STANDARDChemistry-Ionic Equilibrium
STANDARD Chemistry Solubility Product MCQ Question
Type: MCQ-numerical-Medium-Class 11
What is the pH at which Mg(OH)₂ begins to precipitate from a solution containing 0.1 M Mg²⁺ ions? [Kₛₚ for Mg(OH)₂ = 1.0 × 10⁻¹¹]
A
10
B
9
C
8
D
7
Correct Answer
Option B
Detailed Explanation
The solubility product expression for Mg(OH)₂ is [Mg²⁺][OH⁻]² = 1.0 × 10⁻¹¹. Given [Mg²⁺] = 0.1 M, we find [OH⁻] = 10⁻⁵ M. The pOH is 5, so the pH is 9.
Found an issue with this question?
Related Questions
More from
Which of the following will produce a buffer solution when mixed in equal volumes?
EquilibriumChemistry
What is the equilibrium constant for the ionization of a weak base represented as MOH in aqueous solution?
Chemical EquilibriumChemistry
Assertion (A): The pH of a buffer solution containing equal concentrations of ammonia and ammonium chloride is equal to the pKa of ammonia. | Reason (...
pH & Buffer SolutionsChemistry