The process used to obtain sodium hydroxide from brine is called the chlor-alkali process. It involves the electrolysis of brine (concentrated aqueous solution of sodium chloride) using a diaphragm cell or a mercury cell.
In the chlor-alkali process, brine is electrolyzed using inert electrodes (e.g., graphite for anode and steel for cathode). During the electrolysis:
At the cathode (reduction): Sodium ions (\(\text{Na}^+\)) are reduced to sodium metal (\(\text{Na}\)), which immediately reacts with water to form sodium hydroxide (\(\text{NaOH}\)) and hydrogen gas (\(\text{H}_2\)).
\[ 2\text{Na}^+(\text{aq}) + 2e^- \rightarrow 2\text{Na}(\text{s}) \] \[ 2\text{Na}(\text{s}) + 2\text{H}_2\text{O}(\text{l}) \rightarrow 2\text{NaOH}(\text{aq}) + \text{H}_2(\text{g}) \]
At the anode (oxidation): Chloride ions (\(\text{Cl}^-\)) are oxidized to chlorine gas (\(\text{Cl}_2\)).
\[ 2\text{Cl}^-(\text{aq}) \rightarrow \text{Cl}_2(\text{g}) + 2e^- \]
The overall reaction is:
\[ 2\text{NaCl}(\text{aq}) + 2\text{H}_2\text{O}(\text{l}) \rightarrow 2\text{NaOH}(\text{aq}) + \text{H}_2(\text{g}) + \text{Cl}_2(\text{g}) \]
Gases produced:
Uses of gases:
Chlorine (\(\text{Cl}_2\)):
Hydrogen (\(\text{H}_2\)):
For a reaction, \[ {N}_2{O}_5(g) \rightarrow 2{NO}_2(g) + \frac{1}{2} {O}_2(g) \] in a constant volume container, no products were present initially. The final pressure of the system when 50% of the reaction gets completed is:
In Carius method for estimation of halogens, 180 mg of an organic compound produced 143.5 mg of AgCl. The percentage composition of chlorine in the compound is ___________%. [Given: Molar mass in g mol\(^{-1}\) of Ag = 108, Cl = 35.5]