A) A student measures the molar solubility of calcium carbonate
in a water solution to be 6.35×10-5 M.
Based on her data, the solubility product constant for this
compound is
B) A student measures the CrO42- concentration in a saturated
aqueous solution of calcium chromate to be 2.74×10-2 M.
Based on her data, the solubility product constant for calcium
chromate is
A)
At equilibrium:
CaCO3 <----> Ca2+ + CO32-
s s
Ksp = [Ca2+][CO32-]
Ksp = (s)*(s)
Ksp = 1(s)^2
Ksp = 1(6.35*10^-5)^2
Ksp = 4.032*10^-9
Answer: 4.03*10^-9
B)
At equilibrium:
CaCrO4 <----> Ca2+ + CrO42-
s s
Ksp = [Ca2+][CrO42-]
Ksp = (s)*(s)
Ksp = 1(s)^2
Ksp = 1(2.74*10^-2)^2
Ksp = 7.508*10^-4
Answer: 7.51*10^-4
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