, Acids, Bases, and Salts
ACIDS BASES
Sour in taste. Bitter in taste and soapy in touch .
Release H+ ions in water. Release OH- ions in water.
Change the color of blue litmus to red. Change the color of red litmus to blue.
Indicators are substances that indicate the acidic or basic nature. They can either be:
Natural Olfactory Synthetic
obtained via natural sources, their odour/smell changes in they are synthesized in labs.
eg- turmeric, litmus, red acidic and basic media. Eg.- Eg.- Methyl orange,
cabbage, flower petals of Vanilla, clove, onion, etc. Phenolphthalein, etc.
Hydrangea, Petunia, and
Geraniumetc.
Indicator Acid Base
Red Litmus No change Blue
Blue Litmus
Turmeric
Red
No change
.0
No Change
Red- brown
Red cabbage
Onion
Red-Pink
No Change
2
Green- yellow
No smell
Vanilla
Phenolpthalein
ng No Change
Colorless
No smell
Pink
Methly orange
ni Red Yellow
Litmus solution is a purple dye (in neutral state) derived from lichens and is used as an acid-base indicator.
ar CHEMICAL PROPERTIES OF ACIDS AND BASES
Le 1. Reaction Of Acids With Metals
Upon reaction with metals, the hydrogen atoms of acids get displaced by the metal in the form of H₂ gas and for a
Examples:
ive
compound called salt.
→
Acid + Metal →Salt + Hydrogen gas
t
2NaOH(aq) + Zn(s) Na₂ZnO₂(s) + H₂ (g)
Zn(s) + 2HCl(aq) → ZnCl₂ (aq) + H₂ (g)
a
Mg(s) + H₂SO₄(aq)
e
→ MgSO₄(aq) + H₂ (g)
r
2. Reaction Of Acids With Metal Carbonates and Metal Hydrogencarbonates
C
On reacting with metal carbonates and metal hydrogencarbonates, acids produce salt, carbon dioxide, and water.
Metal carbonate/Metal hydrogencarbonate + Acid →
Salt + CO₂ + H₂O
Examples:
2NaHCO₃(aq) + H₂SO₄(aq) →
NaCl(aq) + CO₂ + Water
2Na₂CO₃(aq) + 2HCl(aq) →
2NaCl(aq) + CO₂ + Water SALT
3. Reaction Between Acids And Bases (Neutralisation reaction)
An acid nullifies the effect of base and vice-versa. Hence, it is referred to as neutralisation reaction.
They react to give salt and water, i.e., Acid + Base →Salt + Water.
Example:
NaOH (aq) + HCl (aq) →NaCl (aq) + H₂O (l)
HCl (aq) + Ca(OH)₂ (aq) →
CaCl₂ (aq) + H₂O (l)
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ACIDS BASES
Sour in taste. Bitter in taste and soapy in touch .
Release H+ ions in water. Release OH- ions in water.
Change the color of blue litmus to red. Change the color of red litmus to blue.
Indicators are substances that indicate the acidic or basic nature. They can either be:
Natural Olfactory Synthetic
obtained via natural sources, their odour/smell changes in they are synthesized in labs.
eg- turmeric, litmus, red acidic and basic media. Eg.- Eg.- Methyl orange,
cabbage, flower petals of Vanilla, clove, onion, etc. Phenolphthalein, etc.
Hydrangea, Petunia, and
Geraniumetc.
Indicator Acid Base
Red Litmus No change Blue
Blue Litmus
Turmeric
Red
No change
.0
No Change
Red- brown
Red cabbage
Onion
Red-Pink
No Change
2
Green- yellow
No smell
Vanilla
Phenolpthalein
ng No Change
Colorless
No smell
Pink
Methly orange
ni Red Yellow
Litmus solution is a purple dye (in neutral state) derived from lichens and is used as an acid-base indicator.
ar CHEMICAL PROPERTIES OF ACIDS AND BASES
Le 1. Reaction Of Acids With Metals
Upon reaction with metals, the hydrogen atoms of acids get displaced by the metal in the form of H₂ gas and for a
Examples:
ive
compound called salt.
→
Acid + Metal →Salt + Hydrogen gas
t
2NaOH(aq) + Zn(s) Na₂ZnO₂(s) + H₂ (g)
Zn(s) + 2HCl(aq) → ZnCl₂ (aq) + H₂ (g)
a
Mg(s) + H₂SO₄(aq)
e
→ MgSO₄(aq) + H₂ (g)
r
2. Reaction Of Acids With Metal Carbonates and Metal Hydrogencarbonates
C
On reacting with metal carbonates and metal hydrogencarbonates, acids produce salt, carbon dioxide, and water.
Metal carbonate/Metal hydrogencarbonate + Acid →
Salt + CO₂ + H₂O
Examples:
2NaHCO₃(aq) + H₂SO₄(aq) →
NaCl(aq) + CO₂ + Water
2Na₂CO₃(aq) + 2HCl(aq) →
2NaCl(aq) + CO₂ + Water SALT
3. Reaction Between Acids And Bases (Neutralisation reaction)
An acid nullifies the effect of base and vice-versa. Hence, it is referred to as neutralisation reaction.
They react to give salt and water, i.e., Acid + Base →Salt + Water.
Example:
NaOH (aq) + HCl (aq) →NaCl (aq) + H₂O (l)
HCl (aq) + Ca(OH)₂ (aq) →
CaCl₂ (aq) + H₂O (l)
10
