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Use the Ksp values to calculate the molar solubility of each of the following compounds in pure water.?
a) BaSO4 (Ksp = 1.07×10−10)
b) Ag2CrO4 (Ksp = 1.12×10−12)
c) Ca(OH)2 (Ksp = 4.68×10−6)
1 Answer
- hcbiochemLv 71 year ago
a) BaSO4(s) <--> Ba2+(aq) + SO42-(aq)
Let S = molar solubility = [Ba2+] = [SO42-]Ksp = [Ba2+][SO42-] = 1.07X10^-10S^2 / 1.07X10^-10S = 1.03X10^-5 Mb) Ag2CrO4(s) <--> 2 Ag+(aq) + CrO42-(aq)
Let S = molar solubility = [CrO42-], and [Ag+] = 2S
Ksp = [Ag+]^2[CrO42-] = 1.12X10^-12
1.12X10^-12 = (2S)^2(S) = 4S^3
S = 6.54X10^-5 M
c) Solve this one just as b). Use S = [Ca2+] and [OH-] = 2S.
