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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![**Solubility Problem for Cu2CO3 in Solution**
In this exercise, we are to determine the solubility of CuCO3(s) in a 0.15 M Cu2CO3 (aq) solution given that \( K_{sp} = 1.1 \times 10^{-10} \).
When calculating the solubility of a compound in a solution where a common ion effect may be present, it's important to consider the dissociation equilibrium and the solubility product constant (Ksp).
Recall that the solubility product constant (Ksp) is an expression of the product of the molar concentrations of the ions each raised to the power of their coefficients in the balanced equation. For Cu2CO3, the dissociation equation and the Ksp expression would be:
\[ Cu_2CO_3(s) \rightleftharpoons 2Cu^{2+}(aq) + CO_3^{2-}(aq) \]
\[ K_{sp} = [Cu^{2+}]^2[CO_3^{2-}] \]
Given:
- Concentration of \(Cu^{2+}\) in the solution = 0.15 M
- \( K_{sp} = 1.1 \times 10^{-10}\)
We can set up the equation according to the Ksp expression:
\( 1.1 \times 10^{-10} = [0.15]^2[CO_3^{2-}] \)
By solving this equation, we will find the concentration of \( CO_3^{2-} \) ions.
This type of calculation is vital in chemistry, especially when predicting the solubility of sparingly soluble salts in solutions where ions from the salt are already present.
**Instructions for Solving:**
1. **Write the expression for the solubility product (Ksp).**
2. **Input the given concentration and Ksp values.**
3. **Isolate and solve for the unknown ion concentration.**
4. **Interpret the results in terms of the solubility in the given solution.**
This problem emphasizes the concept of solubility equilibria and the influence of the common ion effect on solubility.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2704aedc-cd59-4651-b157-0d8c71ae74f0%2Fc433feb0-3093-41d8-8f59-4b8fac06303f%2Fm2ht3k_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Solubility Problem for Cu2CO3 in Solution**
In this exercise, we are to determine the solubility of CuCO3(s) in a 0.15 M Cu2CO3 (aq) solution given that \( K_{sp} = 1.1 \times 10^{-10} \).
When calculating the solubility of a compound in a solution where a common ion effect may be present, it's important to consider the dissociation equilibrium and the solubility product constant (Ksp).
Recall that the solubility product constant (Ksp) is an expression of the product of the molar concentrations of the ions each raised to the power of their coefficients in the balanced equation. For Cu2CO3, the dissociation equation and the Ksp expression would be:
\[ Cu_2CO_3(s) \rightleftharpoons 2Cu^{2+}(aq) + CO_3^{2-}(aq) \]
\[ K_{sp} = [Cu^{2+}]^2[CO_3^{2-}] \]
Given:
- Concentration of \(Cu^{2+}\) in the solution = 0.15 M
- \( K_{sp} = 1.1 \times 10^{-10}\)
We can set up the equation according to the Ksp expression:
\( 1.1 \times 10^{-10} = [0.15]^2[CO_3^{2-}] \)
By solving this equation, we will find the concentration of \( CO_3^{2-} \) ions.
This type of calculation is vital in chemistry, especially when predicting the solubility of sparingly soluble salts in solutions where ions from the salt are already present.
**Instructions for Solving:**
1. **Write the expression for the solubility product (Ksp).**
2. **Input the given concentration and Ksp values.**
3. **Isolate and solve for the unknown ion concentration.**
4. **Interpret the results in terms of the solubility in the given solution.**
This problem emphasizes the concept of solubility equilibria and the influence of the common ion effect on solubility.
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