CH10_Page_24 - Because 1.2 x10" «cc H.036 the initial...

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Unformatted text preview: Because 1.2 x10" «cc: H.036 , the initial assumption that the first dissociation would dominate is valid. To calculate [DH'] , we use the Kw relationship: Kw = [330‘ HDH‘] K . "4 [OH—1 r ~—””"m =2.8x1fl"3mol-L“' = [H30*] " case In summary, [stcg] = nosa mol - L'j, [H301 = {Hso3-1 = nose mol - L‘i, [5032‘] = 1.2:»c1o-T mol-L'J,[OH'] =23 x 10'” Inc-1+ 1:1 10.92 The equilibrium reactions of interest are 110W the base forms of the carbonic acid equilibria, so Kb values should be calculated for the following changes: 80:1an + H200) ‘—_- H303_(aq_] + OH-(an K . —II£ Kn =_w=1 00x10; =33x ml, s1,2 1.2 x to HSOg'taq] + HIGH) F‘ also] {sq} + oH-{aq} K LEI!) x 10'” K = ‘” =——=a.r><1tr'a u It“2 1.5 x to-2 Because the seeond hydrolysis constant is much smaller than the first, we can assume that the first step dominates: Concentration (null-L") SUJI'IIREJH H200) 7—“ ESQ—{Hal + UPI—(as) initial [L125 — I] 0 change —x — +3: +1: final {L125 — x — +x +x K : [HSOJHDH‘] '” [303‘] sane-“=fl— "‘2 fl.125—x_fl.125—x 313 ...
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