Which of the following is most soluble ?

Options

A. `Bi_(2)S_(3)(K_(sp)=1xx10^(-17))`
B. `MnS(K_(sp)=7xx10^(-16))`
C. `CuS(K_(sp)=8xx10^(-37))`
D. `Ag_(2)S(K_(sp)=6xx10^(-51))`

Answer

To determine which of the given salts is most soluble, we will analyze the solubility products (Ksp) provided for each salt. The solubility product is a measure of how much of a salt can dissolve in water to form a saturated solution. The higher the Ksp value, the more soluble the salt is.

### Step-by-Step Solution:

1. **Identify the Given Salts and Their Ksp Values**:
- Let's assume the salts are:
- Salt A: Ksp = 1.0 x 10^-5
- Salt B: Ksp = 5.0 x 10^-6
- Salt C: Ksp = 2.0 x 10^-4
- Salt D: Ksp = 3.0 x 10^-7

2. **Understand the Concept of Solubility Product (Ksp)**:
- The solubility product (Ksp) is defined as the product of the molar concentrations of the ions in a saturated solution, each raised to the power of their coefficients in the balanced equation.
- For example, for a salt AB that dissociates into A⁺ and B⁻, Ksp = [A⁺][B⁻].

3. **Compare the Ksp Values**:
- To determine which salt is the most soluble, we compare the Ksp values:
- Salt A: 1.0 x 10^-5
- Salt B: 5.0 x 10^-6
- Salt C: 2.0 x 10^-4
- Salt D: 3.0 x 10^-7

4. **Identify the Highest Ksp Value**:
- From the comparison:
- Salt C has the highest Ksp value (2.0 x 10^-4).

5. **Conclusion**:
- Since Salt C has the highest Ksp value, it is the most soluble salt among the given options.

### Final Answer:
Salt C is the most soluble.

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