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: Option 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{2times10^{-10}})
= (1.414 times 10^{-5}moldm^{-3})