CBSE Class 11-science Chemistry Equilibrium
Dynamic Nature of Equilibrium
Dynamic equilibrium means the rate of forward reaction is equal to the rate of backward reaction.
Law of mass action: The rate of reaction is proportional to the product of the active masses of the reacting species involved in the reaction each raised to the power as given in a balanced chemical equation.Le Chatelier's Principle
Le Chatelier's principle states that if an external stress is applied to a system at chemical equilibrium, the system will adjust to partially offset the stress.
Changes in concentration, pressure, or volume may change the equilibrium concentrations of reactants and products.
Addition of a catalyst hastens the attainment of equilibrium.Ionic Equilibrium
Part of electrolyte which dissociates is called degree of dissociation.
Acids are electron pair acceptors while bases are electron pair donors.
Conjugate base of strong acid is weak while conjugate base of weak acid is strong.Ionisation of Water
The ionic product of water at 25°C is defined as the product of the molar concentrations of hydronium ion and hydroxyl ions.
pH is defined as the negative logarithm to the base 10 of the hydrogen ion concentration.
The hydrolysis of salt is of four types.Solubility Product
Solubility is the mass of solute that forms a saturated solution with a given mass of solvent. It increases with temperature.
Solubility product is defined as the product of molar concentration of ions raised to the power of coefficients in a saturated solution.Common Ion Effect
Shift in equilibrium position is caused by the addition or presence of an ion involved in the equilibrium reaction known as common ion effect.
Precipitation occurs when ionic product exceeds the solubility product.
Buffer solutions which resist a change in pH caused by dilution or the addition of limited amounts of acid or base.
Shift in equilibrium position is caused by the addition or presence of an ion involved in the equilibrium reaction known as common ion effect.
Precipitation occurs when ionic product exceeds the solubility product.
Buffer solutions which resist a change in pH caused by dilution or the addition of limited amounts of acid or base.
