AP Chemistrymediummcq1 pt
Ksp of AgCl is 1.8 × 10⁻¹⁰. What is the molar solubility of AgCl in a 0.10 M NaCl solution?
A.1.3 × 10^-5 M
B.1.8 × 10^-9 M
C.1.8 × 10^-11 M
D.1.8 × 10^-10 M
Explanation
Core Concept
Dissolved NaCl pins [Cl⁻] at 0.10 M, a classic common-ion situation. The product rule demands [Ag⁺][Cl⁻] = 1.8 × 10⁻¹⁰, so [Ag⁺] = 1.8 × 10⁻¹⁰ ÷ 0.10 = 1.8 × 10⁻⁹ M. Each dissolved formula unit delivers exactly one silver ion, making this the molar solubility. Compared with pure water, the added chloride suppresses solubility roughly 7000-fold.
Correct Answer
B1.8 × 10^-9 M
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