BEST AND PERFECT PPT ON ACIDS, BASES AND SALTS CLASS 10 SCIENCE ( not overconfident... but there are no unwanted slides).

1. SCIENCE HOLIDAY HOMEWORK

2. INTRODUCTION
 Acids are sour in taste and change the colour of blue
litmus to red.
 Bases are bitter in taste and change colour of red litmus to
blue.
 Litmus is a natural indicator, turmeric is another such
indicator.

3. COMMON ACIDS AND BASES
 HYDROCHLORIC ACID ( STOMACH ACID ) –
“HCL”
 ACETIC ACID ( VINEGAR ) – “HC2H3O2”
 CARBONIC ACID ( SODA WATER ) – H2CO3
 AMMONIA WATER ( CLEANING AGENT ) –
NH4OH
 ALUMINIUM HYDROXIDE ( ROLAIDS ) –
AL(OH)3

4. REACTION OF ACIDS WITH
METALS
 ACID + METAL → SALT + HYDROGEN
 EX:-
HYDROCHLORIC ACID + ZINC → ZINC
CHLORIDE + HYDROGEN
Not applicable for non- reactive metals like copper, silver,
gold.....

5. REACTION OF ACIDS WITH
METAL CARBONATES
 ACID + METAL CARBONATE → SALT + CARBON
DIOXIDE + WATER
 EX:-
HYDROCHLORIC ACID + SODIUM
CARBONATE → SODIUN CHLORIDE + CARBON
DIOXIDE + WATER

6. REACTION OF ALKALI WITH
AMMONIUM SALTS
 ALKALI + AMMONIUM SALT → SALT + AMMONIA
+ WATER
 EX:-
SODIUM HYDROXIDE + AMMONIUM
CHLORIDE → SODIUM CHLORIDE + AMMONIA +
WATER

7. NEUTRALIZATION
 ACID + BASE → SALT + WATER
 EX:-
HYDROCHLORIC ACID + SODIUM
HYDROXIDE → SODIUM CHLORIDE + WATER

8. SALTS
 A salt is formed when a hydrogen of an acid is totally or
partially replaced by a metal.
 Salts of a strong acid and a strong base are neutral with pH
value of 7. on the other hand, salts of a strong acid and a
weak base are acidic with pH value of less than 7 and
those of a strong base and weak acid are basic in nature,
with pH value more than 7.

9. pH SCALE
 For measuring the hydrogen
concentration in a solution, called pH
scale is developed. Where “p” stands
for potenz which means power in
German.
 On the pH scale we can generally
measure from 0( very acidic ) to 10 (
very alkaline ).
 The pH of a neutral solution is 7. the
pH below 7 turns that the solution is
acidic and if the pH of a solution is
above 7 it is alkali.

10. IMPORTANCE OF Ph EVERYDAY
 ARE PLANTS AND ANIMALS Ph SENSITIVE?
ANS. Our body works within the pH range of 7.0 to 7.8.
living organisms can survive only in a narrow range of pH
change. If rain water of less than 5.8 pH i.e., acid rain falls
into rivers the survival of aquatic life becomes difficult.
Thus, plants and animals are pH sensitive.

11. • pH IN OUR DIGESTIVE SYSTEM
ANS. Components in saliva help keep the pH in
your mouth between 6.5 and 7 so that the enzyme
salivary amylase can start to break down
carbohydrates. The enzymes that help digest food
in the stomach, such as pepsin, work best at a pH
around 2, while those that function in the
intestines, including peptidases and maltase,
work best at a pH around 7.5.
Antacids increase the pH in the stomach, which
might make the enzymes in the stomach less
effective. The low pH of the juices in the stomach
can cause ulcers if they eat through the walls of
the small intestine or stomach. This low pH also
kills many microorganisms in the food you eat,
helping prevent illnesses.

12.  pH changes as the cause of tooth decay.
ANS. 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 rate
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.

13. CHEMICALS FROM COMMON
SALTS
 Seawater contains many salts dissolved in it. Sodium
chloride is separated from these salts. Deposits of solid
salts are also found in several parts of the world. There
large crystals are often brown due to impurities. This is
called rock salt. Beds of rock salts were formed when seas
of bygone ages dried up. Rock salts are mined a coal.
 Some examples of salts are:

14.  COMMOM SALT
The common salts 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.

15.  SODIUM HYDROXIDE
When electricity is passed through an aqueous solution of
sodium hydroxide ( called brine ), it decomposes to form
sodium hydroxide. The process is called the chlor-alkali
process because of the products formed- clor for chlorine
and alkali for sodium hydroxide.
2NaCl + 2H2O → NaOH + Cl2 + H2

16.  BLEACHING POWDER
Chlorine is produced during the electrolysis of aqueous sodium
solution ( 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
representated as CaOCl2, through the actual composition is
quite complex.
Ca(OH)2 + Cl2 → CaOCl2 + H2O
 BLEACHING POWDER IS USED IN:
1] for bleaching cotton and linen in the textile industry, for
bleaching wood pulp in paper factories and for bleaching washed
clothes in laundry.
2] as an oxidising agent in many chemical industries
3] for disinfecting drinking water to make it free of germs.

17.  BAKING SODA
The soda is commonly used in kitchen for making tasty
crispy pakoras is baking soda. Sometimes it is added for
faster cooking. The chemical name of the compound is
sodium hydrogencarbonate ( NaHCO3 ). It is produced
using sodium chloride as one of its raw material.
NaCl + H2O + CO2 + NH3 → NH4Cl + NaHCO3

18.  WASHING SODA
Another chemical that can be obtained from sodium
chloride is NaCo3.10H2O ( Washing Soda ). Sodium
carbonate can be obtained by heating baking soda;
recrystallisation of Sodium Carbonate gives washing soda.
It is also a basic salt.
Na2CO3 + 10H2O → Na2CO3.10H2O.

19. ARE THE CRYSTALS OF SALTS
REALLY DRY?
 Copper sulphate crystals which seem to be dry contain
water of crystallisation. When we heat the crystals, this
water is removed and the salt turns white.
 If you moisten the crystals again with water, the blue
colour reappears.
 Water of Crystallisation has a fixed number of crystals
water molecules present in one formula unit of a salt. Five
water molecules are present in one formula unit of copper
sulphate.
CaSO4.5H2O

20. PLASTER OF PARIS ( P.O.P )
 On heating gypsum at 373K, it loses water molecules and
becomes calcium sulphate hemihydrate [ CaSo4.1/2H2o
]. 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 giving a hard
solid mass.

21. THANK YOU