Equal length of magnesium ribbon are taken in two test tubes $^{'} A^{'}$ and $^{'} B^{'}$ . $H_{2} S O_{4}$ is added to test tube $^{'} A^{'}$ and $H_{2} C O_{3}$ in the test tube $^{'} B^{'}$ in equal amounts.
(a) Identify the test tube showing vigorous reaction
(b) Give reason to support your answer.
(c) Name the gas liberated in both the tubes. How will your prove its liberation?
(d) Write chemical equations for both the reaction.
(e) Out of the two acids taken above:
(i) Which one will have lower pH value?
(ii) Lower $H^{+}$ concentration respectively.

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Solution

a) $H_{2} S O_{4}$ test tube i.e $A$ will show more rigorous reactions
b) Since acidic strength of $H_{2} S O_{4}$ is more than $H_{2} C O_{3}$

c) $M g + H_{2} S O_{4} \to M g S O_{4} + H_{2} (g)$

$M g + H_{2} C O_{3} \to M g C O_{3} + H_{2} (g)$

The liberated gas is $H_{2}$ and it burns with popping sound.

d) $M g + H_{2} S O_{4} \to M g S O_{4} + H_{2} (g)$

$M g + H_{2} C O_{3} \to M g C O_{3} + H_{2} (g)$

e)
i) Since $H_{2} S O_{4}$ is more acidic, it will have lower pH value.

ii) Test tube $B$ will have lower $H^{+}$ concentration as $H_{2} C O_{3}$ is a weak acid.

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