Equilibrium

Whenever equilibrium is disturbed by change in the concentration, pressure or volume, the composition of the equilibrium mixture changes because the reaction quotient, Q_c no longer equals the equilibrium constant, Kc. However, when a change in temperature occurs, the value of equilibrium constant, K

If the volume is kept constant and an inert gas such as argon is added which does not take part in the reaction, the equilibrium remains undisturbed. It is because the addition of an inert gas at constant volume does not change the partial pressures or the molar concentrations of the substance invol

The intensity of the red colour becomes constant on attaining equilibrium. This equilibrium can be shifted in either forward or reverse directions depending on adding a reactant or a product. The equilibrium can be shifted in the opposite direction by adding reagents that remove Fe³⁺or SCN^– ions. Fo

This is because at lower pH, the concentration of the anion decreases due to its protonation. This in turn increase the solubility of the salt so that K_sp = Q_sp.

The solutions which resist change in pH on dilution or with the addition of small amounts of acid or alkali are called Buffer Solutions.

1. Its pH does not change on the addition of small amount of acid or base.
2. Its pH does not change on dilution or standing.

It is product of molar concentration of ion raised to the power of number of ions produced per compound in saturated solution.

Solubility of electrolyte decreases due to common ion effect.

Equilibrium is a state at which rate of forwarding reaction is equal to the rate of backward reaction. The equilibrium between ions and unionised molecules is called ionic equilibrium.

A catalyst does not affect the equilibrium composition of a reaction mixture. Catalysts influence the rate of both forward and backward reactions equally.

Equilibrium constant depends upon the way in which the reaction is written.