The solubility of manganese (II)hydroxide (Mn(OH)₂)is 2.2 × 10^-5 M. What is the K_sp of Mn(OH)₂? A)1.1 × 10^-14 B)4.3 × 10^-14 C)2.1 × 10^-14 D)4.8 × 10^-10 E)2.2 × 10^-5

Question

Quizplus · Accepted Answer

The solubility product constant (Ksp) is the product of the concentration of the ions produced when a slightly soluble compound dissolves in water, each concentration raised to the power of its stoichiometric coefficient. The balanced equation for the dissolution of manganese (II) hydroxide is:

Mn(OH)2(s) ⇌ Mn2+(aq) + 2OH-(aq)

The solubility of Mn(OH)2 is given as 2.2 × 10^-5 M, which means that at equilibrium, the concentration of Mn2+ ions is also 2.2 × 10^-5 M, and the concentration of OH- ions is twice that, or 4.4 × 10^-5 M.

Substituting these values into the equation for Ksp, we get:

Ksp = [Mn2+][OH-]^2

Ksp = (2.2 × 10^-5)(4.4 × 10^-5)^2

Ksp = 4.3 × 10^-14

Therefore, the answer is B, 4.3 × 10^-14.

The Solubility of Manganese (II)hydroxide (Mn(OH)2)is 2

The Solubility of Manganese (II)hydroxide (Mn(OH)₂)is 2