Solubility product of AgCl is 2.0 x 10^-10 mol2 dm-6. Maximum Concentration of Ag+1 ions in the solution is__________________?
Correct answer: B. 1.414 x 10^-5 mol dm-3
- A. 2.0 x 10^-10 mol dm-3
- B. 1.414 x 10^-5 mol dm-3
- C. 1.0 x 10^-10 mol dm-3
- D. 1.0 x 10^-5 mol dm-3
Explanation
For AgCl(s) ⇌ Ag+ + Cl-, if the solubility is s mol dm-3, then [Ag+] = [Cl-] = s and Ksp = s2. Therefore s = square root of 2.0 x 10^-10 mol2 dm-6 = 1.414 x 10^-5 mol dm-3. The common mistake is choosing 2.0 x 10^-10 mol dm-3 by treating Ksp itself as the ion concentration.
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About Solubility Product
The solubility product constant, Ksp, represents the equilibrium concentrations of ions from a sparingly soluble salt, each raised to its stoichiometric power. Problems involve writing Ksp expressions, calculating molar solubility, applying the common-ion effect and predicting precipitation from the ionic product.
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