State as to why
(a) a solution of `Na_(2)CO_(3)` is alkaline ?
(b) alkali metals are prepared by electrolysis of their fused chlorides?
(c) sodium is found to be more useful than potassium ?

Sodium is found more useful than potassium ? Explain.

An aqueous solution of Na_2CO_3 is alkaline ? Explain.

Why can we not use an aqueous solution of sodium chloride to isolate sodium metal by electrolysis ?

Why is only molten salt used for the electrolysis of a very active metal like sodium or potassium ?

Alkali &alkaline earth metals have low ionisation enthalpies and hence exhibit characteristic flame colouration. They have high negative electrode potentials & hence are strong reducing agents. It dissolve in liquid ammonia to give a solution which conducts electricity and act as strong reducing agent. being stronger reducing agent than hydrogen, they are usually prepared by the electrolysis of their fused chlorides. Their oxides are basic and the basic strength increases down the group. The solubility of carbonates and sulphates of alkali and alkaline earth metals show opposite trends. only the carbonates of Li and alkaline earth metals decompose on heating. The bicarbonates of both alkali & alkaline earth metals on heating give carbonates. Which of the following process is used in the extractive metallurgy of sodium?

Assertion (A): Aqueous solution of Na_(2)CO_(3) is alkaline in nature. Reason (R ): when dissolved in water, Na_(2)CO_(3) undergoes anionic hydrolysis.

Assertion (A): Aqueous solution of Na_(2)CO_(3) is alkaline in nature. Reason (R ): when dissolved in water, Na_(2)CO_(3) undergoes anionic hydrolysis.

Why potassium carbonate (K_(2)CO_(3)) cannot be prepared by Solvay-ammonia process ?

Why potassium carbonate (K_(2)CO_(3)) cannot be prepared by Solvay-ammonia process ?

Value of standard electrode potential for the oxidation of Cl^(-) ions is more positive than that of water, even then in the electrolysis of aqueous sodium chloride, why is Cl^(-) oxidsied at anode instead of water?