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Chapter 15: Problem 20

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
\(a. \mathrm{Ag}_{2}\mathrm{CO}_{3}\left(s\right) \longleftrightarrow 2\mathrm{Ag}^{+}\left(aq\right) + \mathrm{CO}_{3}^{2-}\left(aq\right)\), \(\mathrm{K}_{sp} = [\mathrm{Ag}^{+}]^2[\mathrm{CO}_{3}^{2-}]\) \(b. \mathrm{Ce}\left(\mathrm{IO}_{3}\right)_3\left(s\right) \longleftrightarrow \mathrm{Ce}^{3+}\left(aq\right) + 3\mathrm{IO}_3^-\left(aq\right)\), \(\mathrm{K}_{sp} = [\mathrm{Ce}^{3+}][\mathrm{IO}_{3}^{-}]^3\) \(c. \mathrm{BaF}_{2}\left(s\right) \longleftrightarrow \mathrm{Ba}^{2+}\left(aq\right) + 2\mathrm{F}^{-}\left(aq\right)\), \(\mathrm{K}_{sp} = [\mathrm{Ba}^{2+}][\mathrm{F}^{-}]^2\)

Step by step solution

01

a. Solve for Silver Carbonate (\(\mathrm{Ag}_{2} \mathrm{CO}_{3}\))

Step 1: Write the dissociation/dissolution reaction of the given solid. Silver Carbonate will dissociate into Silver ions and Carbonate ions: \(\mathrm{Ag}_{2}\mathrm{CO}_{3}\left(s\right) \longleftrightarrow 2\mathrm{Ag}^{+}\left(aq\right) + \mathrm{CO}_{3}^{2-}\left(aq\right)\) Step 2: Write the solubility product expression. The solubility product expression for Silver Carbonate is: \(\mathrm{K}_{sp} = [\mathrm{Ag}^{+}]^2[\mathrm{CO}_{3}^{2-}]\)
02

b. Solve for Cerium(III) Iodate (\(\mathrm{Ce}\left(\mathrm{IO}_{3}\right)_{3}\))

Step 1: Write the dissociation/dissolution reaction of the given solid. Cerium(III) Iodate dissociates into Cerium ions and Iodate ions: \(\mathrm{Ce}\left(\mathrm{IO}_{3}\right)_3\left(s\right) \longleftrightarrow \mathrm{Ce}^{3+}\left(aq\right) + 3\mathrm{IO}_3^-\left(aq\right)\) Step 2: Write the solubility product expression. The solubility product expression for Cerium(III) Iodate is: \(\mathrm{K}_{sp} = [\mathrm{Ce}^{3+}][\mathrm{IO}_{3}^{-}]^3\)
03

c. Solve for Barium Fluoride (\(\mathrm{BaF}_{2}\))

Step 1: Write the dissociation/dissolution reaction of the given solid. Barium Fluoride dissociates into Barium ions and Fluoride ions: \(\mathrm{BaF}_{2}\left(s\right) \longleftrightarrow \mathrm{Ba}^{2+}\left(aq\right) + 2\mathrm{F}^{-}\left(aq\right)\) Step 2: Write the solubility product expression. The solubility product expression for Barium Fluoride is: \(\mathrm{K}_{sp} = [\mathrm{Ba}^{2+}][\mathrm{F}^{-}]^2\)

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Most popular questions from this chapter

What mass of ZnS \(\left(K_{\mathrm{sp}}=2.5 \times 10^{-22}\right)\) will dissolve in \(300.0 \mathrm{mL}\) of \(0.050 \mathrm{M} \mathrm{Zn}\left(\mathrm{NO}_{3}\right)_{2} ?\) Ignore the basic properties of \(\mathrm{S}^{2-}\).

A solution contains \(1.0 \times 10^{-5} M \mathrm{Ag}^{+}\) and \(2.0 \times 10^{-6} M \mathrm{CN}^{-}\) Will AgCN( \(s\) ) precipitate? \(\left(K_{\mathrm{sp}} \text { for } \mathrm{AgCN}(s) \text { is } 2.2 \times 10^{-12} .\right)\)

Calculate the molar solubility of \(\mathrm{Mg}(\mathrm{OH})_{2}, K_{\mathrm{sp}}=8.9 \times 10^{-12}\).

Calculate the concentration of \(\mathrm{Pb}^{2+}\) in each of the following. a. a saturated solution of \(\mathrm{Pb}(\mathrm{OH})_{2}, K_{\mathrm{sp}}=1.2 \times 10^{-15}\) b. a saturated solution of \(\mathrm{Pb}(\mathrm{OH})_{2}\) buffered at \(\mathrm{pH}=13.00\) c. Ethylenediaminetetraacetate (EDTA \(^{4-}\) ) is used as a complexing agent in chemical analysis and has the following structure: Solutions of EDTA \(^{4-}\) are used to treat heavy metal poisoning by removing the heavy metal in the form of a soluble complex ion. The reaction of EDTA \(^{4-}\) with \(\mathrm{Pb}^{2+}\) is $$\begin{aligned} \mathrm{Pb}^{2+}(a q)+\mathrm{EDTA}^{4-}(a q) \rightleftharpoons \mathrm{PbEDTA}^{2-}(a q) & \\ K &=1.1 \times 10^{18} \end{aligned}$$ Consider a solution with 0.010 mole of \(\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}\) added to \(1.0 \mathrm{L}\) of an aqueous solution buffered at \(\mathrm{pH}=13.00\) and containing 0.050 \(M\) \(\mathrm{Na}_{4} \mathrm{EDTA}\). Does \(\mathrm{Pb}(\mathrm{OH})_{2}\) precipitate from this solution?

The solubility of \(\mathrm{Ce}\left(\mathrm{IO}_{3}\right)_{3}\) in a \(0.20-M\) KIO \(_{3}\) solution is \(4.4 \times 10^{-8} \mathrm{mol} / \mathrm{L} .\) Calculate \(K_{\mathrm{sp}}\) for \(\mathrm{Ce}\left(\mathrm{IO}_{3}\right)_{3}\).
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