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Chapter 18: Problem 46

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.

Short Answer

Expert verified
Only H2C2O4 is more soluble in a basic solution than in water. The other compounds, BaSO4, Fe(OH)3, NaNO3, and MnS, are not.

Step by step solution

01

Identify Solids that Participate in Acid-Base Reactions

Analyze the given compounds and identify those that can act as acids. These compounds are more soluble in a basic solution than in water, as they can react with hydroxyl ions. In the provided list, the compound H2C2O4, an organic acid, can react with hydroxyl ions.
02

Identify Solids that Form Complex Ions

Next, look for compounds that can form complex ions with hydroxyl groups. These compounds will also be more soluble in basic solutions. None of the given compounds, BaSO4, H2C2O4, Fe(OH)3, NaNO3, or MnS, form complex ion in basic solution.
03

Evaluate Solubility for Remaining Solids

Finally, evaluate the remaining solids. BaSO4, Fe(OH)3, NaNO3, and MnS do not fall under any of the categories mentioned in step 1 and 2. Hence, these compounds are not more soluble in basic solutions than in water.

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Most popular questions from this chapter

When \(200.0 \mathrm{mL}\) of \(0.350 \mathrm{M} \mathrm{K}_{2} \mathrm{CrO}_{4}(\mathrm{aq})\) are added to 200.0 mL of 0.0100 M AgNO 3(aq), what percentage of the \(\mathrm{Ag}^{+}\) is left unprecipitated?

Fluoridated drinking water contains about 1 part per million (ppm) of \(\mathrm{F}^{-}\). Is \(\mathrm{CaF}_{2}\) sufficiently soluble in water to be used as the source of fluoride ion for the fluoridation of drinking water? Explain. [Hint: Think of 1 ppm as signifying \(1 \mathrm{g} \mathrm{F}^{-}\) per \(10^{6} \mathrm{g}\) solution.

Which of the following solids is (are) more soluble in an acidic solution than in pure water: \(\mathrm{KCl}\), \(\mathrm{MgCO}_{3}\), \(\mathrm{FeS}, \mathrm{Ca}(\mathrm{OH})_{2,}\) or \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{COOH} ?\) Explain.

Reaction (18.10), described in the Integrative Example, is called a carbonate transposition. In such a reaction, anions of a slightly soluble compound (for example, hydroxides and sulfates) are obtained in a sufficient concentration in aqueous solution that they can be identified by qualitative analysis tests. Suppose that \(3 \mathrm{M} \mathrm{Na}_{2} \mathrm{CO}_{3}\) is used and that an anion concentration of \(0.050 \mathrm{M}\) is sufficient for its detection. Predict whether carbonate transposition will be effective for detecting (a) \(\mathrm{SO}_{4}^{2-}\) from \(\mathrm{BaSO}_{4}(\mathrm{s}) ;\) (b) \(\mathrm{Cl}^{-}\) from \(\mathrm{AgCl}(\mathrm{s}) ;(\mathrm{c}) \mathrm{F}^{-}\) from \(\mathrm{MgF}_{2}(\mathrm{s})\).

A solution is \(0.05 \mathrm{M}\) in \(\mathrm{Cu}^{2+},\) in \(\mathrm{Hg}^{2+},\) and in \(\mathrm{Mn}^{2+}\). Which sulfides will precipitate if the solution is made to be \(0.10 \mathrm{M} \mathrm{H}_{2} \mathrm{S}(\mathrm{aq})\) and \(0.010 \mathrm{M} \mathrm{HCl}(\mathrm{aq}) ?\) For \(\mathrm{CuS}\), \(K_{\mathrm{spa}}=6 \times 10^{-16} ;\) for \(\mathrm{HgS}, K_{\mathrm{spa}}=2 \times 10^{-32} ;\) for \(\mathrm{MnS}\), \(K_{\mathrm{spa}}=3 \times 10^{7}\).
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