Question

The Ksp for silver carbonate (Ag2CO3) is 8.1???10?12. Calculate the solubility of silver carbonate in each of the following.

(a) water mol/L

(b) 0.15 M AgClO3 mol/L

(c) 0.43 M Na2CO3 mol/L

Answer 1

Ksp for silver carbonate (Ag2CO3) = 8.1?x?10^-12

The reaction is

Ag2CO3 = 2Ag+ + CO3(-2)

Let the molar solubility of Ag2CO3 = x M

Equilibrium constant expression of the reaction

Ksp = (2x)^2 * (x)

8.1?* 10^-12 = 4x³

x³ = 2.025*10^-12

x = 0.0001265

= 1.265*10^-4 M

Part b

AgClO3 = Ag+ + ClO3-

Initial concentration of [Ag+] = 0.15 + 2x

Equilibrium constant expression of the reaction

Ksp = (0.15 + 2x)^2 * (x)

8.1?* 10^-12 = 0.0225x + 4x³ + 0.6x²

8.1?* 10^-12 - 0.0225x - 4x³ - 0.6x² = 0

x = 3.599*10^-10 M

Part C

Initial concentration of [CO3-2] = 0.43 + x

Equilibrium constant expression of the reaction

Ksp = (2x)^2 * (0.43 + x)

8.1?* 10^-12 = (4x^2) * (0.43 + x)

8.1?* 10^-12 = 1.72x^2 + 4x^3

8.1?* 10^-12 - 4x³ - 1.72x² = 0

x = 0.0000021700868 M

= 2.17*10^-6 M