1. Calculate values of K SP for the following salts using the information given:

Question

1.     Calculate values of KSP for the following salts using the information given:

a.     A sample of 4.8 x 10-5 mol of calcium oxalate (CaC2O4) dissolves in 1.0 L of water to produce a saturated solution.

CaC2O4 (s) ? Ca2+ (aq) + C2O42- (aq)

b.     The concentration of Pb2+ in a solution saturated with PbBr2 is 2.14 x 10-2 M.

c.     The molar solubility of BiI3 is 1.32 x 10-5 mol / L.

2.     The KSP for lead (II) iodide is 1.4 x 10-8. Calculate the solubility of lead (II) iodide in each of the following:

a.     Water

b.     0.10 M lead (II) nitrate

c.     0.010 M sodium iodide

Explanation / Answer

2.b. for 0.10 M lead (II) nitrate

Let x = mol/L of PbI2 that dissolve : this will give us x mol/L of Pb2+ and 2x mol/L of I-.
But we have arleady 0.10 M of Pb2+ ( common ion effect)
[Pb2+] = x + 0.10
[I-] = 2x

Ksp = [x + 0.10][2x]^2
we can neglet x compared to 0.10
Ksp = 1.4 x 10^-8 = 0.10 ( 4x^2) = 0.40 x^2

x = molar solubility = 1.9 x 10^-4 M

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