Sulfuric Acid MCQ - Practice Questions & Answers

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Sulphuric Acid(H2SO4)

Preparation
Sulphuric acid is one of the most important industrial chemicals worldwide. Sulphuric acid is manufactured by the Contact Process which involves three steps:
(i) burning of sulphur or sulphide ores in air to generate SO₂.
(ii) conversion of SO₂ to SO₃ by the reaction with oxygen in the presence of a catalyst (V₂O₅).
(iii) absorption of SO₃ in H₂SO₄ to give Oleum (H₂S₂O₇).

A flow diagram for the manufacture of sulphuric acid is shown in the figure given below. The SO₂ produced is purified by removing dust and other impurities such as arsenic compounds.
The key step in the manufacture of H₂SO₄ is the catalytic oxidation of SO₂ with O₂ to give SO₃ in the presence of V₂O₅ (catalyst).

$2 \mathrm{SO}_{2}(\mathrm{g})+\mathrm{O}_{2}(\mathrm{g}) \overset{\mathrm{V}_{2} \mathrm{O}_{5}}{\longrightarrow}2 \mathrm{SO}_{3}(\mathrm{g}) \quad \Delta_{\mathrm{r}} H^{\ominus}=-196.6 \mathrm{kJmol}^{-1}$

The reaction is exothermic, reversible and the forward reaction leads to a decrease in volume. Therefore, low temperature and high pressure are the favourable conditions for maximum yield. But the temperature should not be very low otherwise rate of reaction will become slow. In practice, the plant is operated at a pressure of 2 bar and a temperature of 720 K. The SO₃ gas from the catalytic converter is absorbed in concentrated H₂SO₄ to produce oleum. Dilution of oleum with water gives H₂SO₄ of the desired concentration. In the industry two steps are carried out simultaneously to make the process a continuous one and also to reduce the cost.

$\mathrm{SO}_{3}+\mathrm{H}_{2} \mathrm{SO}_{4} \rightarrow \mathrm{H}_{2} \mathrm{S}_{2} \mathrm{O}_{7}$
The sulphuric acid obtained by Contact process is 96-98% pure.

Properties
Sulphuric acid is a colourless, dense, oily liquid with a specific gravity of 1.84 at 298 K. The acid freezes at 283 K and boils at 611 K. It dissolves in water with the evolution of a large quantity of heat. Hence, care must be taken while preparing a sulphuric acid solution from concentrated sulphuric acid. The concentrated acid must be added slowly into water with constant stirring. The chemical reactions of sulphuric acid are as a result of the following characteristics: (a) low volatility (b) strong acidic character (c) strong affinity for water and (d) ability to act as an oxidising agent. In aqueous solution, sulphuric acid ionises in two steps.

$\begin{array}{l}{\mathrm{H}_{2} \mathrm{SO}_{4}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \rightarrow \mathrm{H}_{3} \mathrm{O}^{+}(\mathrm{aq})+\mathrm{HSO}_{4}^{-}(\mathrm{aq}) ; K_{\mathrm{a}_{1}}=\text { very large }\left(K_{\mathrm{a}_{1}}>10\right)} \\ {\mathrm{HSO}_{4}^{-}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}(\mathrm{l}) \rightarrow \mathrm{H}_{3} \mathrm{O}^{+}(\mathrm{aq})+\mathrm{SO}_{4}^{2-}(\mathrm{aq}) ; K_{\mathrm{a}_{2}}=1.2 \times 10^{-2}}\end{array}$

The larger value of K_a1 (K_a1>10) means that H₂SO₄ is largely dissociated into H⁺ and HSO^3–. Greater the value of dissociation constant (K_a), the stronger is the acid. The acid forms two series of salts: normal sulphates (such as sodium sulphate and copper sulphate) and acid sulphates (e.g., sodium hydrogen sulphate). Sulphuric acid, because of its low volatility can be used to manufacture more volatile acids from their corresponding salts.

$2 \mathrm{MX}+\mathrm{H}_{2} \mathrm{SO}_{4} \rightarrow 2 \mathrm{HX}+\mathrm{M}_{2} \mathrm{SO}_{4}\left(\mathrm{X}=\mathrm{F}, \mathrm{Cl}, \mathrm{NO}_{3}\right)$

Concentrated sulphuric acid is a strong dehydrating agent. Many wet gases can be dried by passing them through sulphuric acid, provided the gases do not react with the acid. Sulphuric acid removes water from organic compounds; it is evident by its charring action on carbohydrates.

$\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11} \stackrel{\mathrm{H}_{2} \mathrm{SO}_{4}}{\longrightarrow} 12 \mathrm{C}+11 \mathrm{H}_{2} \mathrm{O}$

Hot concentrated sulphuric acid is a moderately strong oxidising agent. In this respect, it is intermediate between phosphoric and nitric acids. Both metals and non-metals are oxidised by concentrated sulphuric acid, which is reduced to SO₂.

$\begin{array}{l}{\mathrm{Cu}+2 \mathrm{H}_{2} \mathrm{SO}_{4}(\mathrm{conc} .) \rightarrow \mathrm{CuSO}_{4}+\mathrm{SO}_{2}+2 \mathrm{H}_{2} \mathrm{O}} \\ {\mathrm{S}+2 \mathrm{H}_{\mathrm{2}} \mathrm{SO}_{4}(\mathrm{conc} .) \rightarrow 3 \mathrm{SO}_{2}+2 \mathrm{H}_{2} \mathrm{O}} \\ {\mathrm{C}+2 \mathrm{H}_{2} \mathrm{SO}_{4}(\mathrm{conc} .) \rightarrow \mathrm{CO}_{2}+2 \mathrm{SO}_{2}+2 \mathrm{H}_{2} \mathrm{O}}\end{array}$

Uses

Sulphuric acid is a very important industrial chemical.
It is needed for the manufacture of hundreds of other compounds and also in many industrial processes.
The bulk of sulphuric acid produced is used in the manufacture of fertilisers(e.g., ammonium sulphate, superphosphate).
Other uses are in: (a) petroleum refining (b) manufacture of pigments, paints and dyestuff intermediates (c) detergent industry (d) metallurgical applications (e.g., cleansing metals before enameling, electroplating and galvanising (e) storage batteries (f) in the manufacture of nitrocellulose products and (g) as a laboratory reagent.