Acids Bases and Salts Class 10 PDF

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Acids Bases and Salts Class 10

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Through our post, students can easily get Class 10 important notes and topics of Acids Bases and Salts in pdf form which can very beneficial for the students to get the high score in the exam. To understand Class 10 Chemistry, it is essential to understand Acids, Bases and Salts first because they form the basis of Chemistry.

Class 10 Chapter 2 Acids, Bases and Salts explains all the essential concepts that students need to know to understand how the chemical reaction happens and how these chemical substances work. To know more meaningful information related to this chapter you can read this article till the end.

Acids Bases and Salts Class 10 PDF: Introduction

Elements combine to form numerous compounds. On the basis of their chemical properties, compounds
can be classified into three categories:

1. Acids
2. Bases
3. Salts

Acids and Bases in the Laboratory

Indicators

An indicator tells us whether a substance is acidic or basic in nature, by the change in colour.

Common Indicators

• An acid turns blue litmus red and a base turns red litmus blue.
• Methyl orange indicator gives a red colour in an acidic solution and gives a yellow colour in a basic solution.
• Phenolphthalein is colourless in an acidic solution and gives a pink colour in a basic solution.

Olfactory Indicators

• Those substances whose odour changes in acidic or basic media are called olfactory indicators. For example onion, vanilla and clove oil.
• On adding sodium hydroxide solution to a cloth strip treated with onion, the smell of the onion is not detected. An acidic solution does not eliminate the smell of the onion.

Reaction of Acids & Bases with Metals

Acids react with metals to produce salt by displacing hydrogen.

For Example:

i. When dilute sulphuric acid reacts with the metal zinc, zinc sulphate is formed with the evolution of hydrogen gas.

Zn + H2SO4 → ZnSO4 + H2

ii. Zinc is the only metal which reacts with sodium hydroxide to form sodium zincate with the release of hydrogen gas.

Zn + 2NaOH → Na2ZnO2 + H2

Reaction of Metal Carbonates & Bicarbonates with Acids

Acids react with metal carbonates or bicarbonates to form salt and water with the evolution of carbon dioxide gas.

For Example:

i. Hydrochloric acid reacts with sodium carbonate to form sodium chloride and water with the release of carbon dioxide gas.

Na2CO3(s) + 2 HCl(aq) → 2NaCl(aq) + CO2(g) + H2O(l)

ii. Similarly, sodium bicarbonate also reacts with hydrochloric acid to form sodium chloride and water with the release of carbon dioxide gas.

NaHCO3(s) + HCl (aq) → NaCl (aq) + CO2(g) + H2O(l)

Reaction of Metallic Oxides with Acids

Acids react with metallic oxides to form salt and water.

For Example:

Copper oxide (II), a black metal oxide reacts with dilute hydrochloric acid to form a blue-green coloured copper chloride (II) solution.

CuO + 2HCl → CuCl2(aq) + H2O

Reaction of Non-Metallic Oxides with Base

Bases react with non-metallic oxides to form salt and water.

For Example:

Calcium hydroxide reacts with non-metallic oxides like carbon dioxide to form calcium carbonate salt and water.

Ca(OH)2 + CO2 → CaCO3 + H2O

Manufacture of Acids and Bases

a) Nonmetal oxide + water → acid

SO₂(g) + H₂O(l) → H₂SO₃(aq)
SO₃(g) + H₂O(l) → H₂SO₄(aq)
4NO₂(g) + 2H₂O(l) + O₂(g) → 4HNO₃(aq)

Non-metal oxides are thus referred to as acid anhydrides.

b) Hydrogen + halogen → acid

H₂(g) + Cl₂(g) → 2HCl(g)
HCl(g) + H₂O(l) → HCl(aq)

c) Metallic salt + conc. sulphuric acid → salt + more volatile acid
2NaCl(aq) + H₂SO₄(aq) → Na₂SO₄(aq) + 2HCl(aq)
2KNO₃(aq) + H₂SO₄(aq) → K₂SO₄(aq) + 2HNO₃(aq)

d) Metal + oxygen → metallic oxide (base)
4Na(s) + O₂(g) → 2Na₂O(s)
2Mg(s) + O₂(g) → 2MgO(s)

e) Metal + water → base or alkali + hydrogen
Zn(s) + H₂O(steam) → ZnO(s)+ H₂(g)

f) Few metallic oxides + water → alkali
Na₂O(s) + H₂O(l) → 2NaOH(aq)

g) Ammonia + water → ammonium hydroxide
NH₃(g) + H₂O(l) → NH₄OH(aq)

Acids and Bases in Water

Acids

An acid is a substance which dissociates (or ionises) when dissolved in water to release hydrogen ions.

For Example:

An aqueous solution of hydrochloric acid dissociates to form hydrogen ions. Since hydrogen ions do not exist as H+
in solution, they combine with polar water molecules to form hydronium ions [H3O+].

HCl (aq) → H+(aq) + Cl-(aq)

H+ + H2O → H3O+

The presence of hydrogen ions [H+] in hydrochloric acid solution makes it behave like an acid.

Bases

A base is a substance which dissolves in water to produce hydroxide ions [OH- ions].

Bases which are soluble in water are called alkalis.

For Example:

Sodium hydroxide dissolves in water to produce hydroxide and sodium ions.
NaOH (aq) → Na+   (aq) + OH-    (aq)

The presence of hydroxide ions [OH-] in sodium hydroxide solution makes it behave like a base.

Difference between a base and an alkali

Base:

• Bases undergo a neutralisation reaction with acids.
• They are comprised of metal oxides, metal hydroxides, metal carbonates and metal bicarbonates.
• Most of them are insoluble in water.

Alkali:

• An alkali is an aqueous solution of a base, (mainly metallic hydroxides).
• It dissolves in water and dissociates to give OH⁻ ion.
• All alkalis are bases, but not all bases are alkalis.

More about Salts

Salts having the same positive ions (or same negative ions) are said to belong to a family of salts.

pH of Salts

Salts of strong acid and a strong base are neutral, with a pH value of 7.

For Example: NaCl, Na2SO4

Salts of strong acid and weak base are acidic, with a pH value of less than 7.

For Example: The ammonium chloride solution has a pH value of 6.

Salts of a weak acid and strong base are basic, with a pH value of more than 7.

For Example: Sodium carbonate solution has a pH value of 9.

Common Salt

Chemical name: Sodium chloride

Common salt is a neutral salt and can be prepared in the laboratory by the reaction of sodium hydroxide and hydrochloric acid.

NaOH(aq) + HCl(aq) → NaCl(aq) + H2O(aq)

It is an important raw material for products of daily use such as NaOH, baking soda, washing soda and bleaching powder.

Sodium Hydroxide

Sodium hydroxide is produced by the electrolysis of an aqueous solution of sodium chloride (called brine).

The process is called the chlor-alkali process because of the products formed, i.e. ‘chlor’ for chlorine and ‘alkali’ for sodium hydroxide.

2NaCl(aq) + 2H2O(aq) → 2NaOH(aq) + H2(g) + Cl2(g)

Arrhenius Theory of Acids and Bases

Arrhenius acid – when dissolved in water, dissociates to give H⁺ (aq) or H₃O⁺ ion.
Arrhenius base – when dissolved in water, dissociates to give OH⁻ ion.

Examples:

Acids 

• Hydrochloric acid (HCl)
• Sulphuric acid  (H₂SO₄)
• Nitric acid (HNO₃)

Bases

• Sodium hydroxide (NaOH)
• Potassium hydroxide (KOH)
• Calcium hydroxide (Ca(OH)₂)

Importance of pH in Everyday life

1. pH sensitivity of plants and animals

Plants and animals are sensitive to pH. Crucial life processes such as digestion of food, and functions of enzymes and hormones happen at a certain pH value.

2. pH of a soil

The pH of soil optimal for the growth of plants or crops is 6.5 to 7.0.

3. pH in the digestive system

The process of digestion happens at a specific pH in our stomach which is 1.5 to 4.
The pH of the interaction of enzymes, while food is being digested, is influenced by HCl in our stomach.

4. pH in tooth decay

Tooth decay happens when the teeth are exposed to an acidic environment of pH 5.5 and below.

5. pH of self-defence by animals and plants

Acidic substances are used by animals and plants as a self-defence mechanism. For example, bees and plants like nettle secrete a highly acidic substance for self-defence. These secreted acidic substances have a specific pH.

What Is an Acid and a Base?

Ionisable and Non-Ionisable Compounds

• An ionisable compound when dissolved in water or in its molten state, dissociates into ions almost entirely. Example: NaCl, HCl, KOH, etc.
• A non-ionisable compound does not dissociate into ions when dissolved in water or in its molten state. Example: glucose, acetone, etc.

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