A precipitate is formed when ionic product becomes equal to the solubility product.

Answer

To solve the question regarding the formation of a precipitate when the ionic product equals the solubility product, we can break down the explanation into clear steps:

### Step-by-Step Solution:

1. **Understanding Solubility Product (Ksp)**:
- The solubility product (Ksp) is a constant that represents the maximum concentration of ions that can exist in a solution at equilibrium for a saturated solution of a sparingly soluble salt. It is specific to a particular salt at a given temperature.

2. **Defining Ionic Product (IP)**:
- The ionic product (IP) is the product of the molar concentrations of the ions in a solution, each raised to the power of their respective coefficients in the balanced chemical equation. It can be calculated at any point in time, regardless of whether the solution is saturated or not.

3. **Comparing IP and Ksp**:
- When the ionic product (IP) is less than the solubility product (Ksp), the solution is unsaturated, and no precipitate forms.
- When the ionic product (IP) equals the solubility product (Ksp), the solution is saturated, and the solution is at equilibrium. At this point, the solution can hold no more dissolved solute, and any additional solute will begin to precipitate out.
- When the ionic product (IP) exceeds the solubility product (Ksp), the solution becomes supersaturated, leading to the formation of a precipitate as the excess solute cannot remain dissolved.

4. **Conclusion**:
- Therefore, the statement that a precipitate is formed when the ionic product becomes equal to the solubility product is correct. At this point, the solution reaches saturation, and any further addition of the solute will result in precipitation.

### Final Statement:
A precipitate is indeed formed when the ionic product of a solution equals its solubility product, indicating that the solution has reached saturation.