What is the role of $H_{2} {SO}_{4}$ ?

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Solution

Sulphuric acid:
It is also known as hydrogen sulfate, which is a highly corrosive, colourless, clear, odourless, and strong mineral acid with the molecular formula of $H_{2} {SO}_{4}$ .
It is very reactive that dissolves most of the metals and forms flammable hydrogen gas which may create an explosion hazard.
It is a concentrated acid that oxidizes, dehydrates, or sulfonates most of the organic compounds that often cause charring.
Role of Sulphuric acid:
Used as a catalyst:
Sulphuric acid is used as a catalyst in the esterification reaction.
Esters are formed by the reaction of ethanoic acid and ethanol in the presence of concentrated sulphuric acid.
${CH}_{3} COOH (l) + {CH}_{3} {CH}_{2} OH (l) \overset{Conc . H_{2} {SO}_{4}}{\to} {CH}_{3} {COOCH}_{2} {CH}_{3} (l) + H_{2} O (l) Ethanoic acid Ethanol Ethyl acetate Water$
Used as an oxidising agent:
The concentrated sulphuric acid acts as both an acid and an oxidizing agent.
The bromide ion oxidizes to bromine and also the reduction of sulphuric acid to sulphur dioxide with the decrease of oxidation state from $+ 6 to + 4$ .
$H_{2} {SO}_{4} (l) + 2 H^{+} (g) + 2 {Br}^{-} (l) \to {Br}_{2} (l) + {SO}_{2} (g) + 2 H_{2} O (l)$
Used as a dehydrating agent:
It has a very high affinity toward the water.
The mixture of nitric acid and sulphuric acid covalently dehydrates to form a nitrating reactant ( ${NO}_{2}^{+}$ ).
${HNO}_{3} (l) + H_{2} {SO}_{4} (l) ⇌ {HSO}_{4}^{-} (l) + {NO}_{2}^{+} (g) + H_{2} O (l)$

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27. A non-metallic element is converted into a compound X after a series of reactions. A little amount of X when tested with blue litmus turns to red. X on complete reaction with another compound Y gave the product which did not respond to litmus test. Identify the correct sequence of the reactions.

(1) $2 {SO}_{2} + O_{2} \to 2 {SO}_{3}$

(2) $H_{2} {SO}_{4} + 2 KOH \to K_{2} {SO}_{4} + 2 H_{2} O$

$(3) {SO}_{3} + H_{2} O \to H_{2} {SO}_{4}$

$(4) S + O_{2} \to {SO}_{2}$

Write the chemical names of the following compounds:

$K_{2} {SO}_{4}$

${Mg}_{3} {({PO}_{4})}_{2}$

${NH}_{4} Cl$

$ZnS$

${Na}_{3_{}} N$

$AgBr$

Complete and balance the following equations

(ⅰ ) $N_{2}$ + $H_{2}$ $\to$ $. . . . .$

(ⅱ) ${NH}_{3}$ + ${Cl}_{2} E x c e s s$ $\to$ $. . . . .$

(ⅱⅰ) $PbO$ + ${NH}_{3}$ $\to$ $. . . . . + . . . . + H_{2} O$

(ⅳ) ${NH}_{3}$ + $O_{2}$ $\overset{pt}{\to} 800 ° C$ $. . . . . + . . . . . .$

In the given reactions,

$1) I_{2} + H_{2} O_{2} + 2 {OH}^{-} \to 2 I^{-} + 2 H_{2} O + O_{2}$

$2) H_{2} O_{2} + HOCl \to {Cl}^{-} + H_{3} O^{+} + O_{2}$

Q. What is the role of CFCs ?

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What is the role of H2SO4?

What is the role of $H_{2} {SO}_{4}$ ?