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Chapter 18: Problem 16

How would you expect the presence of each of the following solutes to affect the molar solubility of \(\mathrm{CaCO}_{3}\) in water: (a) \(\mathrm{Na}_{2} \mathrm{CO}_{3} ;\) (b) \(\mathrm{HCl} ;\) (c) \(\mathrm{NaHSO}_{4}\) ? Explain.

Short Answer

Expert verified
(a) The presence of Na2CO3 will decrease the molar solubility of CaCO3. (b) The presence of HCl will increase the molar solubility of CaCO3. (c) The presence of NaHSO4 will increase the molar solubility of CaCO3.

Step by step solution

01

Analyzing Na2CO3 Effect on CaCO3 Solubility

Na2CO3 will dissociate into Na+ and CO32- ions in solution. Adding it to a solution of CaCO3 introduces a 'common ion' into the mix. This increases the concentration of CO32-, one of the ions in equilibrium with solid CaCO3. According to Le Chatelier's principle, the reaction will shift to the left, decreasing the solubility of CaCO3.
02

Analyzing HCl Effect on CaCO3 Solubility

HCl is a strong acid and will completely dissociate into H+ and Cl- ions in solution. The added H+ ions will react with CO32- ions from CaCO3 to form HCO3-. This reduces CO32- ion concentration and, according to Le Chatelier's principle, the equilibrium will shift to the right to increase the solubility of CaCO3.
03

Analyzing NaHSO4 Effect on CaCO3 Solubility

NaHSO4 will dissociate into Na+ and HSO4- ions in solution. The HSO4- can donate a proton (H+) to form SO42- and that H+ can react with CO32- to form HCO3-. This decreases CO32- concentration, and consistent with Le Chatelier's principle, the equilibrium will shift to the right, increasing the solubility of CaCO3.

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Most popular questions from this chapter

Both \(\mathrm{Mg}^{2+}\) and \(\mathrm{Cu}^{2+}\) are present in the same aqueous solution. Which of the following reagents would work best in separating these ions, precipitating one and leaving the other in solution: \(\mathrm{NaOH}(\mathrm{aq}), \mathrm{HCl}(\mathrm{aq})\), \(\mathrm{NH}_{4} \mathrm{Cl}(\mathrm{aq}),\) or \(\mathrm{NH}_{3}(\mathrm{aq}) ?\) Explain your choice.

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.

If \(100.0 \mathrm{mL}\) of a clear saturated solution of \(\mathrm{Ag}_{2} \mathrm{SO}_{4}\) is added to \(250.0 \mathrm{mL}\) of a clear saturated solution of \(\mathrm{PbCrO}_{4},\) will any precipitate form? [Hint: Take into account the dilutions that occur. What are the possible precipitates?]

In your own words, define the following terms or symbols: (a) \(K_{\mathrm{sp}} ;\) (b) \(K_{f} ;\) (c) \(Q_{\mathrm{sp}} ;\) (d) complex ion.

Pure water is saturated with slightly soluble \(\mathrm{PbI}_{2}\) Which of the following is a correct statement concerning the lead ion concentration in the solution, and what is wrong with the others? (a) \(\left[\mathrm{Pb}^{2+}\right]=\left[\mathrm{I}^{-}\right]\); (b) \(\left[\mathrm{Pb}^{2+}\right]=K_{\mathrm{sp}}\) of \(\mathrm{PbI}_{2} ;(\mathrm{c})\left[\mathrm{Pb}^{2+}\right]=\sqrt{K_{\mathrm{sp}}}\) of \(\mathrm{PbI}_{2}\); (d) \(\left[\mathrm{Pb}^{2+}\right]=0.5\left[\mathrm{I}^{-}\right]\)
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