09 - 2 O to form the conjugate acid and the hydroxide ion...

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11/5/09 Chapter 7 All of the acids we have considered thus far are monoprotic acids Strong acids: HCl, HNO 3 Weak acids: HCN, HF, CH 3 , CO 2 H Polyprotic acids: H 2 CO 3 —carbonic acid H 2 C 2 O 4 —oxalic acid H 3 PO 4 —phosphoric acid H 2 SO 4 —sulfuric H 2 A + H 2 O H 3 O + + HA - HA - + H 2 O H 3 O + + A 2- Question: What are the concentrations of all species in a 3.4 x 10 -3 M H 2 CO 3 solution? Assumption: because K a1 >>K a2 , we will assume all [H + ] derives from first reaction Strong bases: 2 Both completely ionize in H 2 O Weak bases: The most common are ammonia and its derivatives NH 3 CH 3 NH 2 (CH 3 ) 2 NH (CH 3 ) 3 N K b —base dissociation constant refers to the reaction of a base with H
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Unformatted text preview: 2 O to form the conjugate acid and the hydroxide ion The magnitude of K b tell us something about relative base strengths A strong acid has a weak conjugate base A strong base has a weak conjugate acid Suggest a qualitative relationship between the conjugate acid-base pair K a x K b = 1 x 10 -14 The product of the acid dissociation constant with the base dissociation constant for its conjugate base is the ion product constant for H 2 O Hydrolysis the reaction of an ion with H 2 O in which either H 3 O + or OH-is produced...
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