Acids Bases and Salts - Revision Notes

 CBSE Class 10 Science

Revision Notes
CHAPTER – 2
ACIDS, BASES AND SALTS


Acids

Bases

Sour in taste
Derived from Greek word' ACIDUS'

Bitter in taste

Changes blue litmus into red

Changes red litmus into blue

e.g. Hydrochloric acid HCl

e.g. Sodium hydroxide NaOH

Sulphuric acid H2SO4

Potassium hydroxide KOH

Nitric acidHNO3

Calcium hydroxideCa(OH)2

Acetic acidCH3COOH

Ammonium hydroxide

  • Some naturally occurring acids

Vinegar

Acetic Acid

Orange

Citric Acid

Lemon

Citric Acid

Tamarind

Tartaric Acid

Tomato

Oxalic Acid

Sour milk (Curd)

Lactic Acid

Ant and Nettle sting

Methanoic Ac

  • Acid – Base Indicator:Substances which indicate the presence of an acid or base in a solution.
  • Litmus solution – It is a natural indicator. It is a purple dye extracted from Lichens. Other examples are Red Cabbage and coloured petals of Petunia and turmeric.
  • Olfactory indicators : Show odour changes in acidic or basic media. E.g. onion and clove .
  • Acid – Base Indicators

S.No.

Name of the Indicator

Colour Change With Acid

Colour Change with Base

A.

Blue litmus solution

To red

No change

B.

Red litmus solution

No change

To blue

C.

Turmeric

No change

To red

D.

Methyl orange

To red

To yellow

E.

Phenolphthalein (colourless)

No change

To pink

  • Dilute Acid : A dilute acid contains a small amount of acid (lower concentration of hydronium ions)and a large amount of water.
  • Concentrated Acid :A concentrated acid contains a large amount of acid (higher concentration of hydronium ions)and a small amount of water.
  • Chemical Properties of Acids and Bases
  1. Reaction with metal

Acid+MetalSalt+Hydrogen

2HCl+ZnZnCl2+H2

2HNO3+ZnZn(NO3)2+H2

H2SO4+ZnZnSO4+H2

2CH3COOH+Zn(CH3COO)2Zn+H2

  • Pop test : When a burning candle is brought near a test tube containing hydrogen gas it burns with a ‘Pop’ sound. This test is conducted for examining the presence of hydrogen gas.
  • Base + Metal  Salt + Hydrogen

NaOH+ZnNa2ZnO2+H2SodiumZincate

Note– Such reactions are not possible with all the metals.

  • Actions of Acids with metal Carbonates and metal bicarbonates

MetalCarbonate+Acid Salt+Carbondioxide+Water

Na2CO3(aq) 2NaCl(aq)+CO2(g)+H2O(l)

Metalbicarnonate+Acid Salt+Carbondioxide+Water

NaHCO3+HCl NaCl+CO2+H2O

  • Lime water Test : On passing the evolved CO2 gas through lime water, we find that lime water turns milky.

Ca(OH)2(aq)Limewater+CO2(g) CaCO3(s)+H2O(l)Whiteprecipitate

  • CO2 the following reaction takes place

CaCO3(s)+H2O(l)+CO2(g)Ca(HCO3)2aq(solublein water)

  • Reaction of acids and bases with each other to give salt and water are called Neutralisation Reactions

Base+AcidSalt+Water

e.g. NaOH(aq)+HCl(aq) NaCl(aq)+H2O(l)

  • Reactions of metal oxides with acids

MetalOxide+AcidSalt+Water

CuOCopperoxide+HClHydrochloricacidCuCl2CopperChloride+H2OWater

Note : Appearance of blue green colour of the solution because of formation of CuCl2.

Metallic oxides are said to be basic in nature because they give salt and water on reacting with acids.Some metallic oxides react with both acids and base and are called AMPHOTER-
IC OXIDES.

  • Reaction of Non Metallic Oxide with Base

Non-metallic oxide+ Base Salt + Water

CO2+Ca(OH)2CaCO3+H2O

Note : Non Metallic oxides are said to be acidic in nature because on reacting with a base they produce salt and water.

  • All acidic solutions conduct electricity because of formation of (H+)ions in aq. solution.
  • Glowing of bulb indicates that there is a flow of electric current through the solution.
  • Acids or bases in a Water Solution

Acids produceH+ions in the presence of water

HCl+H2OH3O++Cl

H3O+ : Hydronium ion.

H+ion cannot exist alone. It exists as H+(aq)or(H3O+) hydronium ion.

i.e. Base provide OH(aq) ions in the presence of water

NaOH(s)H2ONa+(aq)+OH(aq)

KOH(s)H2OK+(aq)+OH(aq)

Mg(OH)2(s)H2OMg2+(aq)+2OH(aq)

  • Alkalis

All bases do not dissolve in water. An alkali is a base that dissolves in water.Common alkalis are

  • NaOH Sodium hydroxide
  • KOH Potassium hydroxide
  • Calcium hydroxide
  • Ammonium hydroxide

Note : All alkalis are bases but all bases are not alkalis.

  • Precaution must be taken while mixing acid or base with water. The acid must always be added to water with constant stirring as it is a highly exothermic reaction.

When an acid or a base is mixed with water they become dilute. This results in the decrease in the concentration of per unit volume in acids and bases respectively,i.e. no. of H+ionand OHion reduces.

  • Strength of an Acid or Base

Strength of acids and bases depends on the no. of H+ionand OHionproduced respectively.

With the help of a universal indicator we can find the strength of an acid or base as it shows different colours at different concentrations of hydrogen ions in a solution.

A scale for measuring hydrogen ion conc. in a solution called pH scale has been developed.

pH= Potenz in German means power.

This scale measures from 0 (very acidic) to 14 (very alkaline) 7 indicates

Neutral pH (water is neutral).

pH paper : Is a paper which is used for measuring pH

Variation of PH

S. No. PH Colour of the Nature of Solution H+ion Conc. OHion Conc.

Value pH Paper

1.

0

Dark red

Highly acidic

Very high

Very low

2.

4

Orange or yellow

Acidic

High

Low

3.

7

Green

Neutral

Equal

Equal

4.

10

Bluish green or blue

Alkaline

Low

High

5.

14

Dark blue or violet

highly basic

very low

Very high

Importance of pH in our daily life

  • Importance of pH in our digestive system – Our stomach produces hydrochloric acid. This dilute hydrochloric acid help in digestion of food. In case of indigestion our stomach produces acid in a very large quantity because of which we feel pain and irritation in our stomach (ACIDITY).To get relief from this pain ,antacids are used. These antacids neutralize the excess acid because they are basic in nature and we get relief.
  • pH of Acid Rain : When pH of rain water is less than 5.6 it is called acid rain. Flow of acidic rain in water bodies makes them acidic causing a threat to the survival of aquatic life.It also results in damage of structures made with marble like Taj Mahal.
  • pH of Soil : Plants require a specific range of pH for their healthy growth. If pH of soil of any particular place is less or more than normal then the farmers add suitable chemicals to it. The addition of these chemicals of presences of excessive damage the nutrients of the soil and decrease its natural fertility.
  • Our body functions between the pH range of 7.0 to 7.8. Living organisms can survive only in the narrow range of pH change.
  • Tooth decay and pH : Bacteria present in the mouth produces acids by degradation of sugar and food particles remaining in the mouth. Tooth decay begins below the pH 5.6. Using toothpaste which is generally basic, can neutralise the excess acid and prevent tooth decay.
  • Bee sting or Nettle sting contains methanoic acid which causes pain and irritation. Using a weak base like baking soda neutralises the acid giving relief.

Salts and their Derivation

S. No.

Name of Salt

Formula

Derived from

Derived from

1.

Potassium Sulphate

K2SO4

KOH

H2SO4

2.

Sodium Sulphate

Na2SO4

NaOH

H2SO4

3.

Sodium Chloride

NaCl

NaOH

HCl

4.

Ammonium Chloride

NH4Cl

NH4OH

HCl

Note : NaCl andNa2SO4belong to the family of sodium salts as they have the same radicals. Similarly NaCl and KCl belong to the family of chloride salts.

Neutral Salts : Strong Acid + Strong base

pH value is 7

e.g.NaCl, CaSO4

Acidic Salts : Strong Acid + weak base

pH value is less than 7

eq.NH4Cl,NH4NO3

Basic Salts : Strong base + weak acid

pH value is more than 7

e.g.CaCO3,CH3COONa

  • NaCl

Sodium chloride is called as common salt. It is derived from sea water.

Rock Salt is mined like coal, is brown coloured and crystalline is shape.

Preparation :

Sodium chloride is obtained by mining the deposits and brine solution is obtained by passing water into the deposits. Hence the salts get dissolved then the solution is pumped out. Evaporation of the sea water is one of the major processes used to obtain salt . The crystals obtained usually consists of impurities such as calcium sulphate, sodium sulphate etc. Pure crystals are obtained by dissolving the salts with little water and filtering the solution.

Uses

  • Common salt is an important raw material for many materials of daily use such as.
  • Sodium hydroxide
  • Washing Soda
  • Bleaching Power.
  • 2. Used in our food as a preservative and provides flavour to food.
  • 3. Used in industries
  •  
  • Sodium Hydroxide : NaOH, Common Name – caustic soda.

Preparation : Prepared by the method called chlor-alkali process. It is called so because we get chlorine and an alkali (NaOH) in this process.

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

  • Calcium oxy chloride -- CaOCl2
  • The chlorine gas released in brine formation is used to prepare bleach.

Ca(OH)2CalciumHydroxide+Cl2Chlorine CaOCl2bleachingpowder+H2OWater

Uses

(1) for bleaching cotton and linen in textile industries,wood pulp in paper industry,

(2) Used as disinfectant of water

{3} Used as an oxidising agent.

III. Sodium Hydrogen Carbonate – NaHCO3

Common name – Baking Soda. It is mild corrosive base

Preparation :

  1. Used in baking/cooking

Heating NaHCO3+H2O+CO2

NaHCO3heat Na2CO3+H2O+CO2

  1. produced causes dough to rise and help to make cakes and pastries spongy.

2.Used as ingredients of antacids

3.For preparinf baking soda(baking powder+mild edible acid)

4. Used in soda-acid extinguishers.

Washing Soda

Preparation :Recrystallisation of sodium carbonate.

Na2CO3+10H2OHeat Na2CO3.10H2O

It is a basic salt used in

  • manufacture of Borax.
  • `glass,soap and paper industries
  • cleansing agent for domestic purposes.
  • removing permanent hardness of water.

Water of Crytallization: fixed number of water molecules present in on formula unit of a salt.

Eg:

  • CuSO4.5H2O
  • CaSO4.2H2O
  • CaSO4.12H2O

Plaster of Paris

CaSO4.2H2O373KCaSO412H2Oa

When Plaster of Paris is mixed with water it changes to gypsum.

CaSO4.12H2O+112H2O CaSO4.2H2OPOPGYPSUM

: Making toys, decorative material and smoothening surfaces,

plaster for fractured bones.

What you have learnt

Acid-base indicators are dyes or mixtures of dyes which are used to indicate the presence of acids and bases.

  • Acidic nature of a substance is due to the formation of H+(aq) ions in solution. Formation of OH–(aq) ions in solution is responsible for the basic nature of a substance.
  • When an acid reacts with a metal, hydrogen gas is evolved and a corresponding salt is formed.
  • When a base reacts with a metal, along with the evolution of hydrogen gas a salt is formed which has a negative ion composed of the metal and oxygen.
  • When an acid reacts with a metal carbonate or metal hydrogen carbonate, it gives the corresponding salt, carbon dioxide gas and water.
  • Acidic and basic solutions in water conduct electricity because they produce hydrogen and hydroxide ions respectively.
  • The strength of an acid or an alkali can be tested by using a scale called the pH scale (0-14) which gives the measure of hydrogen ion concentration in a solution.
  • A neutral solution has a pH of exactly 7, while an acidic solution has a pH less than 7 and a basic solution a pH more than 7.
  • Living beings carry out their metabolic activities within an optimal pH range.
  • Mixing concentrated acids or bases with water is a highly exothermic process.
  • Acids and bases neutralise each other to form corresponding salts and water.
  • Water of crystallisation is the fixed number of water molecules chemically attached to each formula unit of a salt in its crystalline form.
  • Salts have various uses in everyday life and in industries.