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V$$$$b$bpe# zt O R$FE-Qڛb>"& 0AA !ff̙f3f@d g4KdKd< 0php8 <4BdBd@w 0t0/g4:d:d,k 0p@ pp<4!d!d@w 0t0/ʚ;ʚ;<4dddd@ x 0@r0___PPT10 pp2___PPT9/ 0? %O ==<  & ( )STU?+HIC,DE- P4   0` ̙33` ` ff3333f` 333MMM` f` f` 3>?" dd@,|?" dd@   " @ ` n?" dd@   @@``PR    @ ` ` p>>L0 VN (    6 P  T Click to edit Master title style! !  0T   RClick to edit Master text styles Second level Third level Fourth level Fifth level!     S  0H ``  X*  0쫍 `   Z*  0 `   Z*z  bA޽h @ ?Parchment ̙33 Default Design 0 zr@ ( )   0Xv P   v P*    0v    v R*  d  c $ ?  v  08lv  @ v RClick to edit Master text styles Second level Third level Fourth level Fifth level!     S  6t `P  v P*    6v `  v R*  H  0޽h ? ̙3380___PPT10. 0X(   $+ X X 0v P   v X*  X 0\    v Z*  X 6 `P   X*  X 6  `   Z* H X 0޽h ? ̙3380___PPT10.1$ 0L0 3+P3(  5  0D  5ACIDS, BASES AND SALTS A guide for A level students  (2 828n282<f$ff<f / 00 "`>B u2008 SPECIFICATIONS2(2$   J 0 C "A KTRE  1 0 (H OKNOCKHARDY PUBLISHING(2 f 2 <̙? x @x 0 0 3 <̙? x @t 0 0B  s *޽h ? ̙33y___PPT10Y+D=' = @B +  0L0   P (  dB  <D)P0Q  0Pp@ 0 0dB @ <D)PXP  0X0@ 0 0Y   0_a 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? xP    0t{0P( OKNOCKHARDY PUBLISHING(2    0yX dACIDS, BASES AND SALTS2(2$f<fB  s *޽h ? ̙33y___PPT10Y+D=' = @B + 0L0 (t(  tdB t <D)P0Q t 0Pp@ 0 0dB t@ <D)PXP t 0X0@ 0 0l  t 0t BRNSTED-LOWRY THEORY ACID proton donor HCl   > H+(aq) + Cl(aq) BASE proton acceptor NH3 (aq) + H+(aq)   > NH4+(aq) FHt@! !! f !f     )              t 0`q~ ]ACIDS AND BASES2(2ffB t s *޽h ? ̙33y___PPT10Y+D=' = @B +d 0L0 sk# (  dB  <D)P0Q  0Pp@ 0 0dB @ <D)PXP  0X0@ 0 0,  0ԣz  BRNSTED-LOWRY THEORY ACID proton donor HCl   > H+(aq) + Cl(aq) BASE proton acceptor NH3 (aq) + H+(aq)   > NH4+(aq) Conjugate systems Acids are related to bases ACID PROTON + CONJUGATE BASE Bases are related to acids BASE + PROTON CONJUGATE ACID tH<@P(! !! f !f     !)              0xq~ ]ACIDS AND BASES2(2ffF ?   8N   fB  6DolB  <BDo{>T  # L)?fB  6DolB  <BDo{F ?  07 8N   fB  6DolB  <BDo{>T  # L)?fB  6DolB  <BDo{B  s *޽h ? ̙33y___PPT10Y+D=' = @B +` 0L0 og##(  dB  <D)P0Q  0Pp@ 0 0dB @ <D)PXP  0X0@ 0 0p  08  BRNSTED-LOWRY THEORY ACID proton donor HCl   > H+(aq) + Cl(aq) BASE proton acceptor NH3 (aq) + H+(aq)   > NH4+(aq) Conjugate systems Acids are related to bases ACID PROTON + CONJUGATE BASE Bases are related to acids BASE + PROTON CONJUGATE ACID For an acid to behave as an acid, it must have a base present to accept a proton... HA + B BH+ + A acid base conjugate conjugate acid base example CH3COO + H2O CH3COOH + OH base acid acid base |H<@P(@! !! f !f     !,fffc!33 33333M!)           ~   0q~ ]ACIDS AND BASES2(2ffF ?    F ? 8N    fB   6D3olB   <BD3o{>T   # L)?fB   6D3olB  <BD3o{F ?   8N   fB  6DolB  <BDo{>T  # L)?fB  6DolB  <BDo{F ?  07 8N   fB  6DolB  <BDo{>T  # L)?fB  6DolB  <BDo{F ?  w 8N   fB  6D3olB   <BD3o{>T  !# L)?fB " 6D3olB # <BD3o{B  s *޽h ? ̙33y___PPT10Y+D=' = @B +  0L0    ( w r  0t"80 STRONG ACIDS completely dissociate (split up) into ions in aqueous solution e.g. HCl   > H+(aq) + Cl(aq) MONOPROTIC 1 replaceable H HNO3   > H+(aq) + NO3(aq) H2SO4   > 2H+(aq) + SO42-(aq) DIPROTIC 2 replaceable H s d@&PG@ !f: ff! f!"ff ff! fff!ffff ff! fff!"t`       /  Y dB  <D)P0Q  0Pp@ 0 0dB @ <D)PXP  0X0@ 0 0   0hH8q~ dSTRONG ACIDS AND BASES2(2ffB  s *޽h ? ̙33y___PPT10Y+D=' = @B +  0L0    (  ~  0,O80  STRONG ACIDS completely dissociate (split up) into ions in aqueous solution e.g. HCl   > H+(aq) + Cl(aq) MONOPROTIC 1 replaceable H HNO3   > H+(aq) + NO3(aq) H2SO4   > 2H+(aq) + SO42-(aq) DIPROTIC 2 replaceable H s STRONG BASES completely dissociate into ions in aqueous solution e.g. NaOH(aq)   > Na+(aq) + OH(aq)(@&P@ !f: ff! f!"ff ff! fff!ffff ff fff!% !f-3! 33!f3!`       /          dB  <D)P0Q  0Pp@ 0 0dB @ <D)PXP  0X0@ 0 0  0H}8q~ dSTRONG ACIDS AND BASES2(2ffB  s *޽h ? ̙33y___PPT10Y+D=' = @B + 0L0  X(    0\80  DWeak acids partially dissociate into ions in aqueous solution e.g. ethanoic acid CH3COOH(aq) CH3COO(aq) + H+(aq) When a weak acid dissolves in water an equilibrium is set up HA(aq) + H2O(l) A(aq) + H3O+(aq) The water stabilises the ions To make calculations easier the dissociation can be written... HA(aq) A(aq) + H+(aq) ?@PGFPF f!<333!333! 33!>3!333!3!3333!a3!3! 33!I  0  @    r        dB  <D)P0Q  0Pp@ 0 0dB @ <D)PXP  0X0@ 0 0F ?   :h8N    fB   6D3olB   <BD3o{>T  # L)?fB  6D3olB  <BD3o{F ?   N8N   fB  6D3olB  <BD3o{>T  # L)?fB  6D3olB  <BD3o{F ?  @ n  8N   fB  6D3olB  <BD3o{>T  # L)?fB  6D3olB  <BD3o{  08q~ X WEAK ACIDS2 (2 ffB  s *޽h ? ̙33y___PPT10Y+D=' = @B + 0L0 +#(     080  Weak acids partially dissociate into ions in aqueous solution e.g. ethanoic acid CH3COOH(aq) CH3COO(aq) + H+(aq) When a weak acid dissolves in water an equilibrium is set up HA(aq) + H2O(l) A(aq) + H3O+(aq) The water stabilises the ions To make calculations easier the dissociation can be written... HA(aq) A(aq) + H+(aq) The weaker the acid the less it dissociates the more the equilibrium lies to the left. ?@PGFPF]@ f!<333!333! 33!>3!333!3!3333!a3!3!33!`I  0  @    r       b dB  <D)P0Q  0Pp@ 0 0dB @ <D)PXP  0X0@ 0 0F ?  :h8N   fB   6D3olB   <BD3o{>T   # L)?fB   6D3olB   <BD3o{F ?   N8N   fB  6D3olB  <BD3o{>T  # L)?fB  6D3olB  <BD3o{F ?  @ n  8N   fB  6D3olB  <BD3o{>T  # L)?fB  6D3olB  <BD3o{  0d8q~ X WEAK ACIDS2 (2 ffB  s *޽h ? ̙33y___PPT10Y+D=' = @B + 0L0    \ (      0q0  $:Partially react with water to give ions in aqueous solution e.g. ammonia When a weak base dissolves in water an equilibrium is set up NH3 (aq) + H2O (l) NH4+ (aq) + OH (aq) as in the case of acids it is more simply written NH3 (aq) + H+ (aq) NH4+ (aq) ;@t333 333333 33433333333  #     @        dB   <D)P0Q   0Pp@ 0 0dB  @ <D)PXP   0X0@ 0 0   0` qq~ X WEAK BASES2 (2 ffF ?   ' e8N    fB   6D3olB   <BD3o{>T   # L)?fB   6D3olB   <BD3o{F ?   - [ 8N    fB   6D3olB   <BD3o{>T   # L)?fB   6D3olB   <BD3o{B   s *޽h ? ̙33y___PPT10Y+D=' = @B + 0L0 q(    0|3q0  9Partially react with water to give ions in aqueous solution e.g. ammonia When a weak base dissolves in water an equilibrium is set up NH3 (aq) + H2O (l) NH4+ (aq) + OH (aq) as in the case of acids it is more simply written NH3 (aq) + H+ (aq) NH4+ (aq) The weaker the base the less it dissociates the more the equilibrium lies to the left The relative strengths of bases can be expressed as Kb or pKb values.v@t333 333333 33433333333     #     @           dB  <D)P0Q  0Pp@ 0 0dB @ <D)PXP  0X0@ 0 0  0,qq~ X WEAK BASES2 (2 ffF ?  ' e8N    fB   6D3olB   <BD3o{>T   # L)?fB   6D3olB  <BD3o{F ?  - [ 8N   fB  6D3olB  <BD3o{>T  # L)?fB  6D3olB  <BD3o{B  s *޽h ? ̙33y___PPT10Y+D=' = @B + 0L0  y( w   0aq0 Is a typical acid in dilute aqueous solution HCl   > H+ (aq) + Cl(aq)W@3333 3Z3        dB  <D)P0Q  0Pp@ 0 0dB @ <D)PXP  0X0@ 0 0  0pqq~ mREACTIONS OF HYDROCHLORIC ACID 2 (2ff   0,vq0A H  nHydrogen chloride is a colourless covalent gas; it is a poor conductor of electricity because there are no free electrons or ions present. It has no action on dry litmus paper because there are no aqueous hydrogen ions present.Z@"f f  T   C ,AHClbefore^RVB  s *޽h ? ̙33y___PPT10Y+D=' = @B +f  0L0 u m   ( w   0q0 Is a typical acid in dilute aqueous solution HCl   > H+ (aq) + Cl(aq)W@3333 3Z3        dB  <D)P0Q  0Pp@ 0 0dB @ <D)PXP  0X0@ 0 0  0(qq~ mREACTIONS OF HYDROCHLORIC ACID 2 (2ff   0ȓq0A H  2Hydrogen chloride is a colourless covalent gas; it is a poor conductor of electricity because there are no free electrons or ions present. It has no action on dry litmus paper because there are no aqueous hydrogen ions present.@  l   0q@ 0| BIf the gas is passed into water, the hydrogen chloride molecules dissociate into ions. The solution now conducts electricity showing ions are present. For each hydrogen chloride molecule that dissociates one hydrogen ion and one chloride ion are produced. The solution turns litmus paper red because of the H+(aq) ions.C@7fff f&6   T   C ,AHClbefore^RVR   C *AHClafter5VB  s *޽h ? ̙33y___PPT10Y+D=' = @B +  0L0    G (    0Tq0 Is a typical acid in dilute aqueous solution HCl   > H+ (aq) + Cl(aq)W@3333 3Z3        dB  <D)P0Q  0Pp@ 0 0dB @ <D)PXP  0X0@ 0 0  0pqq~ mREACTIONS OF HYDROCHLORIC ACID 2 (2ff   0q0A H  nHydrogen chloride is a colourless covalent gas; it is a poor conductor of electricity because there are no free electrons or ions present. It has no action on dry litmus paper because there are no aqueous hydrogen ions present.Z@"f f  l   0pq@ 0| BIf the gas is passed into water, the hydrogen chloride molecules dissociate into ions. The solution now conducts electricity showing ions are present. For each hydrogen chloride molecule that dissociates one hydrogen ion and one chloride ion are produced. The solution turns litmus paper red because of the H+(aq) ions.C@7fff f&6   T   C ,AHClbefore^RVR   C *AHClafter5VB  s *޽h ? ̙33y___PPT10Y+D=' = @B +>  0L0 M E   ( eHCla   0Xq0 Is a typical acid in dilute aqueous solution HCl   > H+ (aq) + Cl(aq)W@3333 3Z3        dB  <D)P0Q  0Pp@ 0 0dB @ <D)PXP  0X0@ 0 0  0qq~ mREACTIONS OF HYDROCHLORIC ACID 2 (2ff  0\t/ X ~2 HYDROGEN CHLORIDE HYDROCHLORIC ACID colourless gas Appearance colourless soln. covalent molecule Bonding aqueous ions HCl(g) Formula HCl(aq) poor Conductivity good no reaction Dry blue litmus goes red3@ f2ff ffffff f fff Zl  3  "  c T   C ,AHClbefore^RVR   C *AHClafter5VB  s *޽h ? ̙33y___PPT10Y+D=' = @B +  0L0     (    0Ht0 Is a typical acid in dilute aqueous solution HCl   > H+ (aq) + Cl(aq)W@3333 3Z3        dB  <D)P0Q  0Pp@ 0 0dB @ <D)PXP  0X0@ 0 0   0tq~ mREACTIONS OF HYDROCHLORIC ACID 2 (2ff<   0dt X . Appearance Bonding and formula Conductivity Dry litmus hydrogen chloride colourless gas covalent molecule HCl(g) poor no reaction hydrochloric acid colourless soln. aqueous ions HCl(aq) good goes red0/@] f Z  N        0't0A H  nHydrogen chloride is a colourless covalent gas; it is a poor conductor of electricity because there are no free electrons or ions present. It has no action on dry litmus paper because there are no aqueous hydrogen ions present.Z@"f f  l   0P#t@ 0| BIf the gas is passed into water, the hydrogen chloride molecules dissociate into ions. The solution now conducts electricity showing ions are present. For each hydrogen chloride molecule that dissociates one hydrogen ion and one chloride ion are produced. The solution turns litmus paper red because of the H+(aq) ions.C@7fff f&6   T   C ,AHClbefore^RVR  C *AHClafter5VB  s *޽h ? ̙33y___PPT10Y+D=' = @B + 0L0 @0a(  0 0 0d?t0R |Metals magnesium + dil. hydrochloric acid   > magnesium chloride + hydrogen Mg(s) + 2HCl(aq)   > MgCl2(aq) + H2(g) @ P  N  @33333 &   dB 0 <D)P0Q 0 0Pp@ 0 0dB 0@ <D)PXP 0 0X0@ 0 0  0 0Jtq~ mREACTIONS OF HYDROCHLORIC ACID 2 (2ffB 0 0OtOXD<4___PPT9 0WRITE OUT THE BALANCED EQUATION FOR THE REACTION 1@1 3 1  @`B 0 s *޽h ? ̙33y___PPT10Y+D=' = @B +  0L0   P (    0_t0R Metals magnesium + dil. hydrochloric acid   > magnesium chloride + hydrogen Mg(s) + 2HCl(aq)   > MgCl2(aq) + H2(g) Mg(s) + 2H+(aq) + 2Cl(aq)   > Mg2+(aq) + 2Cl(aq) + H2(g).@ZP  N  @3333 3333333 &   dB  <D)P0Q  0Pp@ 0 0dB @ <D)PXP  0X0@ 0 0   0Tutq~ mREACTIONS OF HYDROCHLORIC ACID 2 (2ff*F      8fB  B 6Do x fB   6Dox  *F      X fB B 6Do x fB  6Dox    0|tOXD<4___PPT9 pWRITE OUT THE BALANCED EQUATION FOR THE REACTION DILUTE ACIDS AND SALTS CONTAIN IONS; WATER, HYDROGEN & CARBON DIOXIDE DON T2}@1 L 3 }  @`B  s *޽h ? ̙33y___PPT10Y+D=' = @B + 0L0   `{ (  @  0t0" Metals magnesium + dil. hydrochloric acid   > magnesium chloride + hydrogen Mg(s) + 2HCl(aq)   > MgCl2(aq) + H2(g) Mg(s) + 2H+(aq) + 2Cl(aq)   > Mg2+(aq) + 2Cl(aq) + H2(g) cancel ions Mg(s) + 2H+(aq)   > Mg2+(aq) + H2(g) @ZPG@  N  @3333 3333333 3!!!! !!! ! &  < dB  <D)P0Q  0Pp@ 0 0dB @ <D)PXP  0X0@ 0 0   0Xtq~ mREACTIONS OF HYDROCHLORIC ACID 2 (2ff*F      8fB  B 6Do x fB   6Dox  *F      X fB B 6Do x fB  6Dox    0tOX D<4___PPT9 vWRITE OUT THE BALANCED EQUATION FOR THE REACTION DILUTE ACIDS AND SALTS CONTAIN IONS; WATER, HYDROGEN & CARBON DIOXIDE DON T CANCEL OUT THE IONS WHICH APPEAR ON BOTH SIDES OF THE EQUATION2@} ? 3   @`B  s *޽h ? ̙33y___PPT10Y+D=' = @B +( 0L0 7/p(    0du0 > Metals magnesium + dil. hydrochloric acid   > magnesium chloride + hydrogen Mg(s) + 2HCl(aq)   > MgCl2(aq) + H2(g) Mg(s) + 2H+(aq) + 2Cl(aq)   > Mg2+(aq) + 2Cl(aq) + H2(g) cancel ions Mg(s) + 2H+(aq)   > Mg2+(aq) + H2(g) Basic Oxides copper(II) oxide + dil. hydrochloric acid   > copper(II) chloride + water CuO(s) + 2HCl(aq)   > CuCl2(aq) + H2O(l) Cu2+O2-(s) + 2H+(aq) + 2Cl(aq)   > Cu 2+ (aq) + 2Cl(aq) + H2O(l) cancel ions O2- + 2H+(aq)   > H2O(l)  @ZP@P@  N  @   3   Z  633333333 3333333 3!! !!!!!! t  d  K    ] dB  <D)P0Q  0Pp@ 0 0dB @ <D)PXP  0X0@ 0 0   0uq~ mREACTIONS OF HYDROCHLORIC ACID 2 (2ff*F      8fB  B 6Do x fB   6Dox  *F      X fB B 6Do x fB  6Dox  *F       fB B 6Do x fB  6Dox  *F      8  fB B 6Do x fB  6Dox  *F       fB B 6Do x fB  6Dox  B  s *޽h ? ̙33y___PPT10Y+D=' = @B +k 0L0  4 (  4 4 0Lu0 nAlkalis sodium hydroxide + dil. hydrochloric acid   > sodium chloride + water NaOH(aq) + HCl(aq)   > NaCl(aq) + H2O(l) Na+(aq) + OH(aq) + H+(aq) + Cl(aq)   > Na+ (aq) + Cl(aq) + H2O(l) cancel ions H+(aq) + OH(aq)   > H2O(l) <@Pb@Px>@  Q  Vfff f ffffffffff  !!!!!!! ! D  H                   '     dB 4 <D)P0Q 4 0Pp@ 0 0dB 4@ <D)PXP 4 0X0@ 0 0  4 0D5uq~ mREACTIONS OF HYDROCHLORIC ACID 2 (2ff*F     4 8fB  4B 6Do x fB  4 6Dox  *F     4 0 fB 4B 6Do x fB 4 6Dox  *F    4  fB 4B 6Do x fB 4 6Dox  B 4 s *޽h ? ̙33a 0L0 (  .  0l@u00 Alkalis sodium hydroxide + dil. hydrochloric acid   > sodium chloride + water NaOH(aq) + HCl(aq)   > NaCl(aq) + H2O(l) Na+(aq) + OH(aq) + H+(aq) + Cl(aq)   > Na+ (aq) + Cl(aq) + H2O(l) cancel ions H+(aq) + OH(aq)   > H2O(l) Carbonates calcium carbonate + hydrochloric acid   > calcium chloride + carbon dioxide + water CaCO3(s) + 2HCl(aq)   > CaCl2(aq) + CO2(g) + H2O(l) Ca2+CO32-(s) + 2H+(aq) + 2Cl(aq)   > Ca2+(aq) + 2Cl(aq) + CO2(g) + H2O(l) cancel ions CO32- + 2H+(aq)   > CO2(g) + H2O(l) t@Pb@Px@Pp@PK@  Q  V      X  ff5ffff fffffff ffffff fff f!!!!!!! !!!! !  D  H                   '     dB  <D)P0Q  0Pp@ 0 0dB @ <D)PXP  0X0@ 0 0   0uq~ mREACTIONS OF HYDROCHLORIC ACID 2 (2ff*F      8fB  B 6Do x fB   6Dox  *F      0 fB B 6Do x fB  6Dox  *F      fB B 6Do x fB  6Dox  *F     ` p fB B 6Do x fB  6Dox  *F     X  fB B 6Do x fB  6Dox  *F     `  fB B 6Do x fB  6Dox  B  s *޽h ? ̙33 0L0 )( w   0Tu00+ hAlkalis sodium hydroxide + dil. hydrochloric acid   > sodium chloride + water NaOH(aq) + HCl(aq)   > NaCl(aq) + H2O(l) Na+(aq) + OH(aq) + H+(aq) + Cl(aq)   > Na+ (aq) + Cl(aq) + H2O(l) cancel ions H+(aq) + OH(aq)   > H2O(l) Carbonates calcium carbonate + hydrochloric acid   > calcium chloride + carbon dioxide + water CaCO3(s) + 2HCl(aq)   > CaCl2(aq) + CO2(g) + H2O(l) Ca2+CO32-(s) + 2H+(aq) + 2Cl(aq)   > Ca2+(aq) + 2Cl(aq) + CO2(g) + H2O(l) cancel ions CO32- + 2H+(aq)   > CO2(g) + H2O(l) Hydrogen carbonates H+(aq) + HCO3   > CO2(g) + H2O(l) J@Pb@Px@Pp@P@  Q  V       X  5         !  !!! !! !!!!!! ^  H                   '      1 dB  <D)P0Q  0Pp@ 0 0dB @ <D)PXP  0X0@ 0 0   0uq~ mREACTIONS OF HYDROCHLORIC ACID 2 (2ff*F      8fB  B 6Do x fB   6Dox  *F      0 fB B 6Do x fB  6Dox  *F      fB B 6Do x fB  6Dox  *F     ` p fB B 6Do x fB  6Dox  *F     X  fB B 6Do x fB  6Dox  *F     X  fB B 6Do x fB  6Dox  B  s *޽h ? ̙33W 0L0  8(  8P 8 0xv0  hSUMMARY METALS react to give a salt + hydrogen METAL OXIDES react to give a salt + water METAL HYDROXIDES react to give a salt + water CARBONATES react to give a salt + water + carbon dioxide HYDROGENCARBONATES react to give a salt + water + carbon dioxide AMMONIA reacts to give an ammonium salt XHa@ f*ff&f f% f?f?f' i dB 8 <D)P0Q 8 0Pp@ 0 0dB 8@ <D)PXP 8 0X0@ 0 0  8 0vq~ mREACTIONS OF HYDROCHLORIC ACID 2 (2ffB 8 s *޽h ? ̙334 0L0 C;"@(   X @ @ <̙? x @D 0 0J @ C "A KTRE: . @ 0ߍx m . 2009 JONATHAN HOPTON & KNOCKHARDY PUBLISHING/(2/ f) !@ 0tfM  STHE END0(2f<f "@ 0(9 ACIDS, BASES AND SALTS T (2 82<f$f<fH @ 0޽h ? ̙33y___PPT10Y+D=' = @B +r@f*1%0&ek( sR+0 8y<:?C0#fG_H S0PBQfu./mOh+'0T hp   No Slide 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