Chapter 2 acides bases and salt

Acids Bases and Salt notes

Properties of Acids:

– Produce hydrogen ions [H⁺] in H₂O.
– Sour taste.
– Turn blue litmus red.
– Act as electrolytes in Solution.
– Neutralize solutions carrying hydroxide ions.
– React with several metals releasing Hydrogen gas.
– React with carbonates releasing CO₂ (g)
– Destroy body tissues.
– corrode metal surface quickly.

On the basis of origin, acids are classified as :

a. Organic acids: Acids derived from living organisms like plants and animals . For example: citric acid is present in fruits, acetic acid present in vinegar, oxalic acid present in tomato, tartaric acid present in tamarind, lactic acid present in sour milk and curd.


b. Mineral acids: They are also called inorganic acids. They are dangerous Example sulphuric acid (H₂SO₄), hydrochloric acid (HCl) etc.

➣  On the basis of their strength, acids are classified as :

a. Strong acids: Completely dissociate into its ions in aqueous solutions.
Example: Nitric acid (HNO₃), sulphuric acid (H₂SO₄), hydrochloric acid (HCl).

b. Weak acids: Weak acids are those acids which do not completely dissociate into
its ions in aqueous solutions. For example: carbonic acid (H₂CO), acetic acid (CH₃COOH).

➣    On the basis of their concentration, acids are classified as :

a. Dilute acids: Have a low concentration of acids in aqueous solutions.
b. Concentrated acids: Have a high concentration of acids in aqueous solutions.

➣     On the basis of number of hydrogen ion, acids can be classified as :

Monoprotic acid – Such type of acid produces one mole of H⁺ ions per mole of acid, e.g., HCl , HNO₃

Diprotic acid – They can produce two moles of H⁺ ions per mole of acid, e.g., H₂SO₄.

Triprotic acid – They produce three moles of H⁺ ions per mole of acid, e.g., H₃PO₄.

Polyprotic – They can produce more than three H+ ions per mole of acid.

➣    Properties of Base:

– Produce hydroxide ions [OH –] in H₂O.
– Water soluble bases are called alkalies.
– Bitter Taste
– Turn Red Litmus blue.
– Act as electrolytes in Solution.
– Neutralize solutions containing H⁺ ions.
– Have a slippery, ‘soapy’ feel.
– Dissolve fatty material.

➣    On the basis of their strength, bases are classified as:

a. Strong bases: Strong bases are those bases which completely dissociate into its ions in aqueous solutions. Example: sodium hydroxide (NaOH), potassium hydroxide (KOH).

b. Weak bases: Weak bases are those bases which do not completely dissociate into its ions in aqueous solutions. For example: ammonium hydroxide (NH₄OH).

➣    On the basis of their concentration, bases are classified as:

a. Dilute bases: Have a low concentration of alkali in aqueous solutions.
b. Concentrated bases: Have a high concentration of alkali in aqueous solutions.

➣    Strength Of Acid Or Base Solutions:

A scale for measuring hydrogen ion concentration in a solution, called pH scale has been developed. The p in pH stands for ‘potenz’ in German, meaning power.
p= potential or Power         H = Hydrogen

pH =7	Neutral Solution	H3O+ = OH –
pH>7	Basic Solution	H3O+ < OH –
pH<7	Acidic Solution	H3O+ > OH –

Range of pH is from 1 to 14

➣    pH Sensitivity of Plants & Animals:

• Human body works in a narrow range of pH 7 to 7.8. Acidity can be lethal for plants and animals.
• pH of Digestive System: Stomach secretes HCl to kill bacteria in the food. The inner lining of stomach protects vital cells from this acidic pH.
• pH and tooth decay: Lower pH because of sour food and sweet food can cause tooth decay. The pH of mouth should always be more than 5.5.
• pH as self defense mechanism in plants & animals: Certain animals like bee and plants like nettle secrete highly acidic substance for self defense.

➣   Properties of salts:

• Salts form by the combination of acid and base through neutralization reaction.
• The acidic and basic nature of salts depends on the acid and base combined in neutralization reaction.

• The most common salt is sodium chloride or table salt which forms by the combination of sodium hydroxide (base) and hydrochloric acid.
• Other examples include Epsom salts (MgSO₄) used in bath salts, ammonium nitrate (NH₄NO₃ ) used as fertilizer, and baking soda (NaHCO₃) used in cooking.
• The pH of salts solution depends on the strength of acids and base combined in neutralization reaction.
• Indicators – Indicators are substances which indicate the acidic or basic nature of the solution by their colour change.

The colour of some acid – base indicators in acidic and basic medium are given below :

S. No.	Indicators	Colour in	Colour in
		acidic medium	basic medium
1	Litmus solution	Red	Blue
2	Methyl Orange	Pink	Orange
3	Phenolphthalein	Colourless	Pink
4	Methyl red	Yellow	Red

Chemical properties of acids:

i) Acids react with active metals to give hydrogen gas.
Zn + H₂SO₃ →ZnSO₄ + H₂

ii) Acids react with metal carbonate and metal hydrogen carbonate to give carbon dioxide.
NaHCO₃ +HCl → NaCl + H₂O + CO₂

iii) Acids react with bases to give salt and water. This reaction is called as neutralization reaction.NaOH + HCl → NaCl +H₂O

iv) Acids react with metals oxides to give salt and water.
CuO + H2SO4 → CuSO₄ + H₂O

Addition of Acids or Bases to Water

The process of dissolving an acid, specially nitric acid or sulfuric acid or a base in water is a highly exothermic one. As a rule: Always add acid to water and never the other way! The acid must be added slowly to water with constant stirring. If one mixes the other way by adding water to a concentrated acid, the heat generated causes the mixture to splash out and cause burns.

➣   Chemical properties of Bases:

i) Reaction with Metals - Certain reactive metals such as Zinc, Aluminium, and Tin react with alkali solutions on heating and hydrogen gas is evolved. 2NaOH + Zn →  Na₂ZnO₂ +H₂

ii) Reaction with acids -Bases react with acids to form salt and water. KOH +HCl → KCl +H₂O

iii) Reaction with Non -metallic oxides – These oxides are generally acidic in nature. They react with bases to form salt and water. 2NaOH + CO₂ → Na₂CO₃ + H₂O

 ➣   Some Important Chemical Compounds:•   

• Common Salt (NaCl)

Sodium chloride is known as common salt. Its main source is sea water. It is also exists in the form of rocks and is called rock salt.
Common salt is an important component of our food. It is also used for preparing sodium hydroxide, baking soda, washing soda etc.

•  Sodium hydroxide (NaOH)

Prepared by Chlor Alkali process :Electricity is passed through an aqueous solution of Sodium chloride (called brine). Sodium chloride decomposes to form sodium hydroxide. Chlorine gas is formed at the anode, and hydrogen gas at the cathode. Sodium hydroxide solution is formed near the  cathode. 2NaCl(aq) + 2 H₂O (l) → 2NaOH(aq) + Cl₂(g) + H₂(g)

• Bleaching powder:

Bleaching powder is represented as CaOCl₂, though the actual composition is quite complex.
Bleaching powder is produced by the action of chlorine on  dry slaked lime. Ca(OH)₂ + Cl₂ → CaOCl₂+ H₂O

• Baking soda:
Sodium hydrogen carbonate (NaHCO₃) Preparation: NaCl + H₂O + CO₂+ NH3 → NH₄Cl + NaHCO₃

•Washing soda: Sodium carbonate N₂CO₃.10H₂ In the first step, sodium carbonate is obtained by heating baking  soda. 2 NaHCO₃(heat) →Na₂CO₃ + H₂O + CO₂

Then washing sod a is produced by recrystallisation of sodium  carbonate Na₂CO₃ + 10H₂O →  Na₂CO₃ .10H₂O

•  Plaster of Paris:
Calcium sulphate hemihydrate CaSO₄. ½ H₂O Prepared by heating Gypsum at 373K. CaSO₄. 2H₂O(Heat at 373K) → CaSO₄. ½ H₂O + 1½ H₂O

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