There is ppt. of solute AB if its product is greater than `K_(sp)` value i.e. `[A][B] gt K_(sp)`True/false

Explanation

To determine whether the statement "There is a precipitate of solute AB if its product is greater than Ksp value" is true or false, we can analyze the situation step by step.

### Step-by-Step Solution:

1. **Understanding Ksp**:
- Ksp (solubility product constant) is a constant that represents the maximum product of the concentrations of the ions in a saturated solution at a given temperature. For a salt AB that dissociates into ions A⁺ and B⁻, the Ksp expression is given by:
\[ K_{sp} = [A^+][B^-] \]

2. **Condition for Precipitation**:
- A precipitate forms when the product of the concentrations of the ions exceeds the Ksp value. This means if:
\[ [A^+][B^-] > K_{sp} \]
then the solution is supersaturated, and a precipitate will form.

3. **Analyzing the Statement**:
- The statement claims that there is a precipitate of solute AB if the product of the concentrations of A⁺ and B⁻ is greater than Ksp. This aligns with our understanding of Ksp and precipitation conditions.

4. **Conclusion**:
- Since the condition for precipitation is indeed when the product of the concentrations of the ions exceeds Ksp, the statement is true.

### Final Answer:
The statement is **True**.

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