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"%!%&%  $ #  U  $ $ $ b$Q x+k,b$,rO oCt02,$$$$b$bpe# zt O_R$FE-Qڛb>"d$$$b$UkTo)? &h 7kb$->/Y6Ʃ:7< vb$= ~:|.PdF# b$-#9_$ \b$I01?" dd@,|?" dd@   " @ ` n?" dd@   @@``PR    @ ` ` p>>L0 VN (    6 P  T Click to edit Master title style! !  0$   RClick to edit Master text styles Second level Third level Fourth level Fifth level!     S  0 ``  X*  0P `   Z*  0L `   Z*z  bA޽h @ ?Parchment ̙33 Default Design 0 zr@ ( )   0d P    P*    0xi     R*  d  c $ ?    0l  @  RClick to edit Master text styles Second level Third level Fourth level Fifth level!     S  6 `P   P*    6q `   R*  H  0޽h ? ̙3380___PPT10.0. 0X(   $+ X X 0`S P    X*  X 0     Z*  X 6 `P   X*  X 6 `   Z* H X 0޽h ? ̙3380___PPT10.0. 0L0 P +( AT葠   0  3INDICATORS & pH CURVES A guide for A level studentsD4(26f6ff   0"`>B 2008 SPECIFICATIONS>G$G   J   C "A KTRE 8  h   0(x m OKNOCKHARDY PUBLISHING(2 fB  s *޽h ? ̙33 0L0 KC(    0`e Z Indicators4 8_2 (f<fdB  <D)@0A  0Pp@ 0 0dB @ <D)@X@  0X0@ 0 0S  0Tf(0P  INTRODUCTION This Powerpoint show is one of several produced to help students understand selected topics at AS and A2 level Chemistry. It is based on the requirements of the AQA and OCR specifications but is suitable for other examination boards. Individual students may use the material at home for revision purposes or it may be used for classroom teaching if an interactive white board is available. Accompanying notes on this, and the full range of AS and A2 topics, are available from the KNOCKHARDY SCIENCE WEBSITE at... www.knockhardy.org.uk/sci.htm Navigation is achieved by... either clicking on the grey arrows at the foot of each page or using the left and right arrow keys on the keyboard (2 2(2 2  75, dB  <D?  B  s *޽h ? ̙33  0L0   `K ( w    0lp~  KCONTENTS Acid-base indicators - theory Titration curves - introduction Titration curve; strong acid - strong base Titration curve; strong acid - weak base Titration curve; weak acid - strong base Titration curve; weak acid - weak base Titration curve; acid - carbonate Titration curve; phosphoric acid Check listD (2C`2C  0pe Z Indicators4 8_2 (f<fdB  <D)@0A  0Pp@ 0 0dB @ <D)@X@  0X0@ 0 0  6X n@ 0 0   60a@ 0 0   68\@ 0 0   60W @ 0 0   6  Q @ 0 0   6  M @ 0 0  6  O @ 0 0  6 N @ 0 0  6Z a@ 0 0B  s *޽h ? ̙33g  0L0   p!h (  h h 0P NAcid-base indicators(2f1 h 6d̙ ?y General Many indicators are weak acids and partially dissociate in aqueous solution HIn(aq) H+(aq) + In(aq) The un-ionised form (HIn) is a different colour to the anionic form (In). hV@)@N@P2@Of ffff-pV    6 FF  j h n tT @  h#  *B  h TDV?@@B  h TDV?@tT @  h# F jB  h TDV?@@B h TDV?@dB h <D)@0A h 0Pp@ 0 0dB  h@ <D)@X@ !h 0X0@ 0 0B h s *޽h ? ̙33 0L0 80(    0 NAcid-base indicators(2f  6̙ ?yd  >General Many indicators are weak acids and partially dissociate in aqueous solution HIn(aq) H+(aq) + In(aq) The un-ionised form (HIn) is a different colour to the anionic form (In). Apply Le Chatelier s Principle to predict any colour change In acid - increase of [H+] - equilibrium moves to the left to give red undissociated form In alkali - increase of [OH] - OH ions remove H+ ions to form water; H+(aq) + OH(aq) H2O(l) - equilibrium will move to the right to produce a blue colourhV@)@N@P2?@_@@Of ffff-;f ,4 ff fff3 V    @   s   T     ? FF  j  n tT @ #  *B  TDV?@@B   TDV?@tT @  # F jB   TDV?@@B   TDV?@FF  j    < tT @ #  *B  TDfV?@@B  TDfV?@tT @ # F jB  TDfV?@@B  TDfV?@dB  <D)@0A  0Pp@ 0 0dB @ <D)@X@  0X0@ 0 0B  s *޽h ? ̙33 0L0 H( w   0 NAcid-base indicators(2f  6̙ ?y  General Many indicators are weak acids and partially dissociate in aqueous solution HIn(aq) H+(aq) + In(aq) The un-ionised form (HIn) is a different colour to the anionic form (In). Apply Le Chatelier s Principle to predict any colour change In acid - increase of [H+] - equilibrium moves to the left to give red undissociated form In alkali - increase of [OH] - OH ions remove H+ ions to form water; H+(aq) + OH(aq) H2O(l) - equilibrium will move to the right to produce a blue colour Summary In acidic solution HIn(aq) H+(aq) + In(aq) In alkaline solutionV@)@N@P2?@_@@*@XF>HOf ffff-;f ,4 ff fff3   ffff .V    @   s   T     j   |B @ TDԔ? m   B,B̙ ?(R  Ff FF  j  n tT @ #  *B  TDV?@@B   TDV?@tT @  # F jB   TDV?@@B   TDV?@FF  j    < tT @ #  *B  TDfV?@@B  TDfV?@tT @ # F jB  TDfV?@@B  TDfV?@FF  j   F j XtT @ #  *B  TDV?@@B  TDV?@tT @ # F jB  TDV?@@B  TDV?@|B  TDԔ?} " dB  <D)@0A  0Pp@ 0 0dB @ <D)@X@  0X0@ 0 0B  s *޽h ? ̙33= 0L0 +=#=MT<(    6TO̙ ?*! t(COLOUR CHANGES OF SOME COMMON INDICATORS)H) ) (  6hT̙ ?y0   Must have an easily observed colour change. Must change immediately in the required pH range over the addition of  half a drop of reagent.t-@c@  I    0_ NAcid-base indicators(2f   Nc̙ 1? 2P  F(2    N$h̙ 1? Pm  F(2   Nhk̙ 1? m  F(2   Nn̙ 1?  F(2   Nr̙ 1?  F(2   Nu̙ 1?  F(2   Nxy̙ 1?   F(2   N$}̙ 1?   F(2   N̙ 1? :  F(2   N̙ 1? :X  F(2   N̙ 1? Xu  F(2   N̙ 1? u  F(2   N̙ 1?   F(2   Nl̙ 1?   F(2   N̙ 1? 2  GPHENOLPHTHALEIN(2  N|̙ 1? 2  >LITMUS(2  Np̙ 1?L2  E METHYL ORANGE(2  N$̙ 1?2PN 91(2  N̙ 1?PmN 92(2  N觚̙ 1?m N 93(2   N ̙ 1? N 94(2 ! Na̙ 1? N 95(2 " N̙ 1? N 96(2 # N0̙ 1? N 97(2 $ N̻̙ 1?N 98(2 % N会̙ 1?:N 99(2 & NDš̙ 1?:XN :10(2 ' Np̙ 1?XuN :11(2 ( Nɚ̙ 1?uN :12(2 ) N\͚̙ 1?N :13(2 * N̙̚ 1?N :14(2 + N̙֚ 1?L2P  F(2  , N$̙ۚ 1?LPm  F(2  - Ndޚ̙ 1?Lm   F(2  . N̙ 1?L   F(2  / Nt̙ 1?L   F(2  0 N<̙ 1?L   F(2  1 N|̙ 1?L   F(2  2 Nx̙ 1?L  F(2  3 N̙ 1?L:  F(2  4 N̙ 1?L:X  F(2  5 NDp̙ 1?LXu  F(2  6 Np̙ 1?Lu  F(2  7 Np̙ 1?L  F(2  8 N4 p̙ 1?L  F(2  9 N̙ 1? 2P  F(2  : Np̙ 1? Pm  F(2  ; Np̙ 1? m  F(2  < NPp̙ 1?  F(2  = Np̙ 1?  F(2  > N p̙ 1?  F(2  ? Nt"p̙ 1?   F(2  @ NT&p̙ 1?   F(2  A N*p̙ 1? :  F(2  B Nh-p̙ 1? :X  F(2  C N0p̙ 1? Xu  F(2  D N4p̙ 1? u  F(2  E N7p̙ 1?   F(2  F N$;p̙ 1?   F(2  G T<>p3f1?   J (23f  H T@Gp1? 2g  J (2  I TIpff1? g   PCHANGE.(2 J TRpf1?TX   J (23f  K TUp1?T2   J (2  L TXp1?T X   PCHANGE.(2 M T4^p31?   J (23f  N TDbp1? 9  J (23f  O Tgp1?   PCHANGE.(2 P 6D̙ ?x)L DpH& 2dB Q <D)@0A R 0Pp@ 0 0dB S@ <D)@X@ T 0X0@ 0 0B  s *޽h ? ̙33  0L0 | t  (     6sp̙ ?7@ = pTo be useful, an indicator must change over the  vertical section of the curve where there is a large change in pH for the addition of a very small volume of alkali. The indicator used depends on the pH changes around the end point - the indicator must change during the  vertical portion of the curve. In the example, the only suitable indicator is PHENOLPHTHALEIN.Zt@'? t (  6p̙ ?y0   Must have an easily observed colour change. Must change immediately in the required pH range over the addition of  half a drop of reagent.t-@c@  I    0tp NAcid-base indicators(2fP  C (Aphwasbgp  d   <f??h h P   C (Aphaxesg7 d  <? r  d   <?C p     6cp̙ ?HI  &PHENOLPHTHALEIN LITMUS METHYL ORANGER 20P2020P2&dB  <D)@0A  0Pp@ 0 0dB @ <D)@X@  0X0@ 0 0B  s *޽h ? ̙33  0L0   3 (    0p C pH curves (2 f(  6p̙ ?y  DTypes There are four types of acid-base titration; each has a characteristic curve. strong acid (HCl) v. strong base (NaOH) weak acid (CH3COOH) v. strong alkali (NaOH) strong acid (HCl) v. weak base (NH3) weak acid (CH3COOH) v. weak base (NH3) In the following examples, alkali (0.1M) is added to 25cm3 of acid (0.1M) End points need not be  neutral due to the phenomenon of salt hydrolysis@HT fffffff fff f9 Ztc    /     dB   <D)@0A   0Pp@ 0 0dB @ <D)@X@  0X0@ 0 0B  s *޽h ? ̙335 0L0  c( S P  C (Aphaxesg P  C (A phsasbgB S  0x 'strong acid (HCl) v. strong base (NaOH)|((2 fff, dB  <D)@0A  0Pp@ 0 0dB @ <D)@X@   0X0@ 0 0B  s *޽h ? ̙33 0L0 0 ( w P  C (Aphaxesg P  C (A phsasbgB F  6x̙ ?   :pH 1 at the start due to 0.1M HCl (strong monoprotic acid)B;H @       S  0x 'strong acid (HCl) v. strong base (NaOH)|((2 fff, dB   <D)@0A   0Pp@ 0 0dB  @ <D)@X@   0X0@ 0 0B  s *޽h ? ̙33 0L0 )! ( w P  C (Aphaxesg P  C (A phsasbgB   64x̙ ? 4   .Very little pH change during the initial 20cm3B/H- / F  6|#x̙ ?   :pH 1 at the start due to 0.1M HCl (strong monoprotic acid)B;H @       S  0+x 'strong acid (HCl) v. strong base (NaOH)|((2 fff, dB   <D)@0A   0Pp@ 0 0dB  @ <D)@X@   0X0@ 0 0B  s *޽h ? ̙33 0L0 OG@ ( IFy P  C (Aphaxesg P  C (A phsasbgB    68x̙ ? 4   .Very little pH change during the initial 20cm3F/H- /   6d>x̙ ?4 , JVery sharp change in pH over the addition of less than half a drop of NaOH KHK&F   F  6Cx̙ ?   :pH 1 at the start due to 0.1M HCl (strong monoprotic acid)B;H @       S  0Jx 'strong acid (HCl) v. strong base (NaOH)|((2 fff, dB   <D)@0A   0Pp@ 0 0dB  @ <D)@X@   0X0@ 0 0B  s *޽h ? ̙33  0L0 j b P  (  P  C (Aphaxesg P   C (A phsasbgB     6Xx̙ ? 4   .Very little pH change during the initial 20cm3F/H- /    6^x̙ ?4 , JVery sharp change in pH over the addition of less than half a drop of NaOH KHK&F      6cx̙ ?D0 CCurve levels off at pH 13 due to excess 0.1M NaOH (a strong alkali) DHD&-   S  0ix 'strong acid (HCl) v. strong base (NaOH)|((2 fff, dB  <D)@0A  0Pp@ 0 0dB @ <D)@X@  0X0@ 0 0F  6ltx̙ ?   :pH 1 at the start due to 0.1M HCl (strong monoprotic acid)B;H @       B  s *޽h ? ̙33 0L0 KC ( w d  <?`Hd  <f? `d  <?h ` P  C (Aphaxesg S  0x 'strong acid (HCl) v. strong base (NaOH)|((2 fff, h  60x̙ ? Any of the indicators listed will be suitable - they all change in the  vertical portion ZHZf Z   6x̙ ?<  \&PHENOLPHTHALEIN LITMUS METHYL ORANGE' 2'P  C (A phsasbg: dB  <D)@0A  0Pp@ 0 0dB @ <D)@X@  0X0@ 0 0B  s *޽h ? ̙33  0L0 A 9 ` ( w P  C (Aphaxesg P  C (A phsawbghK    6H̙ ? 4 2  .Very little pH change during the initial 20cm3F/H- /    6$x̙ ?\ ,8  DSharp change in pH over the addition of less than half a drop of NH3FEHCf E   6Lx̙ ? @Curve levels off at pH 10 due to excess 0.1M NH3 (a weak alkali)FAH/ A   6x̙ ? h  !pH 1 at the start due to 0.1M HCl0"H &   `  0x $strong acid (HCl) v. weak base (NH3)%(2 f f f dB  <D)@0A  0Pp@ 0 0dB @ <D)@X@  0X0@ 0 0B  s *޽h ? ̙33 0L0 f^ (  d  <?`Hd  <f? `d  <?h ` P  C (Aphaxesg   6x̙ ?<  n&PHENOLPHTHALEIN LITMUS METHYL ORANGE,' 2P  C (A phsawbghK `   0$x $strong acid (HCl) v. weak base (NH3)%(2 f f f d   6x̙ ? Only methyl orange is suitable - it is the only one to change in the  vertical portion XHXf X dB   <D)@0A   0Pp@ 0 0dB @ <D)@X@  0X0@ 0 0B  s *޽h ? ̙33\  0L0  $( w P  C (Aphaxesg P   C (Aphwasbgh   6x̙ ?4 l `Steady pH change H    6x̙ ?S ,/ ESharp change in pH over the addition of less than half a drop of NaOH FHF&A     6x̙ ?D0 CCurve levels off at pH 13 due to excess 0.1M NaOH (a strong alkali) DHD&-   %  6$x̙ ?+w  /pH 4 due to 0.1M CH3COOH (weak monoprotic acid)F0H&    G   0x )weak acid (CH3COOH) v. strong base (NaOH)*(2 f ff$dB ! <D)@0A " 0Pp@ 0 0dB #@ <D)@X@ $ 0X0@ 0 0B  s *޽h ? ̙33  0L0   / (  d  <?`Hd  <f? `d  <?h ` P  C (Aphaxesg P  C (Aphwasbgh    6z̙ ?<  &PHENOLPHTHALEIN LITMUS METHYL ORANGEL' 2h   6T z̙ ? Only phenolphthalein is suitable - it is the only one to change in the  vertical portion ZHZf Z G   0lz )weak acid (CH3COOH) v. strong base (NaOH)*(2 f ff$dB   <D)@0A  0Pp@ 0 0dB @ <D)@X@  0X0@ 0 0dB  <D)`@a  0`@ 0 0dB @ <D)`h`  0h@@ 0 0B  s *޽h ? ̙33  0L0  z  $ ( @p D  0x$z &weak acid (CH3COOH) v. weak base (NH3)'(2 f  f fP  C (Aphaxesg P  C (Aphwawbg o   6/z̙ ?I- RTypes  @     6l0z̙ ?4 l `Steady pH change H  7  6d8z̙ ?+w  /pH 4 due to 0.1M CH3COOH (weak monoprotic acid)X0Hf&      6$?z̙ ?} 54 eNO SHARP CHANGE IN pH H     6Cz̙ ?  @Curve levels off at pH 10 due to excess 0.1M NH3 (a weak alkali)FAH/ A dB ! <D)@0A " 0Pp@ 0 0dB #@ <D)@X@ $ 0X0@ 0 0B  s *޽h ? ̙33  0L0    (  d  <?`Hd  <f? `d  <?h ` P  C (Aphaxesg =  6pQz̙ ?<z  9PHENOLPHTHALEIN LITMUS METHYL ORANGE NOTHING SUITABLE ( 22P  C (Aphwawbg o    6\z̙ ?\ hThere is no suitable indicator- none change in the  vertical portion. The end point can be detected by plotting a curve using a pH meter.  Hf  D   0ez &weak acid (CH3COOH) v. weak base (NH3)'(2 f  f fdB   <D)@0A  0Pp@ 0 0dB @ <D)@X@  0X0@ 0 0B  s *޽h ? ̙33  0L0   M (  Q   0uz #Other pH curves - acid v. carbonate@$(2ff dB  <D)@0A  0Pp@ 0 0dB @ <D)@X@  0X0@ 0 0   0z  Sodium carbonate reacts with hydrochloric acid in two steps... Step 1 Na2CO3 + HCl   > NaHCO3 + NaCl Step 2 NaHCO3 + HCl   > NaCl + H2O + CO2 Overall Na2CO3 + 2HCl   > 2NaCl + H2O + CO20PAffffffff fffff ffffffffffffffffffffffffftW        K B  s *޽h ? ̙33j 0L0 (  T  C ,Aphdibaseg;   0z #Other pH curves - acid v. carbonate@$(2ff dB  <D)@0A  0Pp@ 0 0dB @ <D)@X@  0X0@ 0 0   6|̙ ?;  oThere are two sharp pH changes  H   F  6|̙ ?{; P  The second addition of HCl is exactly the same as the first because the number of moles of HCl which react with the NaHCO3 is the same as that reacting with the Na2CO3.@ffCffff)fffff@  A  K   6X|̙ ? q  |17.50cm3D @fff    6|̙ ? X   |35.00cm3D @fff  pB  HDfo?_ pB  HDfo?_ h   0+|  Sodium carbonate reacts with hydrochloric acid in two steps... Step 1 Na2CO3 + HCl   > NaHCO3 + NaCl Step 2 NaHCO3 + HCl   > NaCl + H2O + CO2 Overall Na2CO3 + 2HCl   > 2NaCl + H2O + CO20PAffffffff fffff ffffffffffffffffffffffffftW        K B  s *޽h ? ̙336  0L0    d ( w T  C ,Aphdibaseg;   0lH| #Other pH curves - acid v. carbonate@$(2ff dB  <D)@0A  0Pp@ 0 0dB @ <D)@X@  0X0@ 0 0d   <f?  ( j   6O|̙ ?P PZ  lFirst rapid pH change around pH = 8.5 due to the formation of NaHCO3 . Can be detected using phenolphthaleinhm@Cffff3f m   6dX|̙ ?;  oThere are two sharp pH changes  H     0Pc|  Sodium carbonate reacts with hydrochloric acid in two steps... Step 1 Na2CO3 + HCl   > NaHCO3 + NaCl Step 2 NaHCO3 + HCl   > NaCl + H2O + CO2 Overall Na2CO3 + 2HCl   > 2NaCl + H2O + CO20PAffffffff fffff ffffffffffffffffffffffffftW        K B  s *޽h ? ̙33 0L0   E( w T  C ,Aphdibaseg;   0| #Other pH curves - acid v. carbonate@$(2ff dB  <D)@0A  0Pp@ 0 0dB @ <D)@X@  0X0@ 0 0d   <f?  ( d   <?  ` j   6D|̙ ?P PZ  lFirst rapid pH change around pH = 8.5 due to the formation of NaHCO3 . Can be detected using phenolphthaleinhm@Cffff3f m m   6|̙ ? P  oSecond rapid pH change around pH = 4 due to the formation of acidic CO2 . Can be detected using methyl orange. hp@Ffff f3f p   6Ƞ|̙ ?;  oThere are two sharp pH changes  H     0H|  Sodium carbonate reacts with hydrochloric acid in two steps... Step 1 Na2CO3 + HCl   > NaHCO3 + NaCl Step 2 NaHCO3 + HCl   > NaCl + H2O + CO2 Overall Na2CO3 + 2HCl   > 2NaCl + H2O + CO20PAffffffff fffff ffffffffffffffffffffffffftW        K B  s *޽h ? ̙33P  0L0   ~ ( w J  0|xH *Other pH curves - polyprotic acids (H3PO4)+(2f  f dB  <D)@0A  0Pp@ 0 0dB @ <D)@X@  0X0@ 0 0  0P| l Phosphoric acid is triprotic; it reacts with sodium hydroxide in three steps... Step 1 H3PO4 + NaOH   > NaH2PO4 + H2O Step 2 NaH2PO4 + NaOH   > Na2HPO4 + H2O Step 3 Na2HPO4 + NaOH   > Na3PO4 + H2O P\fffffffff ffffffffffffffffffffffffft   L  7  5   B  s *޽h ? ̙33  0L0 L D 0  (  J  0xH *Other pH curves - polyprotic acids (H3PO4)+(2f  f dB  <D)@0A  0Pp@ 0 0dB @ <D)@X@  0X0@ 0 0R  C *AphphoshgH   6L̙ ? ; P q!There are three sharp pH changes  "H" " #  6̙ ?   SEach successive addition of NaOH is the same as equal number of moles are involved. THTf&  4   0 l Phosphoric acid is triprotic; it reacts with sodium hydroxide in three steps... Step 1 H3PO4 + NaOH   > NaH2PO4 + H2O Step 2 NaH2PO4 + NaOH   > Na2HPO4 + H2O Step 3 Na2HPO4 + NaOH   > Na3PO4 + H2O P\fffffffff ffffffffffffffffffffffffft   L  7  5   B  s *޽h ? ̙33T  0L0    l ( w lJ l 0:xH *Other pH curves - polyprotic acids (H3PO4)+(2f  f dB  l <D)@0A  l 0Pp@ 0 0dB  l@ <D)@X@  l 0X0@ 0 0R l C *AphphoshgH pB l HDfo? `p  l 6$F̙ ?f J pH of H3PO4 = 1.5j@   l 0`U ~ Phosphoric acid is triprotic; it reacts with sodium hydroxide in three steps... Step 1 H3PO4 + NaOH   > NaH2PO4 + H2O Step 2 NaH2PO4 + NaOH   > Na2HPO4 + H2O Step 3 Na2HPO4 + NaOH   > Na3PO4 + H2O P\ffffff ffffffffffffffffffffffffft   L  7  5   B l s *޽h ? ̙33  0L0   @ * ( w J  0sxH *Other pH curves - polyprotic acids (H3PO4)+(2f  f dB  <D)@0A  0Pp@ 0 0dB @ <D)@X@  0X0@ 0 0R  C *AphphoshgH pB   HDfo? `p pB   HDfo?( p (   6̙ ?   pH of NaH2PO4 = 4.4j@    *  6̙ ?f J pH of H3PO4 = 1.5|@ffff ff3    0ܖ ~ Phosphoric acid is triprotic; it reacts with sodium hydroxide in three steps... Step 1 H3PO4 + NaOH   > NaH2PO4 + H2O Step 2 NaH2PO4 + NaOH   > Na2HPO4 + H2O Step 3 Na2HPO4 + NaOH   > Na3PO4 + H2O P\ffffff ffffffffffffffffffffffffft   L  7  5   B  s *޽h ? ̙33 0L0 PH( w J  0xH *Other pH curves - polyprotic acids (H3PO4)+(2f  f dB  <D)@0A  0Pp@ 0 0dB @ <D)@X@  0X0@ 0 0R  C *AphphoshgH pB   HDfo? `p pB   HDfo?( p ( pB   HDfo? p   6̙ ?   pH of Na2HPO4 = 9.6j@   (  6̙ ?   pH of NaH2PO4 = 4.4|@ ffff ff3  *  6<̙ ?f J pH of H3PO4 = 1.5|@ffff ff3    0h  Phosphoric acid is triprotic; it reacts with sodium hydroxide in three steps... Step 1 H3PO4 + NaOH   > NaH2PO4 + H2O Step 2 NaH2PO4 + NaOH   > Na2HPO4 + H2O Step 3 Na2HPO4 + NaOH   > Na3PO4 + H2O P\fffffffff ffffffffffffffffffffffft   L  7  5   B  s *޽h ? ̙33M 0L0 P{(  J  0xH *Other pH curves - polyprotic acids (H3PO4)+(2f  f dB  <D)@0A  0Pp@ 0 0dB @ <D)@X@  0X0@ 0 0R  C *AphphoshgH pB   HDfo? `p pB   HDfo?( p ( pB   HDfo? p pB   HDfo? p    6̙ ? z pH of Na3PO4 = 12j@   (  6̙ ?   pH of Na2HPO4 = 9.6|@ffff ff3  (  6(̙ ?   pH of NaH2PO4 = 4.4|@ ffff ff3  *  6@"̙ ?f J pH of H3PO4 = 1.5|@ffff ff3    01 ~ Phosphoric acid is triprotic; it reacts with sodium hydroxide in three steps... Step 1 H3PO4 + NaOH   > NaH2PO4 + H2O Step 2 NaH2PO4 + NaOH   > Na2HPO4 + H2O Step 3 Na2HPO4 + NaOH   > Na3PO4 + H2O P\fffffffff fffffffffffffffffffffft   L  7  5   B  s *޽h ? ̙33 0L0 ` <(    0P JREVISION CHECK (2  04U ZWhat should you be able to do? (2Z   0 Yh  Recall the definition of a weak acid Understand why indicators can be made from weak acids Understand why indicators must change colour quickly over a small pH range Recall and explain the shape of titration curves involving acids and bases Explain why particular indicators are used for certain titrations Explain the shape of the titration curve for phosphoric acid Explain the shape of the titration curve for acid -sodium carbonate reactions 2f#f f,f fBff8ff;ff6ffGf8   0j   ~,CAN YOU DO ALL OF THESE? YES NO6- 2!    0 H @P 0 0   0f h @U 0 0H  0޽h ? ̙335 0L0 p](  9  0s  YYou need to go over the relevant topic(s) again Click on the button to return to the menudG(282/$f f) f"  s *fX@ 0 0  0P@Q 0 0  s * x  P @S 0 0H  0޽h ? ̙33> 0L0 f(    0xK (WELL DONE! Try some past paper questions@)(2 <fff"  s *fX@ 0 0  0P@N 0 0H  0޽h ? ̙33 0L0 PH(    0x ~INDICATORS & pH CURVES THE ENDD(26f6ff  0 h. 2009 JONATHAN HOPTON & KNOCKHARDY PUBLISHING/(2/fB  s *޽h ? ̙33r d#)O/2  G )B |w3*.`=~Q&dH~+="+GWdsR~jn.:5Oh+'0T hp   No Slide TitleHOPTONJONATHAN HOPTON540Microsoft PowerPoint@@@hNx@0a!yGSg  )'    """)))UUUMMMBBB999|PP3f333f3333f3ffffff3f̙3ff333f333333333f33333333f33f3ff3f3f3f3333f33̙33333f333333f3333f3ffffff3f33ff3f3f3f3fff3ffffffffff3ffff̙fff3fffff3fff333f3f3ff3ff33f̙̙3̙ff̙̙̙3f̙3f333f3333f3ffffff3f̙3f3f3f333f3333f3ffffff3f̙3f3ffffffffff!___wwwT4'A x(xKʦ 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