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
jamb 2000chemistry

The correct answer is D. 1.414 * 10-5mol dm-3

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

\(2 \times 10^{-10} = d \times d= d^{2}\)

\(d = \sqrt{2\times10^{-10}}\)

= \(1.414 \times 10^{-5}moldm^{-3}\)

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