Multiple Choice
Calculate the solubility (in grams per 1.00×10^2 mL of solution) of magnesium hydroxide in a solution buffered at pH = 12 given that the Ksp for Mg(OH)2 is 2.06×10^(-13).
224
views
18. Aqueous Equilibrium
Solubility Product Constant: Ksp
Multiple Choice
Which of the following is the correct Kₛₚ expression for the dissolution of Sr₃(PO₄)₂ in water?
A
Kₛₚ = [Sr²⁺]²[PO₄³⁻]³
B
Kₛₚ = [Sr²⁺]²[PO₄³⁻]²
C
Kₛₚ = [Sr²⁺][PO₄³⁻]
D
Kₛₚ = [Sr²⁺]³[PO₄³⁻]²
Verified step by step guidance1
First, understand that the solubility product constant (Kₛₚ) is used to describe the equilibrium between a solid and its ions in a saturated solution. It is specific to sparingly soluble salts.
Next, write the balanced chemical equation for the dissolution of Sr₃(PO₄)₂ in water: Sr₃(PO₄)₂(s) ⇌ 3Sr²⁺(aq) + 2PO₄³⁻(aq). This shows the stoichiometry of the ions produced.
From the balanced equation, identify the stoichiometric coefficients of the ions: 3 for Sr²⁺ and 2 for PO₄³⁻. These coefficients will be used as exponents in the Kₛₚ expression.
Construct the Kₛₚ expression using the concentrations of the ions raised to the power of their stoichiometric coefficients: Kₛₚ = [Sr²⁺]³[PO₄³⁻]².
Verify that the Kₛₚ expression matches the stoichiometry of the dissolution reaction, ensuring that the exponents correspond to the number of ions produced in the balanced equation.
Related Videos
Related Practice
