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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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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Acid-Base Reactions
Acid-base reactions are a fascinating topic in chemistry where acids and bases interact to neutralize each other, forming water and a salt. Acids are substances that can donate a proton (H⁺), while bases can accept a proton or donate a hydroxyl ion (OH⁻). In the context of solubility, some solids dissolve better in basic solutions due to their acidic nature. For example, when an acidic compound like oxalic acid (\(\mathrm{H}_2\mathrm{C}_2\mathrm{O}_4\)) is placed in a basic solution, it can react with hydroxyl ions from the base, forming water and thus increase its solubility. This is because the reaction removes the acid component from the equilibrium, driving the dissolution process forward to replace the reacted acid. To sum up, if a substance can participate in an acid-base reaction, it is likely to be more soluble in a solution where the opposite reaction partner is present, like a base for an acid. Understanding these principles can help predict solubility behavior of various compounds in different types of solutions.
Complex Ion Formation
Complex ion formation refers to the process where compounds form stable ions in solution by binding to central metal ions, usually through coordination with ligands. This happens when metal ions combine with other molecules or ions (like hydroxyl ions or ammonia) to form a complex with a unique structure and properties. Although none of the compounds discussed in the exercise form complex ions in a basic solution, it's worth noting that complex ions can significantly enhance the solubility of certain compounds. For instance, if a compound consists of elements capable of forming complexes, such as transition metals, the presence of ligands can facilitate increased solubility by keeping the metal ions in solution. Complex ion formation is especially important in the context of transition metals, where solubility can be deeply influenced by the formation of these complex structures. Understanding when and how complex ions form allows chemists to manipulate conditions to enhance or reduce the solubility of specific compounds.
Basic Solution Solubility
Basic solutions are characterized by the presence of excess hydroxyl ions (OH⁻). These solutions often affect the solubility of various compounds differently compared to pure water. Some solids dissolve better in basic solutions, especially if they can interact with the hydroxyl ions present. For example, acidic compounds such as oxalic acid can exhibit higher solubility in basic solutions because they react with the hydroxyl ions, as mentioned earlier. However, substances that do not react with hydroxyl ions directly or form complex ions do not show a significant increase in solubility. It's important to consider the chemical nature of a compound when predicting its solubility in basic conditions. Having a clear understanding of the behavior of both acidic and non-acidic solids in basic solutions is crucial for chemists in fields ranging from material science to pharmacology. This knowledge helps in anticipating solubility issues and enhances the efficiency of various chemical processes.

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Most popular questions from this chapter

Can \(\mathrm{Fe}^{2+}\) and \(\mathrm{Mn}^{2+}\) be separated by precipitating \(\mathrm{FeS}(\mathrm{s})\) and not \(\mathrm{MnS}(\mathrm{s}) ?\) Assume \(\left[\mathrm{Fe}^{2+}\right]=\left[\mathrm{Mn}^{2+}\right]=\) \(\left[\mathrm{H}_{2} \mathrm{S}\right]=0.10 \mathrm{M} .\) Choose a \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\) that ensures maximum precipitation of \(\mathrm{FeS}(\mathrm{s})\) but not \(\mathrm{MnS}(\mathrm{s}) .\) Will the separation be complete? For \(\mathrm{FeS}, K_{\mathrm{spa}}=6 \times 10^{2} ;\) for \(\mathrm{MnS}, K_{\mathrm{spa}}=3 \times 10^{7}\).

Which of the following has the highest molar solubility? (a) \(\mathrm{MgF}_{2}, K_{\mathrm{sp}}=3.7 \times 10^{-8}\) \(\mathrm{MgCO}_{3}\), \(K_{\mathrm{sp}}=3.5 \times 10^{-8} ;(\mathrm{c}) \mathrm{Mg}_{3}\left(\mathrm{PO}_{4}\right)_{2}, K_{\mathrm{sp}}=1 \times 10^{-25}\); (d) \(\mathrm{Li}_{3} \mathrm{PO}_{4}, K_{\mathrm{sp}}=3.2 \times 10^{-9}\).

To precipitate as \(\mathrm{Ag}_{2} \mathrm{S}(\mathrm{s}),\) all the \(\mathrm{Ag}^{+}\) present in \(338 \mathrm{mL}\) of a saturated solution of \(\mathrm{AgBrO}_{3}\) requires \(30.4 \mathrm{mL}\) of \(\mathrm{H}_{2} \mathrm{S}(\mathrm{g})\) measured at \(23^{\circ} \mathrm{C}\) and \(748 \mathrm{mm} \mathrm{Hg} .\) What is \(K_{\mathrm{sp}}\) for \(\mathrm{AgBrO}_{3} ?\)

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.

A 2.50 g sample of \(\mathrm{Ag}_{2} \mathrm{SO}_{4}(\mathrm{s})\) is added to a beaker containing 0.150 L of 0.025 M BaCl\(_2\) (a) Write an equation for any reaction that occurs. (b) Describe the final contents of the beaker- -that is, the masses of any precipitates present and the concentrations of the ions in solution.
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