The document discusses the properties and reactions of acids, bases, and salts, including indicators for identifying them. It explains the pH scale, the importance of pH in daily life, and various applications of compounds like sodium chloride, baking soda, and washing soda. Additionally, it highlights the role of these substances in digestion, tooth decay, and industrial processes.

1. Acids,
Bases and
Salts

2. Handwritten Digitalised
Notes + PYQs (10 Years)

3. FREE QUIZ + DPP
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4. The sour and bitter
tastes of food are due to
acids and bases, respectively,
present in them.

5. Litmus ki baat!
Acid turns BLUE litmus RED!
Base turns RED litmus BLUE!
AB ROAD!

6. An indicator tells us whether the given substance is an
acid or a base by the change in it's colour!
For now, we need to know about 3 types of indicators

7. Natural Indicators : Indicators which are obtained naturally are called
natural indicators, for example: Litmus, red cabbage, turmeric,
onion, vanilla, clove, etc
Synthetic Indicators - Synthetic indicators are obtained from artificial
substances that are synthesized in laboratories Ex: Methyl
Orange, Phenolphthalein.
Olfactory Indicators - Substances which change their odour with acid
and base are called olfactory indicators. Vanilla, cloves, onion, etc.
TYPES OF INDICATORS

8. Acids are ionic compounds that, when dissolved in water,
produce positive hydrogen ions ( H+) When dissolved in water,
acids taste acidic, conduct electricity and react with metals to
create hydrogen gas.
Bases are those substances which have bitter taste.
They turn red litmus to blue. Those bases which are
soluble in water are called alkali. A base is a substance
which dissolves in water to produce hydroxide in the
solution. For Example: NaOH,KOH, Mg(OH) 2 , NH 4OH.
ACIDS
BASES

10. Acids that give high concentration of H+ ions on
ionisation in aqueous solution are said to be strong acids
and acids which give less H+ ions on ionisation in
aqueous solution are said to be weak acids. Ex of strong
acids : Hydrochloric acid and nitric acid
Strong Acids
Strong Bases
A base which which completely ionises in water and
produce large amount of hydroxide ions. Ex: NaOH, KOH

11. HOW DO ACIDS AND BASES REACT WITH METALS?
ACID + METAL →SALT + HYDROGEN GAS
Zn + H2SO4→ZnSO4 + H2

12. HOW DO METAL CARBONATES AND METAL HYDROGENCARBONATES
REACT WITH ACIDS?

13. Limestone, chalk and marble are
different forms of calcium
carbonate.
All metal carbonates and
hydrogencarbonates react with
acids to give a corresponding salt,
carbon dioxide and water.

14. ACID AND BASE REACTION
Base + Acid →Salt + Water

15. REACTION OF METALLIC OXIDES WITH ACIDS
Metal oxide + Acid →Salt + Water
2HCl+CuO⟶CuCl2+H2O

16. REACTION OF A NON-METALLIC
OXIDE WITH BASE
Non- Metal oxide + Base →Salt + Water

17. Both acids and bases are electrolytes
which means that they're good
conductors of electricity. Acids and
bases both produce ions in water
solution.
WHAT DO ACIDS AND
BASES HAVE IN COMMON?

18. Acid or Base in Water Solution
Hydrogen ions in HCl are produced in the presence of water. The separation of H+ ion
from HCl molecules cannot occur in the absence of water.

19. All bases do not dissolve in water. An alkali is a base that
dissolves in water.
They are soapy to touch, bitter and corrosive. Don't taste
or touch them as they may cause harm. (dikkat hojayegi)
Alkalis

20. HOW STRONG ARE ACID OR BASE SOLUTIONS?
A scale for measuring hydrogen ion concentration in a solution, called pH scale
has been developed .
On the pH scale we can measure pH from 0 (very acidic) to 14 (very alkaline). pH
should be thought of simply as a number which indicates the acidic or basic
nature of a solution.
Higher the hydronium ion concentration, lower is the pH value.

22. Importance of pH in
Everyday Life
Our body works within the pH range of 7.0 to 7.8.
When pH of rain water is less than 5.6, it is called acid rain.
When acid rain flows into the rivers, it lowers the pH of the river water.
The survival of aquatic life in such rivers becomes difficult.

23. pH in our Digestive System!
Our stomach produces hydrochloric acid.
It helps in the digestion of food without harming
the stomach.
During indigestion the stomach produces too
much acid and this causes pain and irritation.
Antacids are used to cure this.
Magnesium hydroxide (Milk of magnesia), a mild
base, is often used forthis purpose.

24. pH in mouth
Tooth decay starts when the pH of the mouth is lower than 5.5.
Tooth enamel, made up of calcium phosphate is the hardest substance in the
body.
It does not dissolve in water, but is corroded when the pH in the mouth is below 5.5.
Bacteria present in the mouth produce acids by degradation of sugar and food
particles remaining in the mouth after eating.

25. Naturally Occuring Acids

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

27. Sodium Chloride (Nacl)
The common salt thus obtained is an
important raw material for various
materials of daily use, such as sodium
hydroxide, baking soda, washing
soda, bleaching powder and many more.

28. When electricity is passed through an aqueous
solution of sodium chloride (called brine), it
decomposes to form sodium hydroxide.
The process is called the chlor-alkali process
because of the products formed– chlor for chlorine
and alkali for sodium hydroxide.
Sodium hydroxide (NaOH)

29. USES

30. Chlorine is produced during the electrolysis of aqueous sodium
chloride (brine).
This chlorine gas is used for the manufacture of bleaching
powder.
Bleaching powder is produced by the action of chlorine on dry
slaked lime [Ca(OH)2].
Bleaching powder is represented as CaOCl2
BLEACHING POWDER

31. (i) for bleaching cotton and linen in the textile
industry, for bleaching wood pulp in paper
factories and for bleaching washed clothes in
laundry
(ii) as an oxidising agent in many chemical
industries
(iii) for disinfecting drinking water to make it
free of germs.
Use of Bleaching Powder:

32. The chemical name of the compound is sodium
hydrogencarbonate (NaHCO3).
The soda commonly used in the kitchen for
making tasty crispy pakoras is baking soda.
Sometimes it is added for faster cooking
Baking soda

33. When NaHCO3 is heated while cooking, following reaction takes place.

34. (i) For making baking powder, mixture of sodium hydrogen carbonate (baking
soda) and mild edible acid such as tartaric acid are used.
Carbon dioxide produced during the reaction causes bread or cake to rise
making them soft and spongy.
(ii) It is used in antacids, being basic in nature it can neutralize excess of acid in
the stomach and provides relief.
(iii) It is also used in soda-acid fire extinguishers.
Uses of Baking soda:

35. Washing soda
Recrystallisation of sodium carbonate gives
washing soda. It is also a basic salt.

36. Uses Of Washing Soda:
(i) Sodium carbonate (washing soda) is used in glass, soap and
paper industries.
(ii) It is used in the manufacture of sodium compounds such as
borax.
(iii) Sodium carbonate can be used as a cleaning agent for
domestic purposes.
(iv) It is used for removing permanent hardness of water.

37. Water of crystallisation is the fixed number of water
molecules present in one formula unit of a salt.
Water of Crystallisation

38. On heating gypsum at 373 K, it loses water molecules and becomes
calcium sulphate hemihydrate ( CaSO4 . 1/2 H2O ).
This is called Plaster of Paris, the substance which doctors use as plaster
for supporting fractured bones in the right position. Plaster of Paris is a
white powder and on mixing with water, it changes to gypsum once again
giving a hard solid mass.
Plaster of Paris