This document discusses acids, bases, and salts. It defines acids as substances that taste sour, react with metals and carbonates, and change litmus color. Bases taste bitter, feel slippery, and also change litmus color. Salts are water-soluble ionic compounds that can be acidic, basic, or neutral depending on whether they contain ions from strong/weak acids or bases. The document also covers ionization of water, pH and pOH calculations, acid-base concepts, conjugate pairs, and salt hydrolysis reactions that can produce acidic or basic solutions.

1. ACIDS,
BASIS AND
SALTS
NAVEED MALLANA

2. Reduced Syllabus For 2021 Examination
8. ACIDS, BASES ANDSALTS
Introduction
8.2 8.2.2 Relative Strength of Acids and Bases
8.3 Conjugate Acid-Base Pairs
8.4 Strength of Acids and Bases
8.4.1 Ionization Equation of Water and calculation of PH and POH in
aqueous medium using given Kw values.
8.4.2 Strong and weak acid
8.4.3 Strong and weak base
8.4.4 Relationship of Ka and Kb
8.6 Buffer Solutions and their Applications
8.7 Salt Hydrolysis

3. Introduction:
Acids:
sour taste
react with “active” metals
• e.g., Al, Zn, Fe, but not Cu, Ag, or Au
• 2 Al + 6 HCl → 2 AlCl3 + 3 H2
• corrosive
react with carbonates, producing CO2
• marble, baking soda, chalk, limestone
• CaCO3 + 2 HCl → CaCl2 + CO2 + H2O
change color of vegetable dyes
• blue litmus turns red
react with bases to form ionic salts
Bases:
also known as alkalis
taste bitter
• alkaloids = plant product that is alkaline
• often poisonous
solutions feel slippery
change color of vegetable dyes
• different color than acid
• red litmus turns blue
react with acids to form ionic salts
• neutralization

4. Properties of Salts:
Salts are water-soluble ionic compounds.
Salts that contain the cation of a strong base and an anion that is the conjugate
base of a weak acid are basic.
• NaHCO3 solutions are basic.
• Na+ is the cation of the strong base NaOH.
• HCO3
− is the conjugate base of the weak acid H2CO3.
Salts that contain cations that are the conjugate acid of a weak base and an
anion of a strong acid are acidic.
• NH4Cl solutions are acidic.
• NH4
+ is the conjugate acid of the weak base NH3.
• Cl− is the anion of the strong acid HCl.

5. 8.2: Bronsted Lowery Concepts for
Acids and Bases
• lone pair  bond
• bond  lone pair
Lewis acid–base theory focuses
on transferring an electron pair.
does NOT require H atoms
• electron rich; therefore, nucleophile
The electron donor is called the
Lewis base.
• electron deficient; therefore, electrophile
The electron acceptor is called
the Lewis acid.

6. Conjugate Acids Base Pairs

7. 8.4: Strength of Acids and Bases
Strong Acids:
An acid which can donate proton to a higher degree of than another acid is said to be strong
acid. For example HCl. Ability of an acid to donate proton is called strength of acids.
Strong Base:
A base which can accept proton to higher degree than another base is called strong base and
the ability of a base to accept proton is called strength of base. For example Ammonia is a
strong base.

8. Ionization Constant of Water and calculation of
pH and pOH Using Kw value
 Water is a unique compound, it can donate proton as well as accept
proton. Like that

11. Salt Hydrolysis
It is defined as the reaction of the cation or anion of the salt with water to
produce either acidic or basic solution.
Consider a salt 𝑴𝑿 is dissolved in water, It splits up into its 𝑴+ and 𝑿− ions.
Cations come from base and anions come from acid
𝑴+
+ 𝑯 − 𝑶𝑯 ↔ 𝑴𝑶𝑯 + 𝑯+
𝑿− + 𝑯 − 𝑶𝑯 ↔ 𝑯𝑿 + 𝑶𝑯−
Since 𝑯+
and 𝑶𝑯−
ions are produced in these reactions, the solution of the
salt may be acidic or basic.

12. Types of Salts on the basis
of reactivity with water
Salts of strong acid and strong base
Salts of weak acid and strong base
Salts of strong acid and weak base
Salts of weak acid and weak base

17. Type of Salt Common
examples
Ions which
impart
hydrolysis
Solution pH
Acid Base
Strong Strong NaCl, NaBr None =7.0 (Neutral)
Strong Weak 𝑵𝑯 𝟒 𝑵𝑶 𝟑, 𝑵𝑯 𝟒 𝑪𝒍 Cations <7.0 (Acidic)
Weak Strong NaCN, 𝑲 𝟐 𝑪𝑶 𝟑 Anions >7.0 (Basic)
Weak Weak 𝑵𝑯 𝟒 𝑪𝑵,
𝑵𝑯 𝟒 𝑵𝑶 𝟐
Both Smaller, Equal
or greater