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Chapter 16: Problem 24

Write balanced equations for the dissolution reactions and the corresponding solubility product expressions for each of the following solids a. \(\mathrm{Ag}_{2} \mathrm{CO}_{3}\) b. \(\mathrm{Ce}\left(\mathrm{IO}_{3}\right)_{3}\) c. \(\mathrm{BaF}_{2}\)

Short Answer

Expert verified
a. Dissolution: \(\mathrm{Ag}_{2} \mathrm{CO}_{3} \rightleftharpoons 2 \mathrm{Ag^+} + \mathrm{CO^{2-}_3}\), Solubility product: \(K_{sp} = [\mathrm{Ag^+}]^2 [\mathrm{CO^{2-}_3}]\) b. Dissolution: \(\mathrm{Ce}\left(\mathrm{IO}_{3}\right)_{3} \rightleftharpoons \mathrm{Ce^{3+}} + 3 \mathrm{IO^{-}_3}\), Solubility product: \(K_{sp} = [\mathrm{Ce^{3+}}] [\mathrm{IO^{-}_3}]^3\) c. Dissolution: \(\mathrm{BaF}_{2} \rightleftharpoons \mathrm{Ba^{2+}} + 2 \mathrm{F^{-}}\), Solubility product: \(K_{sp} = [\mathrm{Ba^{2+}}] [\mathrm{F^{-}]^2\)

Step by step solution

01

Write balanced equations for the dissolution reactions

We will write balanced equations for the dissolution reactions of the given solids: a. \(\mathrm{Ag}_{2} \mathrm{CO}_{3}\) \(\mathrm{Ag}_{2} \mathrm{CO}_{3} \rightleftharpoons 2 \mathrm{Ag^+} + \mathrm{CO^{2-}_3}\) b. \(\mathrm{Ce}\left(\mathrm{IO}_{3}\right)_{3}\) \(\mathrm{Ce}\left(\mathrm{IO}_{3}\right)_{3} \rightleftharpoons \mathrm{Ce^{3+}} + 3 \mathrm{IO^{-}_3}\) c. \(\mathrm{BaF}_{2}\) \(\mathrm{BaF}_{2} \rightleftharpoons \mathrm{Ba^{2+}} + 2 \mathrm{F^{-}}\)
02

Write the solubility product expressions

Now we will write the corresponding solubility product expressions for each equation: a. \(\mathrm{Ag}_{2} \mathrm{CO}_{3}\) \(K_{sp} = [\mathrm{Ag^+}]^2 [\mathrm{CO^{2-}_3}]\) b. \(\mathrm{Ce}\left(\mathrm{IO}_{3}\right)_{3}\) \(K_{sp} = [\mathrm{Ce^{3+}}] [\mathrm{IO^{-}_3}]^3\) c. \(\mathrm{BaF}_{2}\) \(K_{sp} = [\mathrm{Ba^{2+}}] [\mathrm{F^{-}]^2\)

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Most popular questions from this chapter

The \(K_{\mathrm{sp}}\) for silver sulfate $\left(\mathrm{Ag}_{2} \mathrm{SO}_{4}\right)\( is \)1.2 \times 10^{-5} .$ Calculate the solubility of silver sulfate in each of the following. a. water b. \(0.10M\) \(\mathrm{AgNO}_{3}\) c. \(0.20M\) \(\mathrm{K}_{2} \mathrm{SO}_{4}\)

Calculate the solubility of each of the following compounds in moles per liter. Ignore any acid–base properties. a. \(P b I_{2}, K_{s p}=1.4 \times 10^{-8}\) b. \(\operatorname{CdCO}_{3}, K_{s p}=5.2 \times 10^{-12}\) c. $\operatorname{Sr}_{3}\left(\mathrm{PO}_{4}\right)_{2}, K_{s p}=1 \times 10^{-31}$

The equilibrium constant for the following reaction is \(1.0 \times 10^{23} :\) $$\mathrm{Cr}^{3+}(a q)+\mathrm{H}_{2} \mathrm{EDTA}^{2-}(a q) \rightleftharpoons \mathrm{CrEDTA}^{-}(a q)+2 \mathrm{H}^{+}(a q)$$ EDTA is used as a complexing agent in chemical analysis. Solutions of EDTA, usually containing the disodium salt $\mathrm{Na}_{2} \mathrm{H}_{2} \mathrm{EDTA}$ , are used to treat heavy metal poisoning. Calculate \(\left[\mathrm{Cr}^{3+}\right]\) at equilibrium in a solution originally \(0.0010 M\) in \(\mathrm{Cr}^{3+}\) and \(0.050 M\) in $\mathrm{H}_{2} \mathrm{EDTA}^{2-}\( and buffered at \)\mathrm{pH}=6.00.$

A mixture contains \(1.0 \times 10^{-3} M \mathrm{Cu}^{2+}\) and $1.0 \times 10^{-3} M$ \(\mathrm{Mn}^{2+}\) and is saturated with 0.10\(M \mathrm{H}_{2} \mathrm{S} .\) Determine a pH where CuS precipitates but MnS does not precipitate. \(K_{\mathrm{sp}}\) for \(\mathrm{CuS}=8.5 \times 10^{-45}\) and $K_{\mathrm{sp}} \mathrm{for} \mathrm{MnS}=2.3 \times 10^{-13} .$

The common ion effect for ionic solids (salts) is to significantly decrease the solubility of the ionic compound in water. Explain the common ion effect.
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