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Chapter 16: Problem 19

Write balanced equations for the dissolution reactions and the corresponding solubility product expressions for each of the following solids. a. \(\mathrm{AgC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\) b. \(\mathrm{Al}(\mathrm{OH})_{3}\) c. \(\mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2}\)

Short Answer

Expert verified
a) Dissolution reaction of \(\mathrm{AgC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\): \(\mathrm{AgC}_{2} \mathrm{H}_{3} \mathrm{O}_{2(s)} \rightleftharpoons \mathrm{Ag}^{+} _{\mathrm{(aq)}} + \mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}^{-} _{\mathrm{(aq)}}\); Solubility product expression: \(K_\mathrm{sp} = [\mathrm{Ag}^{+}] [\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}^{-}]\) b) Dissolution reaction of \(\mathrm{Al}(\mathrm{OH})_{3}\): \(\mathrm{Al}(\mathrm{OH})_{3(s)} \rightleftharpoons \mathrm{Al}^{3+}_{\mathrm{(aq)}} + 3\mathrm{OH}^{-}_{\mathrm{(aq)}}\); Solubility product expression: \(K_\mathrm{sp} = [\mathrm{Al}^{3+}][\mathrm{OH}^{-}]^{3}\) c) Dissolution reaction of \(\mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2}\): \(\mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2(s)} \rightleftharpoons 3\mathrm{Ca}^{2+}_{\mathrm{(aq)}} + 2\mathrm{PO}_{4}^{3-}_{\mathrm{(aq)}}\); Solubility product expression: \(K_\mathrm{sp} = [\mathrm{Ca}^{2+}]^{3}[\mathrm{PO}_{4}^{3-}]^{2}\)

Step by step solution

01

a) Dissolution reaction of \(\mathrm{AgC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\)#

To write the balanced equation for the dissolution of silver acetate \(\mathrm{AgC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\), we can dissociate the solid into its ionic species: \(\mathrm{AgC}_{2} \mathrm{H}_{3} \mathrm{O}_{2(s)} \rightleftharpoons \mathrm{Ag}^{+} _{\mathrm{(aq)}} + \mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}^{-} _{\mathrm{(aq)}}\)
02

a) Solubility product expression of \(\mathrm{AgC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\)#

For the solubility product (\(K_\mathrm{sp}\)) expression, we can define the equilibrium constant for the dissolution reaction by multiplying the concentrations of the ions in their aqueous state: \(K_\mathrm{sp} = [\mathrm{Ag}^{+}] [\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}^{-}]\)
03

b) Dissolution reaction of \(\mathrm{Al}(\mathrm{OH})_{3}\)#

To write the balanced equation for the dissolution of aluminium hydroxide \(\mathrm{Al}(\mathrm{OH})_{3}\), we can dissociate the solid into its ionic species: \(\mathrm{Al}(\mathrm{OH})_{3(s)} \rightleftharpoons \mathrm{Al}^{3+}_{\mathrm{(aq)}} + 3\mathrm{OH}^{-}_{\mathrm{(aq)}}\)
04

b) Solubility product expression of \(\mathrm{Al}(\mathrm{OH})_{3}\)#

For the solubility product (\(K_\mathrm{sp}\)) expression, we can define the equilibrium constant for the dissolution reaction by multiplying the concentrations of the ions in their aqueous state: \(K_\mathrm{sp} = [\mathrm{Al}^{3+}][\mathrm{OH}^{-}]^{3}\)
05

c) Dissolution reaction of \(\mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2}\)#

To write the balanced equation for the dissolution of calcium phosphate \(\mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2}\), we can dissociate the solid into its ionic species: \(\mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2(s)} \rightleftharpoons 3\mathrm{Ca}^{2+}_{\mathrm{(aq)}} + 2\mathrm{PO}_{4}^{3-}_{\mathrm{(aq)}}\)
06

c) Solubility product expression of \(\mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2}\)#

For the solubility product (\(K_\mathrm{sp}\)) expression, we can define the equilibrium constant for the dissolution reaction by multiplying the concentrations of the ions in their aqueous state: \(K_\mathrm{sp} = [\mathrm{Ca}^{2+}]^{3}[\mathrm{PO}_{4}^{3-}]^{2}\)

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Most popular questions from this chapter

In the presence of \(\mathrm{CN}^{-}, \mathrm{Fe}^{3+}\) forms the complex ion \(\mathrm{Fe}(\mathrm{CN})_{6}^{3-}\). The equilibrium concentrations of \(\mathrm{Fe}^{3+}\) and \(\mathrm{Fe}(\mathrm{CN})_{6}^{3-}\) are \(8.5 \times 10^{-40} M\) and \(1.5 \times 10^{-3} M\), respectively, in a \(0.11 M \mathrm{KCN}\) solution. Calculate the value for the overall formation constant of \(\mathrm{Fe}(\mathrm{CN})_{6}^{3-}\) $$\mathrm{Fe}^{3+}(a q)+6 \mathrm{CN}^{-}(a q) \rightleftharpoons \mathrm{Fe}(\mathrm{CN})_{6}{ }^{3-} \quad K_{\text {overall }}=?$$

The solubility of the ionic compound \(\mathrm{M}_{2} \mathrm{X}_{3}\), having a molar mass of \(288 \mathrm{~g} / \mathrm{mol}\), is \(3.60 \times 10^{-7} \mathrm{~g} / \mathrm{L}\). Calculate the \(K_{\mathrm{sp}}\) of the compound.

A solution is prepared by adding \(0.10 \mathrm{~mol} \mathrm{Ni}\left(\mathrm{NH}_{3}\right)_{6} \mathrm{Cl}_{2}\) to \(0.50 \mathrm{~L}\) of \(3.0 \mathrm{M} \mathrm{NH}_{3} .\) Calculate \(\left[\mathrm{Ni}\left(\mathrm{NH}_{3}\right)_{6}^{2+}\right]\) and \(\left[\mathrm{Ni}^{2+}\right]\) in this solution. \(K_{\text {owerall }}\) for \(\mathrm{Ni}\left(\mathrm{NH}_{3}\right)_{6}^{2+}\) is \(5.5 \times 10^{8} .\) That is, $$5.5 \times 10^{\mathrm{x}}=\frac{\left[\mathrm{Ni}\left(\mathrm{NH}_{3}\right)_{6}^{2+}\right]}{\left[\mathrm{Ni}^{2+}\right]\left[\mathrm{NH}_{3}\right]^{6}}$$ for the overall reaction $$\mathrm{Ni}^{2+}(a q)+6 \mathrm{NH}_{3}(a q) \rightleftharpoons \mathrm{Ni}\left(\mathrm{NH}_{3}\right)_{6}^{2+}(a q)$$

Calculate the molar solubility of \(\mathrm{Al}(\mathrm{OH})_{3}, K_{s p}=2 \times 10^{-32}\).

What mass of \(\mathrm{ZnS}\left(K_{\text {? }}=2.5 \times 10^{-22}\right.\) ) 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 \(\mathrm{S}^{2-}\) .
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