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Question
The acids present in acid rain are:
(i) Peroxyacetylnitrate
(ii) H2CO3
(iii) HNO3
(iv) H2SO4
Solution
(ii) H2CO3
(iii) HNO3
(iv) H2SO4
Explanation:
Since rainwater has a pH of 5.6 due to the presence of H+ ions formed by the reaction of rainwater with carbon dioxide present in the atmosphere. The reactions can be shown as-
\[\ce{H2O (l) + CO2 (g) -> H2CO3 (aq)}\]
\[\ce{H2CO (aq) -> H+ (aq) + HCO3 (aq)}\]
If the pH of the rainwater falls below 5.6 then it is known as acid rain. SO2 and NO2 after oxidation and reaction with water are major contributors to the acid rain.
\[\ce{2SO2 (g) + O2 (g) + 2H2O (l) -> 2H2SO4 (aq)}\]
\[\ce{4NO2 (g) + O2 (g) + 2H2O (l) -> 4HNO^{-}3 (aq)}\]
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Match List - I with List - II.
| List - I | List - II | ||
|
(a) |
\[\ce{2SO2(g) + O2(g) -> 2SO3(g)}\] | (i) | Acid rain |
| (b) | \[\ce{HOCl(g) ->[hv] \overset{\bullet}{O}H + \overset{\bullet}{C}l}\] | (ii) | Smog |
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| (d) | \[\ce{NO2(g) ->[hv] NO(g) + O(g)}\] | (iv) | Tropospheric pollution |
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