For each of the salts on the left, match the salts on the right that can be compared directly, using Ksp values, to estimate solubilities.
(If more than one salt on the right can be directly compared, include all the relevant salts by writing your answer as a string of characters without punctuation, e.g, ABC.)
|1.||lead sulfate||A. BaF2|
|2.||lead bromide||B. Ag2SO3|
Write the expression for K in terms of the solubility, s, for each salt, when dissolved in water.
Note: Multiply out any number and put it first in the Ksp expression. Combine all exponents for s.
**** 1 & 2 COULD HAVE MORE THAN 1 ANSWER *****
Solubility of AB, A2B, AB2, A3B, AB3, A2B3, A3B2
For solubility comparisson:
AB <-> A+ + B-; Ksp = [A+][B-] = S*S = S^2 --> S = sqrt(Ksp)
A2B <--> 2A+ + B-2 Ksp = [A+]^2[B-2] = (2S)^2 * S = 4*S^3 --> S = (Ksp/4)^(1/3)
AB2 <--> A+2 + 2B- ; Ksp = [A+2][B-]^2 = S* (2S)^2 = 4*S^3 --> S = (Ksp/4)^(1/3)
Now, substitute al Ksp values, and identifty molar solubilities:
Lead sulfate = PbSO4 = AB type
Lead Bromide = PbBr2 = AB2 type
BaF2 = AB2 type
Ag2SO3 = A2B type
CaCrO4 = AB type
Pb(OH)2 = AB2 type
then, recall that AB2 = A2B types
from the list
PbSO4 = CaCrO4 only
PbBr2 = (BaF2, Ag2SO3, Pb(OH)2))
Ksp = [Pb2+][SO4-2]
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