MG SCHOOL SCIENCE: Ch 2 Acids, Bases and Salts ppt

Class 10th Science Notes

Chapter 2 Acids, Bases and Salts

Topics in the Chapter

Introduction
Properties of Acids
Properties of Bases
Types of Indicators and its properties
Reaction of Acids and Bases with Metals
Reaction of Acids with Metal Carbonates and Metal Hydrogen carbonates
Reaction of Acids and Bases with each other
Reaction of Metallic Oxides with Acids
Reaction of a Non-metallic Oxide with Base
Similarities between all Acids and all Bases
Acid or Base in Water Solution
Strength of Acids and Base solutions

Introduction

The sour and bitter tastes of food are due to acids and bases are present in them.

Acids are sour in taste and change the colour of blue litmus to red.

Litmus solution is a purple dye, which is extracted from lichen. When the litmus solution is neither acidic nor basic, its colour is purple.

Other natural materials like red cabbage leaves, turmeric, coloured petals of some flowers such as Hydrangea, Petunia and Geranium, which indicate the presence of acid or base in a solution.

Properties of Acids

The term 'acid' has been derived from the Latin word, 'acidus' which means sour.
Acids have sour taste.
They turn blue litmus solution red.
They give H+ ions in aqueous solution.

Strong Acids: HCI, H2 504 , HNO3

Weak Acids: CH3COOH, Oxalic acid, Lactic acid

Concentrated Acids: More amount of acid + Less amount of water

Dilute Acids: More amount of water + Less amount of acid

Properties of Bases

These are the substances which are bitter in taste and soapy in touch.
They turn red litmus solution blue.

They give OH- ions in aqueous solution.

Strong Bases: NaOH, KOH, Ca(OH)2

Weak Bases: NH4OH

Alkalis: These are bases which are soluble in water.

Examples: NaOH, KOH, Ca(OH)2.

Types of Indicators and its properties

Indicators: Substances which change their colour/smell in different types of substances (like acids and bases).

Types of Indicators:

1. Natural indicators

2. Synthetic indicators

3. Olfactory indicators

Natural indicators: Found in nature in plants.

Examples: Litmus, red cabbage leaves extract, flowers of hydrangea plant, turmeric.

Synthetic indicators: These are chemical substances.

Examples: Methyl orange, phenolphthalein.

Olfactory indicators: These substances have different odour in acid and bases.

Reaction of Acids and Bases with Metals

Reaction of Acids with Metals:

Acids react with metal to form metal salt and releases Hydrogen Gas.

Acid + Metal → Salt + Hydrogen Gas

Example: Zinc granules react with dilute Hydrochloric acid in a test tube.

2HCl + Zn → ZnCl2 + H2

Hydrogen gas released can be tested by bringing burning candle near gas bubbles, it burst with pop sound.

Reaction of Bases with Metals

Bases react with metal to evolve hydrogen Gas. Also, note that all metals do not react with bases. The metal must be more reactive than the metals present in the base for the reaction to take place.

Base + Metal → Salt + Hydrogen gas

Example: Zinc granules react with NaOH solution to form sodium zincate and evolve hydrogen gas.

2NaOH + Zn → Na2ZnO2 + H2

Reaction of Acids with Metal Carbonates and Metal Hydrogencarbonates

Acids reacts with Metal Carbonates and Metal Hydrogencarbonates to form Salt, Carbon dioxide and water.

Metal carbonate/Metal hydrogen carbonate + Acid → Salt + Carbon dioxide + Water

Examples:

(i) 2HCl + Na2CO3 → 2NaCl + CO2 + H2O

(ii) HCl + NaHCO3 → NaCl + CO2 + H2O

>CO2 can be tested by passing it through lime water. It turns lime water milky.

Ca(OH)2 + CO2 → CaCO3 + H2O

>When excess CO2 is passed, milkiness disappears.

CaCO3 + CO2 + H2O → Ca(HCO)3

>Bases do not react with Metal Carbonates and Metal Hydrogencarbonates.

Base + Metal Carbonate/Metal Hydrogen Carbonate → No Reaction

Reaction of Acids and Bases with each other

Acids and Bases react to form salt and water.

Acid + Base → Salt + H2O

Neutralisation Reaction: Reaction of acid with a base is called as neutralization reaction.

Example: HCl + NaOH → NaCl + H2O

Strong Acid + Weak Base → Acidic salt + H2O
Weak Acid + Strong Base → Basic salt + H2O
Strong Acid + Strong Base → Neutral salt + H2O
Weak Acid + Weak Base → Neutral salt + H2O

Reaction of Metallic Oxides with Acids

Metallic oxides are basic in nature.

Example: CaO, MgO are basic oxides.Metallic Oxide + Acid → Salt + H2O

CaO + 2HCl → CaCl2 + H2O

Reaction of Non-metallic Oxides with Bases

Non-metallic oxides are acidic in nature.

Non-metallic Oxide + Base → Salt + H2O

CO2 + Ca(OH)2 → CaCO3 + H2O

Reaction of Acid

(i) Acid + Metal Carbonate → Salt + CO2 + Water

(ii) Acid + Metal → Salt + H2

(iii) Acid + Metal Hydrogen Carbonate → Salt + CO2 + H2O

(iv) Acid + Metallic oxide → Salt +H2O

(v) Acid + Base → Salt + H2O

Reaction Of Base

(i) Base + Metal → Salt + H2

(ii) Base + Metal Carbonate → No Reaction

(iii) Base + Metal Hydrogen Carbonate → No Reaction

(iv) Base + Acid → Salt + H2O

(v) Base + Non Metallic oxide → Salt + H2O

Similarities between all Acids and all Bases

All acids have H+ ions in common.
Acids produce H+ ions in solution which are responsible for their acidic properties.
All bases have OH- (hydroxyl ions) in common

Acid or Base in Water Solution

Acids produce H+ ions in presence of water.
H+ ions cannot exist alone, they exist as H3O+ (hydronium ions).

H+ + H2O-->H3O+

HCl + H2O → H3O+ + Cl-

Bases when dissolved in water gives OH − ions.

Bases soluble in water are called alkali.
While diluting acids, it is recommended that the acid should be added to water and not water to acid because the process of dissolving a acid or a base in water is highly exothermic.