Question
What $\left[\mathrm{F}^{-}\right]$ is required to reduce $\left[\mathrm{Ca}^{2+}\right]$ to $1.0 \times 10^{-4} \mathrm{M}$ by precipitation of $\mathrm{CaF}_{2} ?$
Step 1
Step 1: We are given the dissolution equation of calcium fluoride as follows: \[CaF_{2} \rightarrow Ca^{2+} + 2F^{-}\] The solubility product constant, $K_{sp}$, for this reaction is given by: \[K_{sp} = [Ca^{2+}][F^{-}]^{2}\] Show more…
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Calculate the concentration of $\mathrm{F}$ - required to begin precipitation of CaF_{in a solution that is } 0 . 0 1 0 \mathrm { M } \text { in } \mathrm { Ca } ^ { 2 + } .
What mass of $\mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}$ must be added to $1.0 \mathrm{~L}$ of a $1.0-M \mathrm{HF}$ solution to begin precipitation of $\mathrm{CaF}_{2}(s) ?$ For $\mathrm{CaF}_{2}, K_{\mathrm{sp}}=$ $4.0 \times 10^{-11}$ and $K_{u}$ for $\mathrm{HF}=7.2 \times 10^{-4} .$ Assume no volume change on addition of $\mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}(s)$.
What mass of $\mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}$ must be added to 1.0 $\mathrm{L}$ of a $1.0-M \mathrm{HF}$ solution to begin precipitation of $\mathrm{CaF}_{2}(s) ?$ For $\mathrm{CaF}_{2}, K_{\mathrm{sp}}= 4.0 \times 10^{-11}$ and $K_{\mathrm{a}}$ for $\mathrm{HF}=7.2 \times 10^{-4}$ . Assume no volume change on addition of $\mathrm{Ca}\left(\mathrm{NO}_{3}\right)_{2}(s).$
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