solubility product

Question

When ionic product exceeds solubility product:

RankGuru · Accepted Answer

The **Solubility Product ($K_{sp}$)** defines the equilibrium state for a saturated solution of a sparingly soluble salt.
- **Ionic Product ($I.P.$)** is the product of concentrations of ions at any given moment.
1. **$I.P. < K_{sp}$**: Solution is unsaturated. No precipitation.
2. **$I.P. = K_{sp}$**: Solution is exactly saturated. No precipitation.
3. **$I.P. > K_{sp}$**: Solution is supersaturated. **Precipitation** will occur until $[I.P.]$ returns to $[K_{sp}]$.
- This principle is fundamental to quantitative separation of groups in salt analysis.

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More solubility product Practice Questions

The solubility product of AgCl at 298 K is 1.0 × 10⁻¹⁰. The solubility of AgCl in water is: