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Chapter 18: Problem 94

Adding \(1.85 \mathrm{g} \mathrm{Na}_{2} \mathrm{SO}_{4}\) to \(500.0 \mathrm{mL}\) of saturated aqueous \(\mathrm{BaSO}_{4}:\) (a) reduces \(\left[\mathrm{Ba}^{2+}\right] ;\) (b) reduces \(\left[\mathrm{SO}_{4}^{2-}\right]\); (c) increases the solubility of \(\mathrm{BaSO}_{4} ;\) (d) has no effect.

Short Answer

Expert verified
The correct answers are: (a) reduces \(Ba^{2+}\), (b) reduces \(SO_4^{2-}\), (c) does not increase the solubility of BaSO4, and (d) does have an effect.

Step by step solution

01

Understanding the Common Ion Effect

When Na2SO4 is added to an aqueous solution of BaSO4, it dissociates into 2Na+ and \(SO_4^{2-}\) ions. This increases the \(SO_4^{2-}\) ion concentration in the solution. According to the common ion effect, the increase in the \(SO_4^{2-}\) concentration will shift the equilibrium to the left, reducing the \(Ba^{2+}\) concentration and hence the solubility of BaSO4.
02

Assess the change in ion concentration

Due to the shift of equilibrium, the \(Ba^{2+}\) & \(SO_4^{2-}\) ion concentrations both decrease. Hence, addition of Na2SO4 (a) reduces \(Ba^{2+}\) and (b) reduces \(SO_4^{2-}\).
03

Evaluate the effect on solubility

Regarding part (c), because the precipitation of BaSO4 is favored by the increased \(SO_4^{2-}\) ion concentration, the solubility of BaSO4 decreases, not increases. Therefore, (c) is not correct.
04

Summarize the overall effect

The overall effect of adding Na2SO4 to the saturated aqueous solution of BaSO4 is to reduce the concentrations of \(Ba^{2+}\) and \(SO_4^{2-}\) ions and decrease the solubility of BaSO4. Therefore, (d) is also not correct, as the addition of Na2SO4 does have an effect.

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Most popular questions from this chapter

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.

Which of the following solids is (are) more soluble in a basic solution than in pure water: \(\mathrm{BaSO}_{4}, \mathrm{H}_{2} \mathrm{C}_{2} \mathrm{O}_{4}\), \(\mathrm{Fe}(\mathrm{OH})_{3}, \mathrm{NaNO}_{3},\) or MnS? Explain.

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) \(\left[\mathrm{Pb}^{2+}\right]=0.5\left[\mathrm{I}^{-}\right]\)

Will precipitation occur in the following cases? (a) \(0.10 \mathrm{mg}\) NaCl is added to \(1.0 \mathrm{L}\) of \(0.10 \mathrm{M}\) \(\mathrm{AgNO}_{3}(\mathrm{aq})\). (b) One drop \((0.05 \mathrm{mL})\) of \(0.10 \mathrm{M} \mathrm{KBr}\) is added to 250 mL of a saturated solution of AgCl. (c) One drop \((0.05 \mathrm{mL})\) of \(0.0150 \mathrm{M} \mathrm{NaOH}(\mathrm{aq})\) is added to \(3.0 \mathrm{L}\) of a solution with \(2.0 \mathrm{mg} \mathrm{Mg}^{2+}\) per liter.

What percentage of the original \(\mathrm{Ag}^{+}\) remains in solution when \(175 \mathrm{mL} 0.0208 \mathrm{M} \mathrm{AgNO}_{3}\) is added to \(250 \mathrm{mL} 0.0380 \mathrm{M} \mathrm{K}_{2} \mathrm{CrO}_{4} ?\)
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