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10 Science notes Chapter 2 Acids Bases and Salts

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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 ${H_2}S{O_4}$	Potassium hydroxide KOH
Nitric acid $HN{O_3}$	Calcium hydroxide ${C_a}{(OH)_2}$
Acetic acid $C{H_3}\;COOH$	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 hydroniumions) and a large amount of water.
Concentrated Acid : A concentrated acid contains a large amount of acid (higher concentration of hydroniumions)and a small amount of water.
Chemical Properties of Acids and Bases

Reaction with metal

$Acid\; + \;Metal\; \to \;Salt\; + \;Hydrogen$

$2HCl + Zn\xrightarrow{{}}\;ZnC{l_2}\; + \;{H_2}$

$2HN{O_3} + \;Zn\xrightarrow{{\,\,\,\,}}Zn{(N{O_3})_2} + {H_2}$

${H_2}S{O_4} + Zn\xrightarrow{{}}ZnS{O_4} + {H_2}$

$2C{H_3}COOH + Zn\xrightarrow{{}}\\{(C{H_3}COO)_2}Zn + {H_2}$

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 $\xrightarrow{{}}$ Salt + Hydrogen

$NaOH + Zn\;\xrightarrow{{}}\;\mathop {N{a_2}Zn{O_2} + {H_2}}\limits_{Sodium\;Zincate}$

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

Actions of Acids with metal Carbonates and metal bicarbonates

$MetalCarbonate + Acid\xrightarrow{{}}\ Salt + Carbondioxide + Water$

$N{a_2}C{O_{3(aq)}}\xrightarrow{{}} \ 2NaC{l_{(aq)}} + C{O_{2(g)}} + {H_2}{O_{(l)}}$

$Metal bicarnonate + Acid\xrightarrow{{}}\ Salt + Carbondioxide + Water$

$NaHC{O_3} + HCl\xrightarrow{{}}\ NaCl + C{O_2} + {H_2}O$

Lime water Test : On passing the evolved $C{O_2}$ gas through lime water, we find that lime water turns milky.

$\mathop {Ca{{\left( {OH} \right)}_{2(aq)}}}\limits_{Lime\,\,water} + C{O_{2(g)}} \to \ \mathop {CaC{O_{3(s)}} + {H_2}{O_{(l)}}}\limits_{White\,\,precipitate}$

$C{O_2}$ the following reaction takes place

$CaC{O_{3(s)}} + {H_2}{O_{(l)}} + C{O_{2(g)}}\xrightarrow{{}}\\\mathop {Ca{{(HC{O_3})}_2}aq}\limits_{{\text{(soluble}}\,\;{\text{in water)}}}$

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

$Base\; + \;Acid\;\xrightarrow{{}}\;Salt\; + \;Water$

e.g. $NaO{H_{(aq)}} +HC{l_{(aq)}}\xrightarrow{{}}\ NaC{l_{(aq)}} + {H_2}O(l)$

Reactions of metal oxides with acids

$Metal Oxide + Acid\xrightarrow{{}}Salt + Water$

$\mathop {CuO}\limits_{Copperoxide} + \mathop {HCl}\limits_{Hydrochloric\,\,acid} \to \\ \mathop {CuC{l_2}}\limits_{Copper\,\,Chloride} + \mathop {{H_2}O}\limits_{Water}$

Note : Appearance of blue green colour of the solution because of formation of $CuC{l_2}$ .

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 $\xrightarrow{{}}$ Salt + Water

$C{O_2} + Ca{(OH)_2}\xrightarrow{{}}CaC{O_3} + {H_2}O$

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 produce ${H^ + }$ ions in the presence of water

$HCl\; + \;\;{H_2}O\;\xrightarrow{\;}\;{H_3}{O^ + } + C{l^ - }$

${H_3}{O^ + }\;\;$ : Hydroniumion.

${H^ + }$ ion cannot exist alone. It exists as ${H^ + }(aq)\;or\;({H_3}{O^ + })$ hydroniumion.

i.e. Base provide $O{H^ - }_{(aq)}$ ions in the presence of water

$NaO{H_{(s)}}\xrightarrow{{{H_2}O}}N{a^ + }_{(aq)} + O{H^ - }_{(aq)}$

$KO{H_{(s)}}\xrightarrow{{{H_2}O}}{K^ + }_{(aq)} + O{H^ - }_{(aq)}$

$Mg{(OH)_{{2_{(s)}}}}\xrightarrow{{{H_2}O}}M{g^{2+}}(aq) + 2O{H^-}(aq)$

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 ${H^ + }ion$ and $O{H^ - }ion$ reduces.

Strength of an Acid or Base

Strength of acids and bases depends on the no. of ${H^ + }ion$ and $O{H^ - }ion$ produced 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. $O{H^ - }ion$ 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	${K_2}S{O_4}$	KOH	${H_2}S{O_4}$
2.	Sodium Sulphate	$N{a_2}S{O_4}$	NaOH	${H_2}S{O_4}$
3.	Sodium Chloride	NaCl	NaOH	HCl
4.	Ammonium Chloride	$N{H_4}Cl$	$N{H_4}OH$	HCl

Note : NaCl and $N{a_2}S{O_4}$ belong 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, CaSO $_{_4}$

Acidic Salts : Strong Acid + weak base

pH value is less than 7

eq. $N{H_4}Cl,N{H_4}N{O_3}$

Basic Salts : Strong base + weak acid

pH value is more than 7

$e.g.\;\;CaC{O_3},C{H_3}COONa$

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.

$2{N_a}C{l_{(aq)}} + 2{H_2}O(l)\xrightarrow{{}}\\2NaO{H_{(aq)}} + \,\,C{l_{2(g)}} + {H_{2(g)}}$

Calcium oxy chloride — CaOCl $_2$
The chlorine gas released in brine formation is used to prepare bleach.

$\mathop {Ca{{(OH)}_2}}\limits_{Calcium\,\,Hydroxide} + \mathop {C{l_2}}\limits_{Chlorine} \to \ \mathop {CaOC{l_2}}\limits_{bleaching\,\,powder} + \mathop {{H_2}O}\limits_{Water}$

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 – NaHCO $_3$

Common name – Baking Soda. It is mild corrosive base

Preparation :

Used in baking/cooking

Heating $NaHC{O_3}\; + \;{H_2}O\; + \;C{O_2}$

$NaHC{O_3}\xrightarrow{{heat}}\ N{a_2}C{O_3} + {H_2}O + C{O_2}$

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.

$N{a_2}C{O_3} +10{H_2}O\xrightarrow{{Heat}} \ N{a_2}C{O_{{3^.}}}10{H_2}O$

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:

$CuS{O_{{4^.}}}5{H_2}O$
$CaS{O_{{4^.}}}2{H_2}O$
$CaS{O_{{4^.}}}\frac{1}{2}{H_2}O$

Plaster of Paris

$CaS{O_{{4^.}}}2{H_2}O\xrightarrow{{373K}}CaS{O_4}\frac{1}{2}{H_2}Oa$

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

$\begin{gathered} CaS{O_{{4^.}}}^{\frac{1}{2}}{H_2}O\; + {1^{\frac{1}{2}}}{H_2}O\xrightarrow{{}}\ CaS{O_4}.2{H_2}O \hfill \\ \;\;\;\;\;\;\;\;\;\;\;POP\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;\;GYPSUM \hfill \\ \end{gathered}$

: 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.

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