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Chapter 16: Problem 50

For which salt in each of the following groups will the solubility depend on \(\mathrm{pH}\) ? $\begin{array}{ll}{\text { a. AgF, AgCl, AgBr }} & {\text { c. } \operatorname{Sr}\left(\mathrm{NO}_{3}\right)_{2}, \operatorname{Sr}\left(\mathrm{NO}_{2}\right)_{2}} \\ {\text { b. } \mathrm{Pb}(\mathrm{OH})_{2}, \mathrm{PbCl}_{2}} & {\text { d. } \mathrm{Ni}\left(\mathrm{NO}_{3}\right)_{2}, \mathrm{Ni}(\mathrm{CN})_{2}}\end{array}$

Short Answer

Expert verified
The salts with solubility that depends on pH are AgF (Group a), Pb(OH)₂ (Group b), Sr(NO₂)₂ (Group c), and Ni(CN)₂ (Group d).

Step by step solution

01

Understand the effect of pH on solubility

pH affects a salt's solubility if the salt's anion can act as a base and react with H+ ions in the solution, or if its cation can form insoluble hydroxides that dissolve upon the addition of OH- ions.
02

Group a - Analyzing the Anions in AgF, AgCl, and AgBr

The anions in these salts are F-, Cl-, and Br-, respectively. F- is the weakest base among them and can potentially react with H+ ions. In contrast, Cl- and Br- do not significantly react with H+ ions.
03

Group a - Identifying the salt with pH-dependent solubility

Among AgF, AgCl, and AgBr, only AgF has an anion that can potentially react with H+ ions. Therefore, the solubility of AgF depends on pH.
04

Group b - Analyzing the Components of Pb(OH)2 and PbCl2

Pb(OH)2 comprises Pb2+ ions and OH- ions. Pb2+ can form insoluble hydroxides, while OH- ions that can react with H+ ions. PbCl2 is formed by the combination of Pb2+ and Cl- ions. The ions in PbCl2 do not significantly react with H+ or OH- ions.
05

Group b - Identifying the salt with pH-dependent solubility

Among Pb(OH)2 and PbCl2, only Pb(OH)2 has components that can react with H+ or OH- ions. Therefore, the solubility of Pb(OH)2 depends on pH.
06

Group c - Analyzing the Components of Sr(NO3)2 and Sr(NO2)2

Sr(NO3)2 has Sr2+ ions and NO3- ions. The anion NO3- does not react with H+ or OH- ions. Sr(NO2)2 contains Sr2+ ions and NO2- ions. The anion NO2- can react with H+ ions and act as a weak base.
07

Group c - Identifying the salt with pH-dependent solubility

Among Sr(NO3)2 and Sr(NO2)2, only Sr(NO2)2 has an anion that can significantly react with H+ ions. Therefore, the solubility of Sr(NO2)2 depends on pH.
08

Group d - Analyzing the Components of Ni(NO3)2 and Ni(CN)2

Ni(NO3)2 has Ni2+ ions and NO3- ions. The anion NO3- does not react with H+ or OH- ions. Ni(CN)2 contains Ni2+ ions and CN- ions. CN- ions can react with H+ ions as a weak base.
09

Group d - Identifying the salt with pH-dependent solubility

Among Ni(NO3)2 and Ni(CN), only Ni(CN)2 has an anion that can significantly react with H+ ions. Therefore, the solubility of Ni(CN)2 depends on pH. To summarize, the salts with solubility that depends on pH are: - AgF (Group a) - Pb(OH)2 (Group b) - Sr(NO2)2 (Group c) - Ni(CN)2 (Group d)

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Most popular questions from this chapter

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

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 \(\left(\mathrm{EDTA}^{4-}\right)\) is used as a complexing agent in chemical analysis and has the following structure: Solutions of \(\mathrm{ED} \mathrm{TA}^{4-}\) are used to treat heavy metal poisoning by removing the heavy metal in the form of a soluble complex ion. The reaction of \(\mathrm{EDTA}^{4-}\) with \(\mathrm{Pb}^{2+} \mathrm{is}\) $$\mathrm{Pb}^{2+}(a q)+\mathrm{EDTA}^{4-}(a q) \rightleftharpoons \mathrm{PbEDTA}^{2-}(a q) \quad K=1.1 \times 10^{18}$$ 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 \(\mathrm{M}\) Na_thion. Does \(\mathrm{Pb}(\mathrm{OH})_{2}\) precipitate from this solution?

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

Calculate the solubility (in moles per liter) of \(\mathrm{Fe}(\mathrm{OH})_{3}\) $\left(K_{\mathrm{sp}}=4 \times 10^{-38}\right)$ in each of the following. a. water b. a solution buffered at pH \(=5.0\) c. a solution buffered at pH\(=11.0\)

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 \(\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}^{2+}.\) $$\mathrm{Cu}^{2+}(a q)+4 \mathrm{NH}_{3}(a q) \rightleftharpoons \mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}^{2+}(a q) \qquad K_{\mathrm{overall}}=?$$
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