Many chemical salts do not dissolve completely in water. Instead, they establish a dynamic balance between the solid salt and its dissolved ions. This lesson covers part ii equilibria involving sparingly soluble salts to help you master this core chemistry concept.
When you add a sparingly soluble salt to water, only a tiny fraction dissolves. The rate at which the solid dissolves eventually matches the rate at which ions precipitate back into solid form. At this point, the solution reaches dynamic equilibrium. Chemists describe this state using the solubility product constant, known as Ksp.
Understanding Ksp allows you to predict whether a precipitate will form during a chemical reaction. You compare the ion product to the solubility product constant. If the ion product exceeds Ksp, precipitation occurs. If it remains below Ksp, more salt can dissolve safely without forming solids.
This video breaks down the math and concepts behind solubility equilibria. You will see clear examples of calculating molar solubility and finding ion concentrations in saturated solutions. Watch the full tutorial to strengthen your problem-solving skills for Class 11 exams.