InterviewSolution
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InterviewSolution
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The electrochemical cell shown below is a concentration cell. `M|M^(2+)(` saturated solution of sparingly soluble salt, `MX_(2))||M^(2+)(0.001 mol dm^(-3))|M` The `emf` of the cell depends on the difference in the concentration of `M^(2+)` ions at the two electrodes. The `emf` of the cell at `298` is `0.059V`. The solubility product `(K_(sp),mol^(3) dm^(-9))` of `MX_(2)` at 298 based on the information available the given concentration cell is `(` Take `2.303xxRxx298//F=0.059V)`A. `1xx10^(-15)`B. `4xx10^(-15)`C. `1xx10^(-12)`D. `4xx10^(-12)` |
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Answer» Correct Answer - B `M|underset((K_(sp) =?))(M^(+)(sat.))"||"M^(2+) (0.001M)` emf of concentration cell, `E_(cell) = (-0.059)/(n)log. ([M^(+2)]_(a))/([M^(+2)]_(c))` `0.059 = (0.059)/(2)log. ([0.001])/([M^(+2)]_(a))` `[M^(+2)]_(a) = 10^(5) = S` (solubility of salt in saturated solution) `underset((S))(MX_(2))rarr underset((S))(M^(+2)) +underset((2S))(2x^(-)(aq))` `K_(sp) = 4S^(3) = 4 xx (10^(-5))^(3) = 4 xx 10^(-15)` |
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