In which of the following cases is the solution of `AgCl` unsaturated?
A
`[Ag^(+)][Cl^(-)]ltK_(sp)`
B
`[Ag^(+)][Cl^(-)]gtK_(sp)`
C
`[Ag^(+)][Cl^(-)]=K_(sp)`
D
`[Ag^(+)][Cl^(-)]leK_(sp)`
Text Solution
AI Generated Solution
The correct Answer is:
To determine in which case the solution of AgCl is unsaturated, we need to understand the concepts of saturated and unsaturated solutions.
### Step-by-Step Solution:
1. **Define Saturated and Unsaturated Solutions**:
- A **saturated solution** is one in which the maximum amount of solute has been dissolved at a given temperature, and any additional solute will not dissolve. In this case, the concentration of ions (Ag⁺ and Cl⁻) is at its maximum, which means it is equal to the solubility product (Ksp) of AgCl.
- An **unsaturated solution**, on the other hand, is one where less than the maximum amount of solute is dissolved. Here, the concentration of ions is less than the Ksp of AgCl.
2. **Understanding Ksp**:
- The solubility product (Ksp) is a constant that represents the maximum concentration of ions in a saturated solution. For AgCl, the Ksp expression is:
\[
K_{sp} = [Ag^+][Cl^-]
\]
- If the product of the concentrations of Ag⁺ and Cl⁻ ions is less than Ksp, the solution is unsaturated.
3. **Analyzing Given Cases**:
- We need to evaluate the provided cases to see in which one the concentration of Ag⁺ and Cl⁻ is less than the Ksp value.
4. **Conclusion**:
- After analyzing the options, we find that in option A, the concentration of Ag⁺ and Cl⁻ is indeed less than the Ksp value. Therefore, the solution of AgCl in this case is unsaturated.
### Final Answer:
The solution of AgCl is unsaturated in case **A**, where the concentration of Ag⁺ and Cl⁻ is less than the Ksp value.
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