InterviewSolution
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InterviewSolution
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MY and `NY_(3)` two nearly insoluble salts, have the same `K_(sp)` values of `6.2xx10^(-13)` at room temperature. Which statement would be true in rearged to MY and `NY_(3)` ?A. The molar solubility of MY in water is less than that of `NY_(3)`.B. The salts MY and `NY_(3)` are more soluble in 0.5 M KY than in pure waterC. The addition of the salt of KY to solution of MY and `NY_(3)` will have no effect on their solubilitiesD. The molar solubilities of MU and `NY_(3)` in water are identical. |
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Answer» Correct Answer - A For MY, `underset(0)(MY)hArr underset(s)(M^(+))+underset(s)(Y^(-))` where, s = solubility and `K_(sp)` = solubility product. `therefore K_(sp)=[M^(+)][Y^(-)]` `K_(sp)=s^(2)` `s=sqrt(K_(sp))=sqrt(6.2xx10^(-13))=7.874xx10^(-7)` Similarly, for `NY_(3)`, `underset(0)(NY_(3))hArr underset(s)(N^(+))+underset(3s)(3Y^(-))` `therefore K_(sp)=[N^(+)][Y^(-)]^(3)=sxx(3s)^(3)` `K_(sp)=27s^(4)` `therefore s= root(4)((K_(sp))/(27))=root(4)((6.2xx10^(-13))/(27))=3.89xx10^(-4)` Therefore, molar solubility of MY in water is less than that of `NY_(3)`. |
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