Multiple Choice
The molar solubility of manganese (II) hydroxide, Mn(OH)2, is 3.48 × 10^-3 M. What is the Ksp of Mn(OH)2 at this temperature?
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18. Aqueous Equilibrium
Solubility Product Constant: Ksp
Multiple Choice
Given the molar solubility of Ag2SO3 in pure water is 1.55×10⁻⁵ M, what is the solubility product constant (Ksp) for Ag2SO3?
A
2.40×10⁻¹⁵
B
1.48×10⁻¹⁴
C
6.20×10⁻¹⁶
D
3.72×10⁻¹⁰
Verified step by step guidance1
Start by writing the dissociation equation for Ag2SO3 in water: Ag2SO3(s) ⇌ 2Ag⁺(aq) + SO3²⁻(aq).
Identify the stoichiometry of the dissociation: 1 mole of Ag2SO3 produces 2 moles of Ag⁺ and 1 mole of SO3²⁻.
Let the molar solubility of Ag2SO3 be 's'. Therefore, [Ag⁺] = 2s and [SO3²⁻] = s.
Substitute the molar solubility value into the expressions: [Ag⁺] = 2 × 1.55×10⁻⁵ M and [SO3²⁻] = 1.55×10⁻⁵ M.
Calculate the solubility product constant (Ksp) using the expression Ksp = [Ag⁺]²[SO3²⁻]. Substitute the concentrations to find Ksp.
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