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The solubility of Ag2SO4 in water at 25°C is 0.0155 m. What is Ksp for Ag2SO4?
18. Aqueous Equilibrium
Solubility Product Constant: Ksp
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An ionic compound with the formula Q2Z has a molar solubility of 1.01 × 10⁻² M. What is the value of Ksp for this compound?
A
1.01 × 10⁻²
B
1.02 × 10⁻⁴
C
4.12 × 10⁻⁶
D
2.04 × 10⁻⁴
Verified step by step guidance1
Understand the dissociation of the ionic compound Q2Z in water. It dissociates into 2Q⁺ ions and 1Z²⁻ ion. The balanced equation for the dissociation is: Q₂Z(s) ⇌ 2Q⁺(aq) + Z²⁻(aq).
Identify the molar solubility of the compound, which is given as 1.01 × 10⁻² M. This represents the concentration of Z²⁻ ions in the solution at equilibrium.
Determine the concentration of Q⁺ ions. Since the stoichiometry of the dissociation shows that 2 moles of Q⁺ are produced for every mole of Q₂Z that dissolves, the concentration of Q⁺ ions will be 2 × 1.01 × 10⁻² M.
Write the expression for the solubility product constant (Ksp) for the compound. The Ksp expression is: Ksp = [Q⁺]²[Z²⁻].
Substitute the concentrations of Q⁺ and Z²⁻ into the Ksp expression. Use the calculated concentrations: [Q⁺] = 2 × 1.01 × 10⁻² M and [Z²⁻] = 1.01 × 10⁻² M, and solve for Ksp.
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