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Chapter 16: Problem 12

List five insoluble compounds that are more soluble in acidic solution than in neutral solution. List five compounds that are not influenced by the acidity of the solution.

Short Answer

Expert verified
1. CaCO鈧�, 2. Fe(OH)鈧�, 3. PbSO鈧�, 4. AgCl, 5. BaSO鈧� dissolve more in acid. NaCl, KNO鈧�, NH鈧凜l, LiBr, MgSO鈧� are unaffected by acidity.

Step by step solution

01

Identify Insoluble Compounds Soluble in Acidic Solution

To find compounds more soluble in acidic solution, consider metals that form insoluble hydroxides or salts with anions that can react with H+. Examples include: 1. Calcium carbonate (CaCO鈧�) 鈥� dissolves in acid as CO鈧兟测伝 forms CO鈧� and H鈧侽. 2. Iron(III) hydroxide (Fe(OH)鈧�) 鈥� dissolves in acid as OH鈦� reacts with H鈦� to form water. 3. Lead(II) sulfate (PbSO鈧�) 鈥� can become more soluble due to the formation of bisulfate (HSO鈧勨伝). 4. Silver chloride (AgCl) 鈥� solubility increases slightly due to formation of Cl鈦� which reacts with H+. 5. Barium sulfate (BaSO鈧�) 鈥� dissolves slightly better in acidic medium because H鈧係O鈧� can form.
02

Identify Compounds Not Affected by Solution Acidity

To find compounds whose solubility is not influenced by acidity, look for salts of strong acids and bases, as their ionization isn't largely dependent on pH. Examples include: 1. Sodium chloride (NaCl) 鈥� remains soluble regardless of pH. 2. Potassium nitrate (KNO鈧�) 鈥� solubility is unaffected by acidity. 3. Ammonium chloride (NH鈧凜l) 鈥� does not change significantly in different pH solutions. 4. Lithium bromide (LiBr) 鈥� pH has no significant effect on its solubility. 5. Magnesium sulfate (MgSO鈧�) 鈥� remains soluble over a wide pH range.

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Key Concepts

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

Acidic Solutions
In chemistry, acidic solutions are those with a pH less than 7. These solutions have a high concentration of hydrogen ions (H鈦�). Acidic environments can significantly impact the solubility of certain compounds.
For example, in acidic solutions, certain insoluble compounds dissolve better because the extra hydrogen ions can engage in reactions that make these compounds soluble.
  • Calcium carbonate (\( ext{CaCO}_3 \)): It can dissolve in acid because the carbonate ion (\( ext{CO}_3^{2-} \)) reacts with hydrogen ions to form carbon dioxide and water.
  • Iron(III) hydroxide (\( ext{Fe(OH)}_3 \)): The hydroxide ions (\( ext{OH}^- \)) combine with hydrogen ions to form water, allowing it to dissolve.
  • Silver chloride (\( ext{AgCl} \)): Under acidic conditions, the chloride ions may react slightly more, increasing its solubility a little.
Insoluble Compounds
Insoluble compounds are substances that do not dissolve well in water or other solvents. However, some of these compounds become more soluble under certain conditions, such as an acidic environment.
When the pH of a solution is changed, such as becoming more acidic, certain reactions are facilitated, allowing substances that typically don't dissolve to do so. For example:
  • Lead(II) sulfate (\( ext{PbSO}_4 \)): Its solubility increases because the bisulfate ion (\( ext{HSO}_4^- \)) can form.
  • Barium sulfate (\( ext{BaSO}_4 \)): It dissolves slightly more in acidic conditions due to the formation of sulfuric acid (\( ext{H}_2 ext{SO}_4 \)).
Chemical Reactions
Chemical reactions are processes in which substances, known as reactants, are transformed into different substances, known as products. In the context of solubility, the reactions are between hydrogen ions and the ions of insoluble substances.
These reactions facilitate the dissolution of several compounds in acidic solutions by either neutralizing certain ions or forming new compounds. For instance:
  • In the reaction of calcium carbonate with acids, carbon dioxide (\( ext{CO}_2 \)) is a product, making \( ext{CaCO}_3 \) more soluble.
  • Iron hydroxides react with available acids to produce water, further affecting solubility.
pH Influence
The pH of a solution indicates its acidity or basicity, influencing chemical behavior and solubility. Stable pH levels in neutral solutions do not impact solubility significantly, whereas acidic solutions show increased solubility for certain compounds.
The lower the pH, the more H鈦� ions are present, which can lead to increased solubility through chemical reactions, especially for typical insoluble compounds.
  • Solubility changes in acidic versus neutral solutions are crucial in many chemical processes, like ore refinement or pharmaceutical manufacturing.
  • Compounds like sodium chloride or potassium nitrate remain unaffected across a wide pH range, demonstrating the variability based on compound structure.
Neutral Solutions
Neutral solutions have a pH of about 7, indicating a balance between hydrogen ions (H鈦�) and hydroxide ions (\( ext{OH}^- \)). In such solutions, the solubility of various compounds remains stable and is not significantly impacted by pH fluctuations.
Examples of compounds that maintain consistent solubility in neutral solutions include:
  • Sodium chloride (\( ext{NaCl} \)): Always remains soluble, unaffected by changes in pH.
  • Potassium nitrate (\( ext{KNO}_3 \)): Soluble irrespective of pH conditions.
  • Magnesium sulfate (\( ext{MgSO}_4 \)): Solubility persists across neutral pH levels.
Conclusion:
Understanding the effects of acidic, neutral, and different pH levels on solubility is significant for various applications in science and industry, including pollution control and drug formulation.

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Most popular questions from this chapter

Calculate how much \(0.100 \mathrm{M} \mathrm{HCl}\) is needed to react completely (a) \(10.0 \mathrm{~mL}\) of \(0.150 \mathrm{M} \mathrm{KOH}\). (b) \(250.0 \mathrm{~mL}\) of \(0.00520 \mathrm{M} \mathrm{Ba}(\mathrm{OH})_{2}\). (c) \(100.0 \mathrm{~mL}\) of \(0.100 \mathrm{M}\) ammonia.

Calculate the \(\mathrm{pH}\) during the titration of \(1.00 \mathrm{~mL}\) of \(0.240 \mathrm{M} \mathrm{Ba}(\mathrm{OH})_{2}\) with \(0.200 \mathrm{M} \mathrm{HNO}_{3}\) after 0,0.50 1.00,2.40 , and \(3.00 \mathrm{~mL}\) nitric acid have been added. Graph the titration curve and compare with the curve obtained in Exercise 16.21

Sketch a titration curve for the reaction of \(50 \mathrm{~mL}\) of a \(0.10 M\) weak base \(\left(K_{\mathrm{b}}=1.0 \times 10^{-5}\right)\) with \(0.20 \mathrm{M}\) strong acid. On the same axes, sketch the titration curve for the same volume and concentration of \(\mathrm{NaOH}\).

The indicator methyl red is a weak acid with a \(\mathrm{pK}_{\mathrm{In}}\) of 5.00. Calculate the pH values at which the indicator will be \(1 \%, 5 \%, 95 \%\), and \(99 \%\) in the acid form.

Calculate the \(\mathrm{pH}\) of each of the following solutions. (a) \(10.0 \mathrm{~mL}\) of \(0.300 \mathrm{M}\) hydrofluoric acid plus \(30.0 \mathrm{~mL}\) of \(0.100 M\) sodium hydroxide (b) \(100.0 \mathrm{~mL}\) of \(0.250 \mathrm{M}\) ammonia plus \(50.0 \mathrm{~mL}\) of \(0.100 M\) hydrochloric acid (c) \(25.0 \mathrm{~mL}\) of \(0.200 \mathrm{M}\) sulfuric acid plus \(50.0 \mathrm{~mL}\) of \(0.400 \mathrm{M}\) sodium hydroxide
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