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Chapter 16: Problem 23

Write balanced equations for the dissolution reactions and the corresponding solubility product expressions for each of the following solids. a. \(A g C_{2} H_{3} O_{2}\) b. \(A l(O H)_{3}\) c. \(C a_{3}\left(\mathrm{PO}_{4}\right)_{2}\)

Short Answer

Expert verified
a. Dissolution reaction: \(AgC_2H_3O_2 (s) \rightleftharpoons Ag^+ (aq) + C_2H_3O_2^- (aq)\); Solubility product expression: \(K_{sp}(AgC_2H_3O_2) = [Ag^+] [C_2H_3O_2^-]\) b. Dissolution reaction: \(Al(OH)_3 (s) \rightleftharpoons Al^{3+} (aq) + 3OH^- (aq)\); Solubility product expression: \(K_{sp}(Al(OH)_3) = [Al^{3+}] [OH^-]^3\) c. Dissolution reaction: \(Ca_3(PO_4)_2 (s) \rightleftharpoons 3Ca^{2+} (aq) + 2PO_4^{3-} (aq)\); Solubility product expression: \(K_{sp}(Ca_3(PO_4)_2) = [Ca^{2+}]^3 [PO_4^{3-}]^2\)

Step by step solution

01

Write the dissolution reaction for \(AgC_2H_3O_2\)

Dissolve the solid into its individual ions. \(AgC_2H_3O_2 (s) \rightleftharpoons Ag^+ (aq) + C_2H_3O_2^- (aq)\).
02

Write the solubility product expression for \(AgC_2H_3O_2\)

Write the solubility product constant from the given equation as follows: \(K_{sp}(AgC_2H_3O_2) = [Ag^+] [C_2H_3O_2^-]\)
03

Write the dissolution reaction for \(Al(OH)_3\)

Dissolve the aluminum hydroxide into its individual ions. \(Al(OH)_3 (s) \rightleftharpoons Al^{3+} (aq) + 3OH^- (aq)\)
04

Write the solubility product expression for \(Al(OH)_3\)

Write the solubility product constant from the given equation as follows: \(K_{sp}(Al(OH)_3) = [Al^{3+}] [OH^-]^3\)
05

Write the dissolution reaction for \(Ca_3(PO_4)_2\)

Dissolve the calcium phosphate into its individual ions. \(Ca_3(PO_4)_2 (s) \rightleftharpoons 3Ca^{2+} (aq) + 2PO_4^{3-} (aq)\)
06

Write the solubility product expression for \(Ca_3(PO_4)_2\)

Write the solubility product constant from the given equation as follows: \(K_{sp}(Ca_3(PO_4)_2) = [Ca^{2+}]^3 [PO_4^{3-}]^2\)

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Most popular questions from this chapter

In the presence of \(\mathrm{NH}_{3}, \mathrm{Cu}^{2+}\) forms the complex ion \(\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}^{2+} .\) If the equilibrium concentrations of \(\mathrm{Cu}^{2+}\) and \(\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}^{2+}\) are $1.8 \times 10^{-17} \mathrm{M}\( and \)1.0 \times 10^{-3} \mathrm{M},\( respectively, in a \)1.5-M \mathrm{NH}_{3}$ solution, calculate the value for the overall formation constant of \(\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}^{2+}.\) $$\mathrm{Cu}^{2+}(a q)+4 \mathrm{NH}_{3}(a q) \rightleftharpoons \mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}^{2+}(a q) \qquad K_{\mathrm{overall}}=?$$

When 100.0 \(\mathrm{mL}\) of 2.00 $\mathrm{M} \mathrm{Ce}\left(\mathrm{NO}_{3}\right)_{3}\( is added to 100.0 \)\mathrm{mL}$ of \(3.00 \mathrm{M} \mathrm{KIO}_{3},\) a precipitate of \(\mathrm{Ce}\left(\mathrm{IO}_{3}\right)_{3}(s)\) forms. Calculate the equilibrium concentrations of \(\mathrm{Ce}^{3+}\) and \(\mathrm{IO}_{3}^{-}\) in this solution. $\left[K_{\mathrm{sp}} \text { for } \mathrm{Ce}\left(\mathrm{IO}_{3}\right)_{3}=3.2 \times 10^{-10} .\right]$

When aqueous KI is added gradually to mercury (II) nitrate, an orange precipitate forms. Continued addition of KI causes the precipitate to dissolve. Write balanced equations to explain these observations. (Hint: \(\mathrm{Hg}^{2+}\) reacts with \(\mathrm{I}^{-}\) to form \(\mathrm{HgI}_{4}^{2-}.)\)

As sodium chloride solution is added to a solution of silver nitrate, a white precipitate forms. Ammonia is added to the mixture and the precipitate dissolves. When potassium bromide solution is then added, a pale yellow precipitate appears. When a solution of sodium thiosulfate is added, the yellow precipitate dissolves. Finally, potassium iodide is added to the solution and a yellow precipitate forms. Write equations for all the changes mentioned above. What conclusions can you draw concerning the sizes of the \(K_{\mathrm{sp}}\) values for \(\mathrm{AgCl}, \mathrm{AgBr},\) and \(\mathrm{AgI?}\)

Which of the following will affect the total amount of solute that can dissolve in a given amount of solvent? a. The solution is stirred. b. The solute is ground to fine particles before dissolving. c. The temperature changes
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