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  3. 1. from the kb values for arsenate in the followin

1. From the Kb values for arsenate in the following equations, calculate the three Ka values...

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Chemistry

1. From the Kb values for arsenate in the following equations,calculate the three Ka values of arsenic acid. (Assume that Kw is1.01???10?14.)

a) Kb1 = 3.19???10?3

b) Kb3 = 1.76???10?12

2. A solution contains 0.0490 M Ca2+ and0.0316 M Ag+ (The Ksp ofCaSO4 is 2.4???10?5, andtheKsp of Ag2SO4 is1.5???10?5.)

a) What will be the concentration of Ca2+ whenAg2SO4 begins to precipitate?

I would greatly appreciate assistance with the both of theseproblems.

Answer & Explanation Solved by verified expert
4.2 Ratings (868 Votes)
1 GivenKb1 Arsenate 319 x 103pKb log Kb log 319 x 103 250Now Ka x Kb Kw Kw Ionic product of water 1014 at 25OCPutting log on both sideslog Ka x log Kb log KwpKa pKb 14Hence pKa 14 pKb 14 250Hence pKa1 1150pKa    See Answer
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