Nov_23 - Suggested Problems: Chapter 11 21,23, 27, 33, 39,...

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Suggested Problems: Chapter 11 21,23, 27, 33, 39, 65, 77
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Common Ion Effect Addition of salts of weak acids suppresses ionization of weak acids e.g. Calculate [H 3 O + ] after adding 0.010 mole of NaOAc to 1.00 L of 0.15 M HOAc (K a = 1.8 x 10 -5 ) HOAc(aq) + H 2 O(aq) H 3 O + (aq)+ OAc - (aq) 0.15 0 0.010 -x +x +x [H 3 O + ] = 2.7 x 10 -4 M (originally 1.64 x 10 -3 M)
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Bases Strong bases dissociate completely (NaOH, KOH) [OH-] = original [B] Weak bases dissociate only slightly (NH 3 , CH 3 NH 2 ) The extent is reflected in the size of K b K b = [ BH + ][ OH - ] [ B ] Bases (B) produce OH - ions in water B + H 2 O BH + + OH -
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Calculate the pH of 0.35 M trimethyl amine, (CH 3 ) 3 N (K b = 6.3 x 10 -5 ) (CH 3 ) 3 N + H 2 O (CH 3 ) 3 NH + + OH - 0.35 0 0 0.35 – x x x K b = [ BH + ][ OH - ] [ B ] = x 2 .35 x = 6.3 x 10 5 x = [ OH - ] = 4.7 x 10 -3 M K w = [H 3 O + ][OH - ] = 10 -14 so [H 3 O + ] = 2.1x 10 -12 and pH = 11.68
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Hydrolysis Salts of weak acids or bases react with water to
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Nov_23 - Suggested Problems: Chapter 11 21,23, 27, 33, 39,...

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