This document discusses acids and bases according to several theories: - According to the Arrhenius theory, acids donate H+ ions and bases donate OH- ions in water. This theory does not explain behavior in non-aqueous solutions. - The Bronsted-Lowry theory states that acids are proton donors and bases are proton acceptors. Conjugate acids and bases are formed in acid-base reactions. - The Lewis theory defines acids as electron pair acceptors and bases as electron pair donors. Covalent bonds are formed between them. - Strong acids and bases fully dissociate in water while weak acids and bases only partially dissociate. Examples of strong and weak acids and bases are provided

1. ACIDS AND BASES
By:M.Divya

2. ACID
● Produce H+ ions in water
● Have a sour taste
● Breakdown metals
● Formula starts with H
● Poisonous and corrosive to skin
● PH less than 7

3. ACID
● Turns blue litmus to red
● Dissolve in water to form solution which conduct electricity
● React with reactive metals to form salt and hydrogen
● Acid reacts with carbonates and hydrogen carbonates to
form a salt,water and carbon dioxide
● Acid reacts with metal oxides and hydroxides to form a salt
and water

4. BASE
● Produce OH- ions in water
● Have a bitter taste and slippery feel
● Break down fats and oils
● Formula ends with OH
● Poisonous and corrosive to skin
● PH greater than 7

5. BASE
● Turn red litmus blue
● React with acids to form salt and water
● Heated with ammonium salts gives off ammonia
gas
● React with a solution of one metal salt to give
another metal salt and metal hydroxide

6. THEORIES OF ACIDS
AND BASES

7. Arrhenius Concept Of Acids and Bases
● According to the Arrhenius concept of acids and
bases,an acid is a substance that,when dissolved in
water,increases the concentration of hydronium
ion(H3
O+)
● It releases H+ ion in water
● The aqueous hydrogen ion is actually,chemically
bonded to water that is ,H3
O+

8. Arrhenius Concept Of Acids and Bases
● A base,in the Arrhenius concept,is a substance
that,when dissolved in water,increases the
concentration of hydroxide ion,OH-(aq)
● It releases OH- ion in water

9. Limitations Of Arrhenius Theory
● This theory does not explains the acidic
and basic behaviour of substance in
non-aqueous solvent

10. Bronsted-Lowry Acid and Bases
● Bronsted-Lowry acid can donate a proton
● Bronsted-Lowry base can accept a proton
● Must contain a non-bonding pairs of electrons
● Conjugate base of an acid is the species
remaining after the acid has lost a proton

11. Bronsted-Lowry Acids and Bases
● Conjugate acid is the species formed after the base has
accepted a proton
● HCl + H2
O ⟷ H3
O+
+ Cl-
● Water is conjugate base of H3
O+
and Cl-
is conjugate base of
HCl-
● Water can act as both Acid and base.Hence known as
Amphiprotic
● Strong acids have weak conjugate base
● Weak acids have strong conjugate base

12. Lewis Acids and Bases
● Bases can donate a pair of electrons
● Acids can accept a pair of electrons
● Covalent bond is formed
● Many Lewis Acid don’t contain hydrogen

13. Strong Acids and Bases
● Strong acid and base is completely dissociated into its ions in aqueous
solutions
● Strong acids have a PH of 0 to 3
● Strong base have a PH of 11 to 14
● Strong acids:
● HCl(Hydrochloric acid)
● HNO3
(Nitric acid)
● H2
SO4
(Sulfuric acid)
● Strong bases:
● NaOH(Sodium Hydroxide)
● KOH (Potassium Hydroxide)
● Ba(OH) (Barium Hydroxide)

14. Weak Acids and Bases
● Weak acids and bases is slightly dissociated into their ions in
aqueous solution
● Weak Acids:
● CH3
COOH (Ethanoic acid)
● H2
CO3
(Carbonic acid)
● Weak Bases:
● NH3
(Ammonia)
● C2
H5
NH2
(Amino ethane)

15. THANK YOU