Calculate the K_sp for silver sulfite if the solubility of Ag₂SO₃ in pure water is 4.6 × 10^-3g L^-1. A)3.8 × 10^-15 B)1.5 × 10^-14 C)2.4 × 10^-10 D)4.8 × 10^-10

Question

Quizplus · Accepted Answer

The equation for the dissolving of silver sulfite in water is Ag2SO3(S) ↔ 2Ag+(aq) + SO32-(aq).

Using the given solubility of Ag2SO3 in water (4.6 × 10-3 g/L or 4.6 × 10-6 mol/L), we can set up an ICE table:

Initial: 0 mol/L Ag+, 0 mol/L SO32-
Change: +2x mol/L Ag+, +x mol/L SO32-
Equilibrium: 2x mol/L Ag+, x mol/L SO32-

We know that the Ksp expression for Ag2SO3 is [Ag+]2[SO32-]. Plugging in the equilibrium concentrations from the ICE table:

Ksp = (2x)2(x) = 4x3

We need to solve for x, which represents the molar solubility of Ag2SO3.

4.6 × 10-6 mol/L = x
x = 4.6 × 10-6 mol/L

Plugging this value back into the Ksp expression:

Ksp = 4(4.6 × 10-6)3 = 1.5 × 10-14

Therefore, the correct answer is B) 1.5 × 10-14.

Calculate the Ksp for Silver Sulfite If the Solubility of Ag2SO3

Calculate the K_sp for Silver Sulfite If the Solubility of Ag₂SO₃