The precipitation occurs if ionic concentration is

Options

A. Equals `K_(sp)`
B. Exceeds `K_(sp)`
C. Less than `K_(sp)`
D. is very small

Answer

To determine the condition under which precipitation occurs in a solution, we need to understand the relationship between ionic concentration and the solubility product (Ksp). Here’s a step-by-step solution:

### Step-by-Step Solution:

1. **Understanding Ionic Concentration and Solubility Product**:
- Ionic concentration refers to the concentration of ions in a solution. The solubility product (Ksp) is a constant that represents the maximum product of the concentrations of the ions in a saturated solution at a given temperature.

2. **Condition for Precipitation**:
- Precipitation occurs when the ionic product (the product of the concentrations of the ions in the solution) exceeds the solubility product (Ksp) of the solute.

3. **Mathematical Representation**:
- If we denote the ionic product as Q, then the condition for precipitation can be expressed as:
\[ Q > K_{sp} \]
- Here, Q is the ionic product calculated from the concentrations of the ions present in the solution.

4. **Saturation Point**:
- When a solution reaches its saturation point, it means that the maximum amount of solute has dissolved in the solvent. Beyond this point, if more solute is added, it will not dissolve and will instead precipitate out of the solution.

5. **Conclusion**:
- Therefore, the condition for precipitation to occur is that the ionic concentration must exceed the solubility product:
\[ \text{Ionic Concentration} > K_{sp} \]

### Final Answer:
The precipitation occurs if the ionic concentration is greater than the solubility product (Ksp).

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