At $25 \, ^\circ C$,the $K_{sp}$ of $CaF_2$ is $1.7 \times 10^{-10}$. Which of the following combinations will result in the precipitation of $CaF_2$?
- A$1 \times 10^{-2} \, M \, Ca^{2+}$ and $1 \times 10^{-5} \, M \, F^{-}$
- B$1 \times 10^{-4} \, M \, Ca^{2+}$ and $1 \times 10^{-4} \, M \, F^{-}$
- C$1 \times 10^{-3} \, M \, Ca^{2+}$ and $1 \times 10^{-5} \, M \, F^{-}$
- D$1 \times 10^{-2} \, M \, Ca^{2+}$ and $1 \times 10^{-3} \, M \, F^{-}$
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The values of $K_{sp}$ of $CaCO_{3}$ and $CaC_{2}O_{4}$ are $4.7 \times 10^{-9}$ and $1.3 \times 10^{-9}$ respectively at $25 \, ^oC$. If the mixture of these two is washed with water,what is the concentration of $Ca^{2+}$ ions in water $\dots \times 10^{-5} \, M$?
Concentration of $H_2SO_4$ and $Na_2SO_4$ in a solution is $1 \ M$ and $1.8 \times 10^{-2} \ M$,respectively. Molar solubility of $PbSO_4$ in the same solution is $X \times 10^{-Y} \ M$ (expressed in scientific notation). The value of $Y$ is. . . .
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[Given: Solubility product of $PbSO_4$ $(K_{sp})=1.6 \times 10^{-8}$. For $H_2SO_4$,$K_{a1}$ is very large and $K_{a2}=1.2 \times 10^{-2}$]
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