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...
Related questions
Question
![### 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 \(](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fab59d09b-08ac-401f-9f5b-17ad88e0fb6d%2F3b78405d-3dcf-4c0a-812f-7f24aa09f11b%2F2j9gxr_processed.jpeg&w=3840&q=75)
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 \(
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution!
Trending now
This is a popular solution!
Step by step
Solved in 3 steps with 2 images
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Recommended textbooks for you
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY