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Chapter 18: Problem 51

\(\mathrm{PbCl}_{2}(\mathrm{s})\) is considerably more soluble in \(\mathrm{HCl}(\mathrm{aq})\) than in pure water, but its solubility in \(\mathrm{HNO}_{3}(\mathrm{aq})\) is not much different from what it is in water. Explain this difference in behavior.

Short Answer

Expert verified
The increased solubility of PbCl2 in HCl is due to the increase in Cl- ions from HCl dissociation leading to the common ion effect, which shifts the equilibrium to favor the formation of more PbCl2. However, because HNO3 does not contain a common ion (Cl-) with PbCl2, it doesn't significantly affect its solubility, hence its solubility remains similar to that in water.

Step by step solution

01

Analyze the solubility of PbCl2

Lead chloride, PbCl2 is sparingly soluble in water. When dissolved, it dissociates into Pb2+ ions and Cl- ions. The equilibrium can be represented as: \(PbCl2 \leftrightarrow Pb^{2+} + 2Cl^{-}\)
02

Explain the solubility in HCl solution

When PbCl2 is in solution with HCl, it will increase the concentration of Cl- ions since HCl dissociates completely in water to give H+ and Cl-. This high concentration of Cl- shifts the PbCl2 dissolution equilibrium to left (Common ion effect), and favors the formation of more PbCl2, thus increases its solubility.
03

Explain the solubility in HNO3 solution

HNO3 does not contain the Cl- ion. Therefore, adding HNO3 to the solution doesn't add more common ions, from Le Chatelier's principle, it will not influence the dissolution equilibrium of PbCl2 as much. Hence, its solubility in HNO3 is not much different from what it is in water.

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Most popular questions from this chapter

Will \(\mathrm{PbCl}_{2}(\mathrm{s})\) precipitate when \(155 \mathrm{mL}\) of \(0.016 \mathrm{M}\) \(\mathrm{KCl}(\mathrm{aq})\) are added to \(245 \mathrm{mL}\) of \(0.175 \mathrm{M}\) \(\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2}(\mathrm{aq}) ?\)

Will precipitation of \(\mathrm{MgF}_{2}(\mathrm{s})\) occur if a \(22.5 \mathrm{mg}\) sample of \(\mathrm{MgCl}_{2} \cdot 6 \mathrm{H}_{2} \mathrm{O}\) is added to \(325 \mathrm{mL}\) of \(0.035 \mathrm{M} \mathrm{KF}\) ?

Briefly describe each of the following ideas, methods, or phenomena: (a) common-ion effect in solubility equilibrium; (b) fractional precipitation; (c) ion-pair formation; (d) qualitative cation analysis.

Excess \(\mathrm{Ca}(\mathrm{OH})_{2}(\mathrm{s})\) is shaken with water to produce a saturated solution. A 50.00 mL sample of the clear saturated solution is withdrawn and requires \(10.7 \mathrm{mL}\) of \(0.1032 \mathrm{M} \mathrm{HCl}\) for its titration. What is \(K_{\mathrm{sp}}\) for \(\mathrm{Ca}(\mathrm{OH})_{2} ?\)

In the Mohr titration, \(\mathrm{Cl}^{-}(\mathrm{aq})\) is titrated with \(\mathrm{AgNO}_{3}(\text { aq })\) in solutions that are at about \(\mathrm{pH}=7\). Thus, it is suitable for determining the chloride ion content of drinking water. The indicator used in the titration is \(\mathrm{K}_{2} \mathrm{CrO}_{4}(\text { aq }) .\) A red-brown precipitate of \(\mathrm{Ag}_{2} \mathrm{CrO}_{4}(\mathrm{s})\) forms after all the \(\mathrm{Cl}^{-}\) has precipitated. The titration reaction is \(\mathrm{Ag}^{+}(\mathrm{aq})+\mathrm{Cl}^{-}(\mathrm{aq}) \longrightarrow \mathrm{AgCl}(\mathrm{s}) .\) At the equivalence point of the titration, the titration mixture consists of \(\mathrm{AgCl}(\mathrm{s})\) and a solution having neither \(\mathrm{Ag}^{+}\) nor \(\mathrm{Cl}^{-}\) in excess. Also, no \(\mathrm{Ag}_{2} \mathrm{CrO}_{4}(\mathrm{s})\) is present, but it forms immediately after the equivalence point. (a) How many milliliters of \(0.01000 \mathrm{M} \mathrm{AgNO}_{3}(\mathrm{aq})\) are required to titrate \(100.0 \mathrm{mL}\) of a municipal water sample having \(29.5 \mathrm{mg} \mathrm{Cl}^{-} / \mathrm{L} ?\) (b) What is \(\left[\mathrm{Ag}^{+}\right]\) at the equivalence point of the Mohr titration? (c) What is \(\left[\mathrm{CrO}_{4}^{2-}\right]\) in the titration mixture to meet the requirement of no precipitation of \(\mathrm{Ag}_{2} \mathrm{CrO}_{4}(\mathrm{s})\) until immediately after the equivalence point? (d) Describe the effect on the results of the titration if \(\left[\mathrm{CrO}_{4}^{2-}\right]\) were (1) greater than that calculated in part (c) or (2) less than that calculated? (e) Do you think the Mohr titration would work if the reactants were exchanged - that is, with \(\mathrm{Cl}^{-}(\text {aq })\) as the titrant and \(\mathrm{Ag}^{+}(\) aq) in the sample being analyzed? Explain.
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