H_ж_жDo@@xB  l H_ж_жDo @pB l H_ж_жDf3) l N_ж_жk"  a J l C "A  cl-g` N l C &A na+pptfg J l C "A  cl-g a N l C &A na+ppt` J l C "A  cl-g  N l C &A na+ppt  |B Kl TZ_ж_жD!)   Ml 04"` &Prepare a solution of sodium chloride.''&  @` Nl 0="`D` k1!  @`H l 0޽h ? ̙33y___PPT10Y+D=' = @B +  0 &   (    0I fPREPARATION OF INSOLUBLE SALTS,(2ff  0 M"`(s 0METHOD Insoluble salts can be made by mixing appropriate solutions of ions so that a precipitate is formed. PREPARATION OF SILVER CHLORIDE To make silver chloride you need& (i) a soluble silver salt silver nitrate plus (ii) a soluble chloride sodium chloride.pHofT0  @`T  C ,Agcselogo2F  D  : j xB  H_ж_жDo DxB  H_ж_жDo@@xB  H_ж_жDo @pB   H_ж_жDf3)   N_ж_жk"  a J  C "A  cl-g# 6 N  C &A na+ppto y' J  C "A  cl-g  N  C &A na+ppt 85 J  C "A  cl-gj l# N  C &A na+ppt#    0m"`z AThe sodium chloride lattice breaks up and dissolves in the water.BBA  @`  0`o"`D` k2!  @`H  0޽h ? ̙33y___PPT10Y+D=' = @B +) 0 PH"R(    N_ж_жk"     0z fPREPARATION OF INSOLUBLE SALTS,(2ff  0"`(s 0METHOD Insoluble salts can be made by mixing appropriate solutions of ions so that a precipitate is formed. PREPARATION OF SILVER CHLORIDE To make silver chloride you need& (i) a soluble silver salt silver nitrate plus (ii) a soluble chloride sodium chloride.pHofT0  @`T  C ,Agcselogo2F  D  : j xB   H_ж_жDo DxB   H_ж_жDo@@xB   H_ж_жDo @F  D   >  xB   H_ж_жDo DxB  H_ж_жDo@@xB  H_ж_жDo @pB  H_ж_жDf3)  N_ж_жk"  a J  C "A ag+gZC L  C $A  no3-g`D J  C "A ag+gD L  C $A  no3-g kC L   C $A  no3-g`J ! C "A ag+gk J " C "A  cl-g# 6 N # C &A na+ppto y' J $ C "A  cl-g  N % C &A na+ppt 85 J & C "A  cl-gj l# N ' C &A na+ppt#  |B L TZ_ж_жD!)  pB M H_ж_жDf3)J N C "A  cl-g# 6 J O C "A  cl-g  N P C &A na+ppt#   Q 0"` %Prepare a solution of silver nitrate.&&%  @` R 0"`D` k3!  @`H  0޽h ? ̙33y___PPT10Y+D=' = @B +> 0 e].(    N_ж_жk"     0 fPREPARATION OF INSOLUBLE SALTS,(2ff  0"`(s 0METHOD Insoluble salts can be made by mixing appropriate solutions of ions so that a precipitate is formed. PREPARATION OF SILVER CHLORIDE To make silver chloride you need& (i) a soluble silver salt silver nitrate plus (ii) a soluble chloride sodium chloride.pHofT0  @`T  C ,Agcselogo2F  D  : j xB  H_ж_жDo DxB  H_ж_жDo@@xB   H_ж_жDo @F  D   >  xB   H_ж_жDo DxB   H_ж_жDo@@xB   H_ж_жDo @pB  H_ж_жDf3)  N_ж_жk"  a J  C "A  cl-g# 6 N  C &A na+ppto y' J  C "A  cl-g  N  C &A na+ppt 85 J   C "A  cl-gj l# N ! C &A na+ppt#  J " C "A ag+g c L # C $A  no3-g9  J $ C "A ag+g  @ L % C $A  no3-g@  L & C $A  no3-g9 9 J ' C "A ag+g ?t pB + H_ж_жDf3)pB , H_ж_жDf3) - 0 "` @The silver nitrate lattice breaks up and dissolves in the water.AA@  @` . 0"`D` k4!  @`H  0޽h ? ̙33y___PPT10Y+D=' = @B +~ 0 "05(    N_ж_жk"     0 fPREPARATION OF INSOLUBLE SALTS,(2ff  0 "`(s 0METHOD Insoluble salts can be made by mixing appropriate solutions of ions so that a precipitate is formed. PREPARATION OF SILVER CHLORIDE To make silver chloride you need& (i) a soluble silver salt silver nitrate plus (ii) a soluble chloride sodium chloride.pHofT0  @`T  C ,Agcselogo2F  D  : j xB  H_ж_жDo DxB   H_ж_жDo@@xB   H_ж_жDo @F  D   >  xB   H_ж_жDo DxB   H_ж_жDo@@xB  H_ж_жDo @pB  H_ж_жDf3)F  D  " 9  xB  H_ж_жDo DxB  H_ж_жDo@@xB  H_ж_жDo @  N_ж_жk"  a J  C "A  cl-g# 6 N  C &A na+ppto y' J  C "A  cl-g  N  C &A na+ppt 85 J  C "A  cl-gj l# N  C &A na+ppt#  J  C "A ag+g c L  C $A  no3-g9  J  C "A ag+g  @ L  C $A  no3-g@  L  C $A  no3-g9 9 J   C "A ag+g ?t |B -@ TZ_ж_жD!) 3   / 0"` |Mix the two solutions.  @` 0 0"`D` k5!  @`H  0޽h ? ̙33y___PPT10Y+D=' = @B + 0   .8(    N_ж_жk" : 9    0`" fPREPARATION OF INSOLUBLE SALTS,(2ff  0'"`(s 0METHOD Insoluble salts can be made by mixing appropriate solutions of ions so that a precipitate is formed. PREPARATION OF SILVER CHLORIDE To make silver chloride you need& (i) a soluble silver salt silver nitrate plus (ii) a soluble chloride sodium chloride.pHofT0  @`T  C ,Agcselogo2F  D  : j xB  H_ж_жDo DxB   H_ж_жDo@@xB   H_ж_жDo @F  D   >  xB   H_ж_жDo DxB   H_ж_жDo@@xB  H_ж_жDo @pB  H_ж_жDf3)F  D  " 9  xB  H_ж_жDo DxB  H_ж_жDo@@xB  H_ж_жDo @J ! C "A ag+g4  J " C "A  cl-gB  N # C &A na+ppt R L $ C $A  no3-g | J % C "A  cl-g q N & C &A na+ppt  J ' C "A  cl-g R9 N ( C &A na+ppt { 9 J ) C "A ag+g H L * C $A  no3-g  L + C $A  no3-g_ p H J , C "A ag+g0 a   - 0K"` %All four ions are now mixed together.&&%  @` . 0M"`D` k6!  @`H  0޽h ? ̙33y___PPT10Y+D=' = @B + 0 4PI(    N_ж_жk" : 9    N_ж_жk" : {   0Y fPREPARATION OF INSOLUBLE SALTS,(2ff  0^"`(s 0METHOD Insoluble salts can be made by mixing appropriate solutions of ions so that a precipitate is formed. PREPARATION OF SILVER CHLORIDE To make silver chloride you need& (i) a soluble silver salt silver nitrate plus (ii) a soluble chloride sodium chloride.pHofT0  @`T  C ,Agcselogo2F  D  : j xB   H_ж_жDo DxB   H_ж_жDo@@xB   H_ж_жDo @F  D   >  xB   H_ж_жDo DxB  H_ж_жDo@@xB  H_ж_жDo @pB  H_ж_жDf3)F  D  " 9  xB  H_ж_жDo DxB  H_ж_жDo@@xB  H_ж_жDo @J . C "A ag+g4  J / C "A  cl-gB  N 0 C &A na+ppt R L 1 C $A  no3-g | J 2 C "A  cl-g q N 3 C &A na+ppt  J 4 C "A  cl-g R9 N 5 C &A na+ppt { 9 J 6 C "A ag+g H L 7 C $A  no3-g  L 8 C $A  no3-g_ p H J 9 C "A ag+g0 a  ~ : H_ж_ж" o  J ; C "A ag+g, K L < C $A  no3-gV sK J = C "A ag+gw % L > C $A  no3-gF # L ? C $A  no3-g~  J @ C "A ag+g1 . J A C "A  cl-gs V, N B C &A na+ppt  J C C "A  cl-g #< N D C &A na+pptV A J E C "A  cl-g#  N F C &A na+ppt v$4 F  D G   xB H H_ж_жDo DxB I H_ж_жDo@@xB J H_ж_жDo @|B M@ TZ_ж_жD!)1 1 pB N H_ж_жDf3)@ O 08"`? lThe silver ions and chloride ions come together and the insoluble silver chloride forms a white precipitate.mml  @` P 0Ċ"`D` k7!  @`H  0޽h ? ̙33y___PPT10Y+D=' = @B + 0 P44^(    N_ж_жk" : 9    N_ж_жk" : {   0( fPREPARATION OF INSOLUBLE SALTS,(2ff  0"`(s 0METHOD Insoluble salts can be made by mixing appropriate solutions of ions so that a precipitate is formed. PREPARATION OF SILVER CHLORIDE To make silver chloride you need& (i) a soluble silver salt silver nitrate plus (ii) a soluble chloride sodium chloride.pHofT0  @`T  C ,Agcselogo2F  D  : j xB  H_ж_жDo DxB   H_ж_жDo@@xB   H_ж_жDo @F  D   >  xB   H_ж_жDo DxB   H_ж_жDo@@xB  H_ж_жDo @pB  H_ж_жDf3)F  D  " 9  xB  H_ж_жDo DxB  H_ж_жDo@@xB  H_ж_жDo @J  C "A ag+g4  J  C "A  cl-gB  N  C &A na+ppt R L  C $A  no3-g | J  C "A  cl-g q N  C &A na+ppt  J  C "A  cl-g R9 N  C &A na+ppt { 9 J  C "A ag+g H L  C $A  no3-g  L  C $A  no3-g_ p H J  C "A ag+g0 a  ~   H_ж_ж" o  J ! C "A ag+g, K L " C $A  no3-gV sK J # C "A ag+gw % L $ C $A  no3-gF # L % C $A  no3-g~  J & C "A ag+g1 . J ' C "A  cl-gs V, N ( C &A na+ppt  J ) C "A  cl-g #< N * C &A na+pptV A J + C "A  cl-g#  N , C &A na+ppt v$4 F  D -   xB . H_ж_жDo DxB / H_ж_жDo@@xB 0 H_ж_жDo @|B 1@ TZ_ж_жD!)1 1 pB 2 H_ж_жDf3)Q 3 0"`? }Because sodium nitrate is soluble in water their ions remain in solution. The precipitate is then filtered, washed and dried.~~}  @` 4 0"`D` k7!  @`H  0޽h ? ̙33y___PPT10Y+D=' = @B +m" 0 !!NO$!(    N_ж_жk"     N_ж_жk" : 9    N_ж_жk" : {   0p fPREPARATION OF INSOLUBLE SALTS,(2ff  0"`(s 0METHOD Insoluble salts can be made by mixing appropriate solutions of ions so that a precipitate is formed. PREPARATION OF SILVER CHLORIDE To make silver chloride you need& (i) a soluble silver salt silver nitrate plus (ii) a soluble chloride sodium chloride.pHofT0  @`T  C ,Agcselogo2F  D  : j xB   H_ж_жDo DxB   H_ж_жDo@@xB   H_ж_жDo @F  D   >  xB   H_ж_жDo DxB  H_ж_жDo@@xB  H_ж_жDo @pB  H_ж_жDf3)F  D  " 9  xB  H_ж_жDo DxB  H_ж_жDo@@xB  H_ж_жDo @  N_ж_жk"  a J  C "A ag+gZC J  C "A  cl-g` N  C &A na+pptfg L  C $A  no3-g`D J  C "A  cl-g a N  C &A na+ppt` J  C "A  cl-g  N  C &A na+ppt  J  C "A ag+gD L  C $A  no3-g kC L   C $A  no3-g`J ! C "A ag+gk J " C "A  cl-g# 6 N # C &A na+ppto y' J $ C "A  cl-g  N % C &A na+ppt 85 J & C "A  cl-gj l# N ' C &A na+ppt#  J ( C "A ag+g c L ) C $A  no3-g9  J * C "A ag+g  @ L + C $A  no3-g@  L , C $A  no3-g9 9 J - C "A ag+g ?t J . C "A ag+g4  J / C "A  cl-gB  N 0 C &A na+ppt R L 1 C $A  no3-g | J 2 C "A  cl-g q N 3 C &A na+ppt  J 4 C "A  cl-g R9 N 5 C &A na+ppt { 9 J 6 C "A ag+g H L 7 C $A  no3-g  L 8 C $A  no3-g_ p H J 9 C "A ag+g0 a  ~ : H_ж_ж" o  J ; C "A ag+g, K L < C $A  no3-gV sK J = C "A ag+gw % L > C $A  no3-gF # L ? C $A  no3-g~  J @ C "A ag+g1 . J A C "A  cl-gs V, N B C &A na+ppt  J C C "A  cl-g #< N D C &A na+pptV A J E C "A  cl-g#  N F C &A na+ppt v$4 F  D G   xB H H_ж_жDo DxB I H_ж_жDo@@xB J H_ж_жDo @|B K TZ_ж_жD!)  |B L TZ_ж_жD!)  |B M@ TZ_ж_жD!)1 1 |B O@ TZ_ж_жD!) 3  H  0޽h ? ̙33y___PPT10Y+D=' = @B + 0 `8M(  8 8 0 YSALTS - QUESTIONS,(2ffT 8 C ,Agcselogo2H 8 0޽h ? ̙33y___PPT10Y+D=' = @B + 0 p8(  8 8 0 YSALTS - QUESTIONS,(2ffC 8 0,(sf S1. Work out what you get if the following chemicals are mixed. a) zinc and sulphuric acid b) copper carbonate and nitric acid c) sodium hydroxide and hydrochloric acid d) lead oxide and nitric acid e) magnesium and hydrochloric acid f) ammonium hydroxide and sulphuric acid g) magnesium carbonate and sulphuric acid TT>N  #  @`T 8 C ,Agcselogo2H 8 0޽h ? ̙33y___PPT10Y+D=' = @B + 0  (Z(  ( ( 0% YSALTS - QUESTIONS,(2ffY ( 0LD(s  31. Work out what you get if the following chemicals are mixed. a) zinc and sulphuric acid zinc sulphate + hydrogen b) copper carbonate and nitric acid copper nitrate + carbon dioxide + water c) sodium hydroxide and hydrochloric acid sodium chloride + water d) lead oxide and nitric acid lead nitrate + water e) magnesium and hydrochloric acid magnesium chloride + hydrogen f) ammonium hydroxide and sulphuric acid ammonium sulphate + water g) magnesium carbonate and sulphuric acid magnesium + carbon + water sulphate dioxide 4_ff&(ff+ff!ff%ff+ff+?fftN  4 % - @`T ( C ,Agcselogo2 ( n_ж_жAParchment" ( ( @ p H ( 0޽h ? ̙33y___PPT10Y+D=' = @B +  0 ;3 (      0@: YSALTS - QUESTIONS,(2ff   0a(s8 j1. Work out what you get if the following chemicals are mixed. a) zinc and sulphuric acid zinc sulphate + hydrogen b) copper carbonate and nitric acid copper nitrate + carbon dioxide + water c) sodium hydroxide and hydrochloric acid sodium chloride + water d) lead oxide and nitric acid lead nitrate + water e) magnesium and hydrochloric acid magnesium chloride + hydrogen f) ammonium hydroxide and sulphuric acid ammonium sulphate + water g) magnesium carbonate and sulphuric acid magnesium + carbon + water sulphate dioxide 2. Answer the following... Which ion is found in (i) acidic solutions; H+(aq) (ii) alkaline solutions? What is formed when you mix these two ions together? What name do we give to this type of reaction? When making salts from metals, oxides and carbonates, how do you know when all the acid is used up? When making salts from soluble Group I hydroxides, what do you use to check when all the acid is used up? 4M!!! '!!m!N  4 % -^a @`T   C ,Agcselogo2   n_ж_жAParchment" ( ( @ p H   0޽h ? ̙33y___PPT10Y+D=' = @B +  0   $(  $ $ 0W YSALTS - QUESTIONS,(2ffE $ 0p(s8 /1. Work out what you get if the following chemicals are mixed. a) zinc and sulphuric acid zinc sulphate + hydrogen b) copper carbonate and nitric acid copper nitrate + carbon dioxide + water c) sodium hydroxide and hydrochloric acid sodium chloride + water d) lead oxide and nitric acid lead nitrate + water e) magnesium and hydrochloric acid magnesium chloride + hydrogen f) ammonium hydroxide and sulphuric acid ammonium sulphate + water g) magnesium carbonate and sulphuric acid magnesium + carbon + water sulphate dioxide 2. Answer the following... Which ion is found in (i) acidic solutions; H+(aq) (ii) alkaline solutions? OH(aq) What is formed when you mix these two ions together? WATER What name do we give to this type of reaction? NEUTRALISATION When making salts from metals, oxides and carbonates, how do you know when all the acid is used up? WHEN THE SOLID NO LONGER DISSOLVES When making salts from soluble Group I hydroxides, what do you use to check when all the acid is used up? 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