SO₂ gas is passed into lime water. Which of the following does not take place.

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In the beginning, lime water turns milky due to formation of insoluble CaSO₃

If excess SO₂ is passed milkyness disappears due to formation of soluble Ca(HSO₃)₂

On boiling the solution obtained by passing excess SO₂, its milkyness reappears due to decomposition of Ca(HSO₃)₂ to CaSO₃

Crystallization from the solution obtained by passing excess SO₂ forms solid CaS₂O₅

answer is C.

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Detailed Solution

$\underset{lime water}{Ca (OH)_{2}} + {SO}_{2} \to H_{2} O + {CaSO}_{3} (milky)$
$\underset{milkyness}{{CaSO}_{3}} + H_{2} O + {SO}_{2} \to \underset{Colorless solution}{Ca ({HSO}_{3})}$
$Ca {({HSO}_{3})}_{2} \overset{Δ}{\to} {CaS}_{2} O_{5} (s) + H_{2} O$
Bisulphites convert into pyrosulphites during crystallization.