1. The Chemical Properties of Acids and Bases

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Chapter 2

Acids, Bases & Salts

 

Introduction

• A substance that tastes sour in water, turns blue litmus red, and neutralises bases is known as an acid.
• If a substance’s aqueous solution tastes bitter, turns red litmus blue, or neutralises acids, it’s called a base.
• Salt is a neutral material that has no effect on litmus in aqueous solution.

Acids and Bases Reactions

A neutralisation reaction occurs when an acid reacts with a base. A salt and water are the end products of this reaction. An acid–base neutralisation reaction is formulated as a double-replacement reaction in this standard approach.

Reaction of Acid & Bases

a) Reaction of Acid & Bases with Metals

Acids, in general, react with metals to produce salt and hydrogen gas. Bases, in general, do not react with metals and do not produce hydrogen gas.
Acid + active metal → Salt + hydrogen + heat
2HCl + Mg → MgCl₂ + H₂ (↑)
Hydrochloric acid + Magnesium → Magnesium chloride + Hydrogen
Base + metal → Salt + hydrogen + heat
2NaOH + Zn → Na₂ZnO₂ + H₂ (↑)
Sodium hydroxide + Zinc → Sodium zincate + Hydrogen
A more reactive metal displaces the less reactive metal from its base.
2Na + Mg (OH) ₂ → 2NaOH + Mg
Sodium + Magnesium hydroxide → Sodium hydroxide + Magnesium

b) Reaction of Acids with metal carbonates and bicarbonates

Acids produce carbon dioxide, as well as metal salts and water, when they react with metal carbonates or metal bicarbonates. Sodium chloride, carbon dioxide, and water are formed when sodium carbonate interacts with hydrochloric acid. Allowing carbon dioxide gas to travel through lime water turns it milky.

Acid + metal carbonate or bicarbonate → salt + water + carbon dioxide.
2HCl + CaCO₃ → CaCl₂ + H₂O + CO₂
H₂SO₄ + Mg (HCO₃)₂ → MgSO₄ + 2H₂O + 2CO₂
Effervescence indicates liberation of CO₂ gas.

c) Reaction of Acid with base

1. Reaction of metal oxides and hydroxides with acids
Metal oxides or metal hydroxides are basic in nature.
Acid + base → salt + water + heat

H₂SO₄ + MgO → MgSO₄ + H₂O
2HCl + Mg (OH) ₂ → MgCl₂ + 2H₂O

2. Reaction of non-metal oxides with bases

Non-metal oxides are acidic in nature
Base + Nonmetal oxide →  salt + water + heat

2NaOH + CO₂→ Na₂CO₃ + H₂O

3. Reaction of acids and base

A very common acid is hydrochloric acid. The reaction between strong acid says hydrochloric acid and strong base say sodium hydroxide forms salt and water. The complete chemical equation is shown below.
HCl (strong acid) + NaOH (strong base) → NaCl (salt) + H₂O (water)