What is the H⁺ ion concentration in a 2.1 × 10^-4 M Ca(OH)₂ solution?

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Quizplus · Accepted Answer

Ca(OH)₂ is a strong base, so it will dissociate completely in water to form Ca²⁺ and OH^- ions. The OH^- ions will then react with water to form H₂O and OH^- ions. The equilibrium constant for this reaction is 1.0 × 10^-14, so the concentration of H⁺ ions in the solution will be:[H⁺] = 1.0 × 10^-14/[OH^-]²The concentration of OH^- ions in the solution is:[OH^-] = 2 × [Ca(OH)₂] = 2 × 2.1 × 10^-4 M = 4.2 × 10^-4 MTherefore, the concentration of H⁺ ions in the solution is:[H⁺] = 1.0 × 10^-14/(4.2 × 10^-4 M)² = 2.4 × 10^-11 M

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