What is the concentration of the Ag+ ion in a saturated solution of AgCl?(Ksp for AgCl = 1.7 × 10−10)
Correct answer: C. 1.3 × 10−5 M
- A. 1.7 × 10−10 M
- B. 3.4 × 10−10 M
- C. 1.3 × 10−5 M
- D. 2.6 × 10−5 M
Explanation
The solubility product constant (Ksp) for AgCl is given by the equation Ksp = [Ag+][Cl-]. In a saturated solution of AgCl, the concentration of silver ions [Ag+] is equal to the concentration of chloride ions [Cl-]. Let this common concentration be x. Therefore, Ksp = x2. Given that Ksp = 1.7 × 10−10, we solve for x by taking the square root: x = √(1.7 × 10−10) = 1.3 × 10−5 M. This means the concentration of Ag+ ions in the saturated solution is 1.3 × 10−5 M. The other options are incorrect as they either misuse the Ksp value or misinterpret the stoichiometry of the equilibrium.
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Reversible reactions reach dynamic equilibrium when forward and reverse rates become equal, and Le Chatelier's principle predicts the effect of changing concentration, pressure or temperature. The chapter also covers solubility product, the common ion effect, buffer action and the conditions used in Haber's process, with equilibrium shifts distinguished from changes in the equilibrium constant.
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