Chemistry
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ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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![### Understanding Solubility Product Constant (Ksp) and Solubility of Silver Chloride
**Equation:**
\[ \text{AgCl(s) } \rightleftharpoons \text{ Ag}^+ \text{(aq) } + \text{ Cl}^- \text{(aq)} \]
**Task:**
Write an expression for \( K_{sp} \) for silver chloride and indicate its expected magnitude (i.e., large or small). Support your decision given what you know about the solubility of "insoluble" substances.
### Explanation:
The solubility product constant, \( K_{sp} \), is a measure of the solubility of a sparingly soluble ionic compound. It is defined as the product of the concentrations of the ions, each raised to the power of their coefficients in the balanced equation.
For the dissociation of silver chloride:
\[
\text{AgCl(s) } \rightleftharpoons \text{ Ag}^+ \text{(aq) } + \text{ Cl}^- \text{(aq)}
\]
The expression for \( K_{sp} \) is:
\[ K_{sp} = [\text{Ag}^+][\text{Cl}^-] \]
### Magnitude of \( K_{sp} \):
Silver chloride (AgCl) is an example of a compound that is considered "insoluble" in water. This means that it dissolves to such a small extent that its solubility is practically negligible. As a consequence, the concentration of \( \text{Ag}^+ \) and \( \text{Cl}^- \) ions in solution will be very low.
Because of the low solubility, the product of the ionic concentrations \([Ag^+]\) and \([Cl^-]\) will be quite small. Therefore, the \( K_{sp} \) value for silver chloride is expected to be very small.
### Support:
The limited solubility of silver chloride can be used to support the idea that the \( K_{sp} \) value is low. In general, if a compound has low solubility in water, the \( K_{sp} \) value is small because only a tiny amount of the compound dissociates into ions in aqueous solution. Consequently, since AgCl is considered almost insoluble, we can predict that the \(](https://content.bartleby.com/qna-images/question/ab59d09b-08ac-401f-9f5b-17ad88e0fb6d/3b78405d-3dcf-4c0a-812f-7f24aa09f11b/2j9gxr_processed.jpeg)
Transcribed Image Text:### Understanding Solubility Product Constant (Ksp) and Solubility of Silver Chloride
**Equation:**
\[ \text{AgCl(s) } \rightleftharpoons \text{ Ag}^+ \text{(aq) } + \text{ Cl}^- \text{(aq)} \]
**Task:**
Write an expression for \( K_{sp} \) for silver chloride and indicate its expected magnitude (i.e., large or small). Support your decision given what you know about the solubility of "insoluble" substances.
### Explanation:
The solubility product constant, \( K_{sp} \), is a measure of the solubility of a sparingly soluble ionic compound. It is defined as the product of the concentrations of the ions, each raised to the power of their coefficients in the balanced equation.
For the dissociation of silver chloride:
\[
\text{AgCl(s) } \rightleftharpoons \text{ Ag}^+ \text{(aq) } + \text{ Cl}^- \text{(aq)}
\]
The expression for \( K_{sp} \) is:
\[ K_{sp} = [\text{Ag}^+][\text{Cl}^-] \]
### Magnitude of \( K_{sp} \):
Silver chloride (AgCl) is an example of a compound that is considered "insoluble" in water. This means that it dissolves to such a small extent that its solubility is practically negligible. As a consequence, the concentration of \( \text{Ag}^+ \) and \( \text{Cl}^- \) ions in solution will be very low.
Because of the low solubility, the product of the ionic concentrations \([Ag^+]\) and \([Cl^-]\) will be quite small. Therefore, the \( K_{sp} \) value for silver chloride is expected to be very small.
### Support:
The limited solubility of silver chloride can be used to support the idea that the \( K_{sp} \) value is low. In general, if a compound has low solubility in water, the \( K_{sp} \) value is small because only a tiny amount of the compound dissociates into ions in aqueous solution. Consequently, since AgCl is considered almost insoluble, we can predict that the \(
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