Preparation and properties of sodium carbonate, sodium hydroxide and sodium hydrogen carbonate

Preparation of sodium hydroxide :
Nelson's cell
Castner–Kellner process

Nelson cell method :
It is a 'U' shaped perforated steel vessel
Cathode : steel vessel
Anode : graphite rod
At anode : 2Cl⁻ → Cl₂ + 2e⁻
At cathode : 2Na⁺ + 2e⁻ + 2H₂O → 2NaOH + H₂ ↑

Castner - Kellner process :

Outer compartment :
Cathode - 'Hg'
Anode - Graphite
electrolyte - Brine solution
At anode : 2Cl⁻ → Cl₂ + 2e⁻
At cathode : 2Na⁺ + 2e⁻ + Hg → Na₂Hg
Middle compartment :
Cathode - Fe rod
Anode - Hg
electrolyte - dil NaOH
At anode : Na₂Hg → 2Na⁺ + 2e⁻ + Hg
At cathode : 2Na⁺ + 2e⁻ + 2H₂O → 2NaOH

Chemical properties of NaOH :

Non metals : Cl₂, Br₂, I₂ reacts with dil and cold, conc and hot NaOH. It gives NaOCl and NaClO₃ (sodium oxychloride, sodium chlorate)

Chlorine, bromine, iodine, phosphorus gives disproportionation reaction.
With metals :
Aluminium reacts with cold and dil. NaOH gives NaAlO₂
Hot and conc NaOH gives H₂ + Na₃AlO₃

Preparation of sodium peroxide (Na₂O₂)
Preparation : Na_{2}O \xrightarrow[]{\Delta}Na_{2}O_{2}

Na_{2}O_{2} + CO \rightarrow Na_{2}O_{3}
Na_{2}O_{2} + CO_{2} \rightarrow Na_{2}CO_{3} + \frac{1}{2}O_{2}

Preparation of Na₂CO₃ (Sodium carbonate)
Washing soda - Na₂CO₃.10H₂O
soda ash - Na₂CO₃
It is prepared by 1) Leblanc process 2) Solvay process

Leblanc process : Raw materials : NaCl, Coke, limestone
2NaCl + H_{2}SO_{4}\rightarrow Na_{2}SO_{4} + 2HCl
Na_{2}SO_{4} + 4C \rightarrow Na_{2}S + 4CO

Solvay process :
NH_{3} + H_{2}O + O_{2} \rightarrow NH_{4}HCO_{3}
NH_{4}HCO_{3} + NaCl \rightarrow NaHCO_{3}\downarrow + NH_{4}Cl
2NaHCO_{3} \xrightarrow[]{\Delta} Na_{2}CO_{3} + H_{2}O + CO_{2}
2NH_{3}+ H_{2}O + CO_{2} \rightarrow (NH_{4})_{2}CO_{3}
(NH_{4})_{2}CO_{3} + MgCl_{2} \rightarrow MgCO_{3}\downarrow

Physical properties :
Efflorescent substance i.e, it looses its crystalline water molecules when it is kept in open air.
Chemical properties :

Preparation of sodium bicarbonate (NaHCO₃) :
Na_{2}CO_{3} + H_{2}O + CO_{2} \rightarrow 2NaHCO_{3}
Chemical properties :
2NaHCO_{3} \xrightarrow[]{\Delta} Na_{2}CO_{3} + H_{2}O + CO_{2}
CO_3^{-2} \xrightarrow[]{H_{2}O} 2OH^{-}
HCO_3^{-} \xrightarrow[]{H_{2}O} OH^{-}

It is a mild antiseptic for skin infections and fire extinguishers.

General properties of IA group - element :
Atomic size : (↑)
down the group increases
Density : (↑)
But Na > K
Melting and boiling point : down the group decreases.
Conductivity : In free state
Li⁺ > Na⁺ > K⁺ > Rb⁺ > Cs⁺
Aqueous state : Li⁺ < Na⁺ < K⁺ < Rb⁺ < Cs⁺
Lithium has more hydrated energy.
Ionisation enthalpy down the group decreases
Hydration enthalpy down the group increases
Metallic radius down the group increases
Ionic radius down the group increases.

Reducing nature :
Due to small size lithium has more hydration enthalpy and also high negative electrode potential value.
Lithium good reducing agent → More hydration energy.

flame colourisation :
Li → Crimson red
Na → Golden yellow
K → Pale violet
Rb → Red, violet
Cs → Violet

Reactivity towards air :
M + O_{2} \rightarrow M_{2}O(oxide) \xrightarrow[]{H_{2}O}MOH \xrightarrow[]{CO_{2}}M_{2}CO_{3}
4Na + O_{2} \rightarrow 2Na_{2}O
2Na + O_{2} \rightarrow Na_{2}O_{2}(Peroxide)
4Li + O_{2} \rightarrow 2Li_{2}O(oxide)
M + O_{2}(Excess) \rightarrow MO_{2}(superoxide), M = K, Rb, Cs
2M + 2H_{2}O\rightarrow 2M^{+} + 2OH^{-}+ H_{2}
2M + H_{2} \xrightarrow[]{673 K} 2M^{+} + H^{-}

Reactivity with NH₃
Aqueous NH₃ :
M + NH_{3} \rightarrow Ammoniated \ ions+ Ammoniated \ electrons

Conductivity ⇒ Due to Ammoniated ions and electrons.
Alkali metals dissolve in NH₃ giving deep blue colour solution.
On warming blue colour changes to bronze colour and becomes diamagnetic.
Li₂CO₃ on heating gives Li₂O and CO₂
Li_{2}CO_{3} \xrightarrow[]{\Delta} Li_{2}O + CO_{2}
Remaining other all carbonates not decomposed by heating.