Titration is the measurement of the volume of a solution of one reactant that is required to react completely with a measured amount of another reactant. As both the reactants are taken in the form of solution and the titration is the measurement of volume of one solution that must be added to another solution till the reaction is complete, this method of quantitative … [Read more...] about Acid- Base Titration using Indicator
Ionic Equilibrium
Calculation of pH of a Buffer Mixture
For Acidic Buffer mixture( Henderson- Hasselbalch equation) For Basic Buffer mixture pOH = pKb + log [salt] / [Base] pH + pOH =14 pOH = 14 - pH pKa + pKb = 14 pKb=14 - pKa 14 - pH = 14 - pKa + log [salt) / [base] pH = pKa - log [salt] / [base] pH = pKa + log [base] / [salt] where Ka is the ionization constant of the conjugate acid of the … [Read more...] about Calculation of pH of a Buffer Mixture
Buffer solution and Buffer Action
Buffer Solution A buffer solution is defined as a solution which resist any change in its pH value even when small amount of acid or base are added to it. Types of the buffer solution 1) Solution of single substance The solution of the salt of weak acid and weak base eg : ammonium acetate ( CH3COOH) act as a buffer. 2) Solution of Mixture: These are of 2 … [Read more...] about Buffer solution and Buffer Action
Common Ion Effect
If to an ionic equilibrium, AB A+ + B‾ , a salt containing a common ion is added, the equilibrium shifts in the backward direction. This is called common Ion effect. Acetic acid being a weak acid, ionizes to a small extent as: CH3COOH CH3COO‾ + H+ To this solution , suppose the salt of this weak acid with a strong base is added. It ionizes almost completely in … [Read more...] about Common Ion Effect
Solubility Equilibrium and Solubility Product
If a sparingly soluble salt like AgCl is stirred with water ,only a small amount of it goes into solution while most of the salt remain undissolved. But little amount of salt dissolves, it gets completely dissociated into ions. when a sparingly soluble salt is added to water ,there exist a dynamic equilibrium between the undissolved solid salt and the ions which is … [Read more...] about Solubility Equilibrium and Solubility Product
Calculation Of Hydrolysis Constant, Degree of hydrolysis and pH of salt solution
Salt of weak acid and strong base a) Hydrolysis Constant b) Degree of Hydrolysis A‾ + H2O OH‾ + HA c 0 0 original molar conc c(1-h ) ch ch Molar conc at equilibrium c) pH Salt of strong acid and weak base a) Hydrolysis Constant BA + H2O BOH + HA B+ + A‾ + … [Read more...] about Calculation Of Hydrolysis Constant, Degree of hydrolysis and pH of salt solution
Salt Hydrolysis
Salt hydrolysis is defined as the process in which a salt reacts with water to give back the acid and the base. Salt +water ----------> Acid + Base BA + H2O ---------> HA + BOH All salts are strong electrolytes and thus ionize completely in the aqueous solution. (1) If the acid produced is strong and the base produced is weak. B+ + A‾ + H2O -------> H+ + … [Read more...] about Salt Hydrolysis
pH
A solution may be neutral, acidic or alkaline. Kw = 1 × 10-14 at 298 K To express the acidity or alkalinity of a solution, it is sufficient to express only the H3O+ ion concentration. Sorensen , in 1909 , suggested a convenient method of expressing the H3O+ ion concentration in terms of pH. The symbol has been taken from the Danish word potenz de hydrogen ion … [Read more...] about pH
Dissociation Constant and Ionic Product of Water
Pure water is poor conductor of electricity. Water is a weak electrolyte i.e. it is ionized to a very small extent as: H2O H+ + OH‾ H2O + H2O H3O+ + OH‾ This ionization is called self ionization of water. where Keq is the dissociation constant of water. Kw is the ionic product of water. Ionic product of water may be defined as the product of the … [Read more...] about Dissociation Constant and Ionic Product of Water
Strengths of Acids And Bases
According to Arrhenius concept, an acid is defined as a substance which when dissolved in water gives H+ and a base is defined as a substance which when dissolved in water give OH‾ ions. Greater the number of H+ ions produced in the aqueous solution, the stronger is the acid. Greater the number of OH‾ ions produced in the aqueous solution, the stronger is the base. As … [Read more...] about Strengths of Acids And Bases