Notes of Ch 2 Acids, Bases and Salts | Class 10th Science

Study Material and Notes of Ch 2  Acids, Bases and Salts Class 10th Science

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 Hydrogencarbonates
• 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
• Importance of pH in everyday life
→ What is pH?
→ pH sensitivity of Animals and Plants
→ pH of the soil
→ pH in our digestive system
→ cause of tooth decay
→  Self defence by animals and plants through chemical warfare
→ pH of Salts
• Chemicals from Common Salt (NaCl)
→ Sodium Hydroxide (NaOH)
→ Bleaching Powder (CaOCl2)
→ Baking Soda (NaHCO3)
→ Washing Soda (Na2CO3.10H2O)
→ Plaster of Paris (CaSO4.½H2O)
• Water of Crystallization

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: HCl, H2 SO4 , 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:
(i) Natural indicators
(ii) Synthetic indicators
(iii) Olfactory indicators

(i) Natural indicators: Found in nature in plants. Examples: Litmus, red cabbage leaves extract, flowers of hydrangea plant, turmeric.

(ii) Synthetic indicators: These are chemical substances. Examples: Methyl orange, phenolphthalein.

(iii) 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 

→ 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

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

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 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
• 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
• Importance of pH in everyday life
→ What is pH?
→ pH sensitivity of Animals and Plants
→ pH of the soil
→ pH in our digestive system
→ cause of tooth decay
→  Self defence by animals and plants through chemical warfare
→ pH of Salts
• Chemicals from Common Salt (NaCl)
→ Sodium Hydroxide (NaOH)
→ Bleaching Powder (CaOCl2)
→ Baking Soda (NaHCO3)
→ Washing Soda (Na2CO3.10H2O)
→ Plaster of Paris (CaSO4.½H2O)
• Water of Crystallization

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