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 * 10-10moldm-6, what quantity of silver was lost in the process?
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
\(2 \times 10^{-10} = d \times d= d^{2}\)
\(d = \sqrt{2\times10^{-10}}\)
= \(1.414 \times 10^{-5}moldm^{-3}\)
Contributions ({{ comment_count }})
Please wait...
Modal title
Report
Block User
{{ feedback_modal_data.title }}