WBJEE · Chemistry · Ionic Equilibrium
A solution is saturated with \(\mathrm{SrCO}_{3}\) and \(\mathrm{Sr} \mathrm{F}_{2}\). The \(\left[\mathrm{CO}_{3}^{2-}\right]\) is found to be \(1.2 \times 10^{-3} \mathrm{M}\). The concentration of \(\mathrm{F}\) - in the solution would be
- A \(3.7 \times 10^{-6} \mathrm{M}\)
- B \(3.2 \times 10^{-3} \mathrm{M}\)
- C \(5.1 \times 10^{-7} \mathrm{M}\)
- D \(3.7 \times 10^{-2} \mathrm{M}\)
Given : \(\mathrm{K}_{\mathrm{sp}}\left(\mathrm{SrCO}_{3}\right)=7.0 \times 10^{-10}, \mathrm{~K}_{\mathrm{sp}}\left(\mathrm{SrF}_{2}\right)=7.9 \times 10^{-10}\)
Answer & Solution
Correct Answer
(D) \(3.7 \times 10^{-2} \mathrm{M}\)
Given : \(\mathrm{K}_{\mathrm{sp}}\left(\mathrm{SrCO}_{3}\right)=7.0 \times 10^{-10}, \mathrm{~K}_{\mathrm{sp}}\left(\mathrm{SrF}_{2}\right)=7.9 \times 10^{-10}\)
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