2. Acids
Produce H+ ions in water
Have a sour taste
Break down 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 metal 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. Alkalis
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. Alkalis
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)
8. 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+).
Remember, however, that the aqueous hydrogen ion is actually
chemically bonded to water, that is, H3O+.
9. 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).
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
ACID: Ethanol (C2H5OH) =>weak
CONJUGATE BASE: Ethoxide ion (C2H5O-) => strong
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
15. Properties of Acids and Bases
Neutralization reaction with bases
With hydroxides to form salt and water
CH3COOH + NaOH NaCH3COO + H2O
With metal oxides to form a salt and water
H2SO4 + CuO CuSO4 + H2O
With ammonia to form salt
HCl + NH3 NH4Cl
16. Properties of Acids and Bases
With reactive metals to form salt and hydrogen
2HCl + Mg MgCl2 + H2
With carbonates to form salt, CO2, water
2HCl + CaCO3 CaCl2 + CO2 + H2O
With hydrogen carbonates to form salt, CO2, water
HCl + NaHCO3 NaCl + CO2 + H2O
17. 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)
19. 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)
21. Acidic oxides
Acidic oxides are the oxides of non-metals. When combined with
water, they produce acids, e.g.,
Acidic oxides are, therefore, known as acid anhydrides, e.g.,
Sulphur dioxide is sulphurous anhydride; Sulphur trioxide is
sulphuric anhydride.
22. Basic oxides
Basic oxides are the oxides of metals. If soluble in water they react with
water to produce hydroxides (alkalis).
Basic oxides do not reacts with alkalis.
Examples:
CaO + H2O Ca(OH)2
MgO + H2O Mg(OH)2
23. Amphoteric oxides
Amphoteric oxides are metallic oxides, which show both basic as
well as acidic properties. When they react with an acid, they
produce salt and water, showing basic properties. While reacting
with alkalis they form salt and water showing acidic properties
24. Neutral oxides
These are the oxides, which show neither basic nor acidic
properties, that is, they do not form salts when reacted with acids
or bases, e.g., carbon monoxide (CO); nitrous oxide (N2O); nitric
oxide (NO), etc., are neutral oxides.