Calculate the molar solubility of CuCl in a solution that is 0.5.0 M in NaCl.
The formation constant of CuCl, Kf = ?

To calculate the molar solubility of **CuCl** in a solution that is **0.50 M** in NaCl, we first need to understand the relevant equilibria and use the provided information to solve for the solubility. However, since the value for the formation constant, \( K_f \), of CuCl is not given explicitly, we will work with a general approach.

Here are the steps to approach the problem:

### 1. Write the relevant equilibria

CuCl is a slightly soluble salt, and it dissociates according to the following equilibrium equation:

\[
\text{CuCl(s)} \rightleftharpoons \text{Cu}^+ (aq) + \text{Cl}^- (aq)
\]

The solubility product constant \( K_{sp} \) for this reaction is defined as:

\[
K_{sp} = [\text{Cu}^+][\text{Cl}^-]
\]

However, due to the presence of \( \text{NaCl} \), which dissociates completely, the concentration of \( \text{Cl}^- \) will be significantly affected by the NaCl concentration (which is 0.50 M). Therefore, the total chloride ion concentration will be approximately 0.50 M.

### 2. The formation constant (Kf)

The complex formation can also occur:

\[
\text{Cu}^+ + \text{Cl}^- \rightleftharpoons \text{CuCl}_2^-
\]

The formation constant \( K_f \) is defined as:

\[
K_f = \frac{[\text{CuCl}_2^-]}{[\text{Cu}^+][\text{Cl}^-]}
\]

But since \( K_f \) isn't provided in your question, you'd need to look up this value from a data source, as it's typically a known value for CuCl. Once you have \( K_f \), you can set up the equation and solve for the molar solubility \( s \) based on the equilibria.

### 3. Use of NaCl concentration

Given that the \( \text{Cl}^- \) ion concentration is largely determined by the dissociation of NaCl (0.50 M), this value will shift the solubility equilibrium of CuCl and allow us to calculate the molar solubility by combining the \( K_{sp} \) and \( K_f \) expressions.

Would you like more detailed steps once we have the value of \( K_f \)? Alternatively, I can help you look up the appropriate \( K_f \) for this system if you're unsure where to find it.

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### Related questions:
1. What is the significance of \( K_{sp} \) and \( K_f \) in solubility calculations?
2. How does the common ion effect influence the solubility of sparingly soluble salts?
3. Can we calculate the solubility of CuCl without knowing the formation constant?
4. How does the presence of complexing agents (like Cl⁻) affect the solubility of metal salts?
5. What methods are used to experimentally determine solubility product constants?

**Tip**: In problems involving common ions and complex formation, the presence of an excess of one ion can significantly shift the equilibrium and affect solubility.

Calculate the molar solubility of CuCl in a solution that is 0.50 M in NaCl. The formation constant of CuCl, Kf = ?

Learn how to calculate the molar solubility of CuCl in a solution that is 0.50 M in NaCl. This problem explores solubility equilibria, the common ion effect, and complex ion formation. Understand the role of Ksp and Kf in determining solubility shifts in the presence of NaCl.

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