### 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 \(

The reactions in which the reactants react to form the products and proceeds in the forward…

AgCI(s) 2 Ag* (aq) + CI"(aq) Write an expression for Ksp 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.

AgCI(s) 2 Ag* (aq) + CI"(aq) Write an expression for Ksp 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.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Solutions

Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to as solute. Solution chemistry plays an important role in chemistry since it supports many commercial applications of solutions.

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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 \(

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