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Chapter 17: Problem 66

Which of the following ionic compounds will be more soluble in acid solution than in water: (a) \(\mathrm{BaSO}_{4}\), (b) \(\mathrm{PbCl}_{2}\) (c) \(\mathrm{Fe}(\mathrm{OH})\) (d) \(\mathrm{CaCO}_{3} ?\)

Short Answer

Expert verified
Fe(OH)鈧� and CaCO鈧� are more soluble in acid than in water.

Step by step solution

01

Understand the Solubility in Acid

Ionic compounds can be more soluble in acidic solutions if their anions react with hydrogen ions (H鈦�) from the acid. By forming new products, these reactions remove the anion from solution, thus increasing the compound's solubility.
02

Evaluate Compound (a) 鈥� BaSO鈧�

Barium sulfate ( BaSO鈧� ) has the sulfate ion, SO鈧刕{2-} , as its anion. Sulfates generally do not react with H鈦� in acids to form more soluble species, so BaSO鈧� is not more soluble in acid.
03

Evaluate Compound (b) 鈥� PbCl鈧�

Lead(II) chloride ( PbCl鈧� ) has the chloride ion, Cl^{-} , which does not react significantly with H鈦� in acid. Therefore, PbCl鈧� will not be more soluble in acid compared to water.
04

Evaluate Compound (c) 鈥� Fe(OH)

Iron(III) hydroxide ( Fe(OH)鈧� ) contains hydroxide ions, OH^{-} , which can react with H鈦� to form water: OH鈦� + H鈦� 鈫� H鈧侽 . This removes the hydroxide ions from the solution, increasing the solubility of Fe(OH)鈧� in acid.
05

Evaluate Compound (d) 鈥� CaCO鈧�

Calcium carbonate ( CaCO鈧� ) contains carbonate ions, CO鈧僞{2-} , which react with H鈦� to form HCO鈧僞{-} or CO鈧� gas: CO鈧僞{2-} + 2H鈦� 鈫� CO鈧� + H鈧侽 . This reaction increases solubility in acid.
06

Identify the Most Soluble in Acid

From the analysis: Fe(OH)鈧� and CaCO鈧� are more soluble in acidic solutions due to their anion's reaction with H鈦�. However, BaSO鈧� and PbCl鈧� do not show increased solubility in acid.

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Key Concepts

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

Ionic Compounds
Ionic compounds are substances made up of positive and negative ions. These ions are held together by strong electrostatic forces known as ionic bonds. When dissolved in water, these compounds separate into their respective ions.
  • Ionic compounds are commonly formed from metals and nonmetals.
  • Examples include substances like sodium chloride ( NaCl ) and calcium carbonate ( CaCO鈧� ).
In some cases, the solubility of these compounds can increase when placed in different environments, such as acidic solutions. This is mainly due to the interactions between the ions and the elements in the solution which can lead to new, more soluble compounds.
Anion Reactivity
Anions are negatively charged ions that play a crucial role in the solubility of ionic compounds in acidic solutions. The reactivity of anions with hydrogen ions ( H鈦� ) can significantly affect the solubility of a compound.
  • Some anions, like the carbonate ion ( CO鈧僞{2-} ), react readily with H鈦� , forming new products that help dissolve compounds.
  • Others, like the sulfate ion ( SO鈧刕{2-} ), do not react significantly with acids, resulting in little to no increase in solubility.
This difference in reactivity influences whether an ionic compound will be more soluble in an acidic environment.
Hydrogen Ions Interaction
In acidic solutions, the presence of hydrogen ions ( H鈦� ) can modify the behavior of ionic compounds. When H鈦� ions interact with certain anions, new products are formed, which can enhance the solubility of these compounds.
  • For instance, OH^{-} (hydroxide ions) react with H鈦� to create water, effectively removing hydroxide ions from the solution.
  • In the case of CO鈧僞{2-} (carbonate ions), the reaction with H鈦� can produce carbon dioxide and water, aiding in the solubility increase of compounds like calcium carbonate.
These interactions are pivotal in determining how compounds such as iron(III) hydroxide and calcium carbonate behave in acidic environments.
Iron(III) Hydroxide Solubility
Iron(III) hydroxide (Fe(OH)鈧�) tends to have low solubility in water, but when introduced to an acidic solution, its solubility can increase. This is due to the interaction between hydroxide ions and hydrogen ions:\[ ext{OH}^{-} + ext{H}^{+} ightarrow ext{H}_2 ext{O}\]
  • This reaction effectively removes OH^{-} ions from the solution, reducing the tendency for these ions to recombine with iron to form solid Fe(OH)鈧�.
  • As OH^{-} is removed, more Fe(OH)鈧� can dissolve to restore equilibrium, leading to increased solubility.
This process demonstrates how Fe(OH)鈧� transitions from a minimal solubility state in water to enhanced solubility in acidic conditions.
Calcium Carbonate Solubility
Calcium carbonate (CaCO鈧�) also has limited solubility in water. However, it becomes more soluble in acidic conditions. This is due to the reaction of carbonate ions (CO鈧僞{2-}) with hydrogen ions:\[ ext{CO}_3^{2-} + 2 ext{H}^{+} ightarrow ext{CO}_2 + ext{H}_2 ext{O}\]
  • Carbon dioxide gas (CO鈧�) is produced as a byproduct and can escape from the solution, driving the reaction forward.
  • As a result, CaCO鈧� dissolves more readily to replace the lost CO鈧僞{2-} ions.
This process is why calcium carbonate materials, like limestone or chalk, erode more rapidly in acidic environments.

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Most popular questions from this chapter

A 5.00 -g quantity of a diprotic acid was dissolved in water and made up to exactly \(250 \mathrm{~mL}\). Calculate the molar mass of the acid if \(25.0 \mathrm{~mL}\) of this solution required \(11.1 \mathrm{~mL}\) of \(1.00 \mathrm{M} \mathrm{KOH}\) for neutralization. Assume that both protons of the acid were titrated.

The ionization constant \(K_{\mathrm{a}}\) of an indicator HIn is \(1.0 \times 10^{-6} .\) The color of the nonionized form is red and that of the ionized form is yellow. What is the color of this indicator in a solution whose \(\mathrm{pH}\) is \(4.00 ?\)

The solubility product of \(\mathrm{Mg}(\mathrm{OH})_{2}\) is \(1.2 \times 10^{-11} .\) What minimum \(\mathrm{OH}^{-}\) concentration must be attained (e.g., by adding \(\mathrm{NaOH}\) ) to decrease the Mg concentration in a solution of \(\mathrm{Mg}\left(\mathrm{NO}_{3}\right)\), to less than \(1.0 \times 10^{-10} \mathrm{M} ?\)

Outline the general procedure of qualitative analysis.

In a group 1 analysis, a student obtained a precipitate containing both \(\mathrm{AgCl}\) and \(\mathrm{PbCl}_{2}\). Suggest one reagent that would enable the student to separate \(\mathrm{AgCl}(s)\) from \(\mathrm{PbCl}_{2}(s)\)
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