1.0 dm3 of distilled water was used to wash 2.0g of a precipitate of AgCl. If the solubility product of AgCl is 2.0 * 10-10mol2dm-6, what quantity of silver was lost in the process?
A. 2.029 * 10-3mol dm-3 B. 1.414 * 10-3mol dm-3 C. 2.029 * 10-5mol dm-3 D. 1.414 * 10-5mol dm-3
Correct Answer: D
Explanation
In order to calculate this, it suffices to calculate the solubility of Ag, so as to know the amount lost. \(K_{sp} = [Ag^{+}][Cl^{-}]\) Let the solubilty of Ag and Cl = d \(2 \times 10^{-10} = d \times d= d^{2}\) \(d = \sqrt{2\times10^{-10}}\) = \(1.414 \times 10^{-5}moldm^{-3}\) Â
