InterviewSolution
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InterviewSolution
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If `S_(0), S_(1), S_(2)`, and `S_(3)` are the solubility of AgCI in water, `0.01M CaCI_(2), 0.01M NaCI`1, and `0.5M AgNO_(3)` solutions, respectively, then which of the following is true ?A. `S_(0)gtS_(2)gtS_(1)gtS_(3)`B. `S_(0)=S_(2)=S_(1)=S_(3)`C. `S_(3)gtS_(1)gtS_(2)gtS_(0)`D. `S_(0)gtS_(2)gtS_(3)gtS_(1)` |
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Answer» Correct Answer - A Solubility equilibrium is `AgCl(s)hArrAg^(+)(aq.)+Cl^(-)(aq.)` `K_(sp)=C_(Ag^(+))C_(Cl^(-))` The solubility of AgCI is maximum in water as there is no common ion effect. In other solutions, due to the presence of common ions, solubility is less than in pure water. The larger the concentration of common ions, the lower is the solubility. `0.01M CaCl_(2)` provides `Cl^(-)` with `C_(Cl^(-))=2(0.01M) = 0.02M` `0.01M NaCI` provides `Cl^(-)` with `C_(Cl^(-))= 0.01M` `0.5M AgNO_(3)` provides `Ag^(+)` with `C_(Ag^(+)) = 0.5M` Thus, the solubility of AgCI will be minimum in `0.5M AgNO_(3)` where the concentration of common ions is maximum. The correct order of solubility is, thus, `S_(0)gtS_(2)gtS_(1)gtS_(3)` |
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