Explain why sodium hydroxide solution cannot be kept in aluminium containers
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) Sodium hydroxide solution cannot be kept in aluminium containers.
(ii) Silver metal does not combine easily with oxygen but silver jewellery tarnishes after some time.
(iii) Sodium is obtained by the electrolysis of its molten chloride and not from its aqueous solution.
(iv) Aluminium reacts with dilute hydrochloric acid slowly in the beginning.(i) Sodium hydroxide reacts with $Al$ corroding the metal and produces highly flammable hydrogen gas. Hence, it cannot be kept in $Al$ containers.
(ii) Silver is a highly unreactive metal so, it does not react with the oxygen of air easily. But silver jewellery tarnishes after some time (turns black) due to the formation of a thin sulphide layer on their surface by the action of hydrogen sulphide ($H2S$) gas present in air.
(iii) We cannot use an aqueous solution of sodium chloride to obtain sodium metal because if we electrolyse an aqueous solution of $NaCl$, then as soon as sodium metal is produced at cathode, it will react with water present in the aqueous solution to form sodium hydroxide. So, the electrolysis of aqueous solution of $NaCl$ will produce $NaOH$ instead of Na metal.
(iv) Al metal reacts with dilute $HCl$ slowly in the beginning due to the presence of a tough protective layer of aluminium oxide on its surface.
(ii) Silver metal does not combine easily with oxygen but silver jewellery tarnishes after some time.
(iii) Sodium is obtained by the electrolysis of its molten chloride and not from its aqueous solution.
(iv) Aluminium reacts with dilute hydrochloric acid slowly in the beginning.(i) Sodium hydroxide reacts with $Al$ corroding the metal and produces highly flammable hydrogen gas. Hence, it cannot be kept in $Al$ containers.
(ii) Silver is a highly unreactive metal so, it does not react with the oxygen of air easily. But silver jewellery tarnishes after some time (turns black) due to the formation of a thin sulphide layer on their surface by the action of hydrogen sulphide ($H2S$) gas present in air.
(iii) We cannot use an aqueous solution of sodium chloride to obtain sodium metal because if we electrolyse an aqueous solution of $NaCl$, then as soon as sodium metal is produced at cathode, it will react with water present in the aqueous solution to form sodium hydroxide. So, the electrolysis of aqueous solution of $NaCl$ will produce $NaOH$ instead of Na metal.
(iv) Al metal reacts with dilute $HCl$ slowly in the beginning due to the presence of a tough protective layer of aluminium oxide on its surface.
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Sodium hydroxide reacts with aluminum, corroding the metal and producing highly flammable hydrogen gas. That is why sodium hydroxide solution cannot be kept in aluminium containers
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