For each of the salts on the left, match the salts on the right that can be compared directly, using K_{sp} 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. BaF_{2} | ||
2. | lead bromide | B. Ag_{2}SO_{3} | ||
C. CaCrO_{4} | ||||
D. Pb(OH)_{2} |
Write the expression for K in terms of the solubility, s, for each
salt, when dissolved in water.
lead sulfate |
lead bromide |
|||
K_{sp} = |
K_{sp} = |
Note: Multiply out any number and put it first in the K_{sp} 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
for
PbBr2 = (BaF2, Ag2SO3, Pb(OH)2))
Q2.
write Ksp
Ksp = [Pb2+][SO4-2]
Ksp [Pb2+][Br-]^2
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