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Chapter 16: Problem 3

Write the equilibrium equations on which the following \(K_{s p}\) expressions are based. (a) \(\left[\mathrm{Hg}_{2}{ }^{2+}\right]\left[\mathrm{Cl}^{-}\right]^{2}\) (b) \(\left[\mathrm{Pb}^{2+}\right]\left[\mathrm{CrO}_{4}^{2-}\right]\) (c) \(\left[\mathrm{Mn}^{4+}\right]\left[\mathrm{O}^{2-}\right]^{2}\) (d) \(\left[\mathrm{Al}^{3+}\right]^{2}\left[\mathrm{~S}^{2-}\right]^{3}\)

Short Answer

Expert verified
Q: Write the equilibrium equations for each given Ksp expression: a) [Hg2^2+][Cl^-]^2 b) [Pb^2+][CrO4^2-] c) [Mn^4+][O^2-]^2 d) [Al^3+]^2[S^2-]^3 A: a) Hg2Cl2(s) ⇌ Hg2^2+(aq) + 2Cl^-(aq) b) PbCrO4(s) ⇌ Pb^2+(aq) + CrO4^2-(aq) c) MnO2(s) ⇌ Mn^4+(aq) + 2O^2-(aq) d) Al2S3(s) ⇌ 2Al^3+(aq) + 3S^2-(aq)

Step by step solution

01

(a) Writing the equilibrium equation for \(\left[\mathrm{Hg}_{2}{ }^{2+}\right]\left[\mathrm{Cl}^{-}\right]^{2}\)

Begin by identifying the ions in the expression. We have Hg\(_{2}^{2+}\) and Cl\(^-\). The exponents in the expression are their respective stoichiometric coefficients from the balanced chemical equation. In this case, the equation will be: \begin{equation} \mathrm{Hg}_{2}\mathrm{Cl}_{2}(s) \rightleftharpoons \mathrm{Hg}_{2}^{2+}(aq) + 2\mathrm{Cl}^{-}(aq) \end{equation}
02

(b) Writing the equilibrium equation for \(\left[\mathrm{Pb}^{2+}\right]\left[\mathrm{CrO}_{4}^{2-}\right]\)

Identify the ions: Pb\(^{2+}\) and CrO\(_4^{2-}\). Write the balanced chemical equation based on the exponents in the expression: \begin{equation} \mathrm{PbCrO}_{4}(s) \rightleftharpoons \mathrm{Pb}^{2+}(aq) + \mathrm{CrO}_{4}^{2-}(aq) \end{equation}
03

(c) Writing the equilibrium equation for \(\left[\mathrm{Mn}^{4+}\right]\left[\mathrm{O}^{2-}\right]^{2}\)

Identify the ions: Mn\(^{4+}\) and O\(^{2-}\). Write the balanced chemical equation based on the exponents in the expression: \begin{equation} \mathrm{MnO}_{2}(s) \rightleftharpoons \mathrm{Mn}^{4+}(aq) + 2\mathrm{O}^{2-}(aq) \end{equation}
04

(d) Writing the equilibrium equation for \(\left[\mathrm{Al}^{3+}\right]^{2}\left[\mathrm{~S}^{2-}\right]^{3}\)

Identify the ions: Al\(^{3+}\) and S\(^{2-}\). Write the balanced chemical equation based on the exponents in the expression: \begin{equation} \mathrm{Al}_{2}\mathrm{S}_{3}(s) \rightleftharpoons 2\mathrm{Al}^{3+}(aq) + 3\mathrm{S}^{2-}(aq) \end{equation}

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Most popular questions from this chapter

Cadmium(II) chloride is added to a solution of potassium hydroxide with a \(\mathrm{pH}\) of \(9.62 .\left(K_{\mathrm{sp}} \mathrm{Cd}(\mathrm{OH})_{2}=2.5 \times 10^{-14}\right)\) (a) At what concentration of \(\mathrm{Cd}^{2+}\) does a precipitate first start to form? (b) Enough cadmium(II) chloride is added to make [Cd \(\left.^{2+}\right]=\) \(0.0013 M\). What is the \(\mathrm{pH}\) of the resulting solution? (c) What percentage of the original hydroxide ion is left in solution?

Fill in the blanks in the following table. (a) \(\mathrm{CoCO}_{3}\) (b) \(\mathrm{LaF}_{3}\) (c) \(\mathrm{Ba}_{3}\left(\mathrm{PO}_{4}\right)_{2}\)

Write a net ionic equation for the reaction with ammonia by which (a) \(\mathrm{Cu}(\mathrm{OH})_{2}\) dissolves. (b) \(\mathrm{Cd}^{2+}\) forms a complex ion. (c) \(\mathrm{Pb}^{2+}\) forms a precipitate.

Write the equilibrium equations on which the following \(K_{s p}\) expressions are based. (a) \(\left[\mathrm{Ca}^{2+}\right]\left[\mathrm{CO}_{3}{ }^{2-}\right]\) (b) \(\left[\mathrm{Co}^{3+}\right]\left[\mathrm{OH}^{-}\right]^{3}\) (c) \(\left[\mathrm{Ag}^{+}\right]^{2}\left[\mathrm{~S}^{2-}\right]\) (d) \(\left[\mathrm{Pb}^{2+}\right]\left[\mathrm{Cl}^{-}\right]^{2}\)

A 65-mL solution of \(0.40 \mathrm{M} \mathrm{Al}\left(\mathrm{NO}_{3}\right)_{3}\) is mixed with \(125 \mathrm{~mL}\) of \(0.17 \mathrm{M}\) iron(II) nitrate. Solid sodium hydroxide is then added without a change in volume. (a) Which will precipitate first, \(\mathrm{Al}(\mathrm{OH})_{3}\) or \(\mathrm{Fe}(\mathrm{OH})_{2} ?\) (b) What is \(\left[\mathrm{OH}^{-}\right]\) when the first compound begins to precipitate?
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