Home | | Chemistry 12th Std | Summary

Ionic Equilibrium | Chemistry - Summary | 12th Chemistry : UNIT 8 : Ionic Equilibrium

Chapter: 12th Chemistry : UNIT 8 : Ionic Equilibrium

Summary

According to Arrhenius, an acid is a substance that dissociates to give hydrogen ions in water.

Summary

• According to Arrhenius, an acid is a substance that dissociates to give hydrogen ions in water.

• According to Lowry and Bronsted concept, an acid is defined as a substance that has a tendency to donate a proton to another substance and base is a substance that has a tendency to accept a proton from other substance.

• According to Gilbert . N. Lewis , an acid is a species that accepts an electron pair while base is a species that donates an electron pair.

• ionic product (ionic product constant) of water (Kw)=[H3O+][OH]

• pH of a solution is defined as the negative logarithm of base 10 of the molar concentration of the hydronium ions present in the solution.

pH = –log 10 [H3O+]

• when dilution increases, the degree of dissociation of weak electrolyte also increases. This statement is known as Ostwald’s dilution Law.

• When a salt of a weak acid is added to the acid itself, the dissociation of the weak acid is suppressed further this is known as common ion effect

• Buffer is a solution which consists of a mixture of a weak acid and its conjugate base (or) a weak base and its conjugate acid.

• Buffer capacity and buffer index is defined as the number of gram equivalents of acid or base added to 1 litre of the buffer solution to change its pH by unity.

 β = dB/d(pH)

• Henderson – Hasselbalch equation For Acid buffer

pH = pKa + log ([acid]/[salt])

For Basic buffer

pOH = pKb + log ([base]/[salt])

• Hydrolysis of Salt of strong base and weak acid

Kh .Ka =Kw

pH = 7 + 1/2 pKa + 1/2 log C.

• Hydrolysis of salt of strong acid and weak base

 Kh .Kb = Kw

pH = 7 – 1/2 pKb 1/2 log C.

• Hydrolysis of Salt of weak acid and weak base

Ka .Kb .Kh =Kw

pH = 7 + 1/2 pKa 1/2 pKb .

• The solubility product of a compound is defined as the product of the molar concentration of the constituent ions, each raised to the power of its stoichiometric co – efficient in a balanced equilibrium equation.

Tags : Ionic Equilibrium | Chemistry , 12th Chemistry : UNIT 8 : Ionic Equilibrium
Study Material, Lecturing Notes, Assignment, Reference, Wiki description explanation, brief detail
12th Chemistry : UNIT 8 : Ionic Equilibrium : Summary | Ionic Equilibrium | Chemistry


Privacy Policy, Terms and Conditions, DMCA Policy and Compliant

Copyright © 2018-2023 BrainKart.com; All Rights Reserved. Developed by Therithal info, Chennai.