A student prepared a saturated solution of CaCrO_4 and found that when 156 mL of
ID: 955107 • Letter: A
Question
A student prepared a saturated solution of CaCrO_4 and found that when 156 mL of the solution was evaporated, 0.649 g of CaCrO_4 was left behind. What is the value of K_sp for this salt? At 25 degreeC, the molar solubility of silver phosphate is 1.8 times 10^-5 mol L ^-1. Calculate K_sp for this salt. The molar solubility of barium phosphate in water at 25 degreeC is 1.4 times 10^-8 mol L^-1. What is the value of K_sp, for this salt? What is the molar solubility of PbBr_2 in water? What is the molar solubility of Ag_2CrO_4 in water? Calculate the molar solubility of Zn(CN)_2 in water. (Ignore the reaction of the CN^- ion with water.) Calculate the molar solubility of PbF_2 in water. (Ignore the reaction of the ^- ion with water.) At 25 degreeC, the value of for LiF is 1.8 times 10^-3, and that for BaF_2 is 1.7 times 10^-6. Which salt, LiF or BaF_2, has the larger molar solubility in water? Calculate the solubility of each in units of mol L^-l. At 25 degreeC, the value of K_sp for AgCN is 6.0 times 10^-17 and that for Zn(CN)_2 is 3 times 10^-16. In terms of grams per 100 mL of solution, which salt is more soluble in water?Explanation / Answer
17.40.
Ksp for barium phosphate = [Ba2+]^3.[PO4^3-]^2
With molar solubility of salt 1.4 x 10^-8 mol.L-1
[Ba2+] = 3 x 1.4 x 10^-8 = 4.2 x 10^-8 mol.L-1
[PO4^3-] = 2 x 1.4 x 10^-8 = 2.8 x 10^-8 mol.L-1
So, Ksp = (4.2 x 10^-8)^3.(2.8 x 10^-8)^2 = 5.81 x 10^-38
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