THIS PPT WILL EXPLAIN YOU ALL ABOUT ACID AND BASE AND THEORIES OF ACID AND BASE . THIS IS VERY HELPFUL FOR THE STUDENTS FROM DIPLOMA AND BACHELOR PHARMACY STUDENTS.

1. ACID AND BASE
BY: SHIKHA AGRAWAL
NARAINA VIDYAPEETH GROUP
OF INSTITUTION

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
 turn blue litmus red
 Dissolve in water to form solution which conduct
electricity
 React with reactive metals to form salt and hydrogen
(explained)
 Acids react with carbonates and hydrogen carbonates to
form a salt, water and carbon dioxide (explained)
 Acids react with metal oxides and hydroxides to form a
salt and water only(explained)

4. BASE
 Produce OH- ions in water
 Have a bitter taste and a 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 only.(explained)
 Heated with ammonium salts gives off ammonia
gas.(explained)
 React with a solution of one metal salt to give another
metal salt and metal hydroxide.(explained)

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 (H3O+).
 It releases H+ ion in water .
 Remember, however, that the aqueous
hydrogen ion is actually chemically bonded to
water, that is, H3O+.

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. LIMITATION 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 pair of electrons
 Conjugate base of an acid is the species
remaining after the acid has lost a proton

11. Bronsted-Lowry Acid and Bases
 Conjugate acid is the species formed after the
base has accepted a proton
 HCl + H2O ↔ H3O+ + Cl-
 Water is conjugate base of H3O+ and Cl- is
conjugate base of HCl

12. Bronsted-Lowry Acid and Bases
 Water can act both as acid and base. Amphiprotic
 Strong acids have weak conjugate base
 Weak acids have strong conjugate base

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

14. Strong Acids and Bases
 Strong acid and base is completely dissociated
(ionized) into its ions in aqueous solutions
 Strong acids
HCl (Hydrochloric acid)
HNO3 (Nitric Acid)
H2SO4 (Sulfuric Acid)

15. Strong Acids and Bases
 Strong bases
NaOH (Sodium Hydroxide)
KOH (Potassium Hydroxide)
Ba(OH)2 (Barium Hydroxide

16. Weak Acids and Bases
 Weak acids and bases is slightly dissociated into
their ions in aqueous solution
 Weak acids
CH3COOH (Ethanoic Acid)
H2CO3(Carbonic acid)

17. Weak Acids and Bases
 Weak bases
NH3 (Ammonia)
C2H5NH2 (Amino ethane)

18. THANK YOU