JEE Advance - Chemistry (2021 - Paper 2 Online - No. 6)
The correct statement(s) related to oxoacids of phosphorous is(are)
Upon heating, H3PO3 undergoes disproportionation reaction to produce H3PO4 and PH3.
While H3PO3 can act as reducing agent, H3PO4 cannot.
H3PO3 is a monobasic acid.
The H atom of P-H bond in H3PO3 is not ionizable in water.
Explanation
(a) H3PO3 gives H3PO4 and PH3 on heating. This reaction is known as disproportionation reaction.
$$4{H_3}P{O_3}\buildrel \Delta \over \longrightarrow 3{H_3}P{O_4} + P{H_3}$$
(b) P in H3PO4 is in its highest oxidation state i.e. + 5 hence, it cannot act as reducing agent. But P in H3PO3 is in oxidation state, + 3 hence, it can act as reducing agent.
(c) H3PO3 contains two $$-$$OH groups, hence it is a dibasic acid.
(d) Hydrogen attached to P, does not ionise in water. Therefore, options (a), (b) and (d) are correct.
$$4{H_3}P{O_3}\buildrel \Delta \over \longrightarrow 3{H_3}P{O_4} + P{H_3}$$
(b) P in H3PO4 is in its highest oxidation state i.e. + 5 hence, it cannot act as reducing agent. But P in H3PO3 is in oxidation state, + 3 hence, it can act as reducing agent.
(c) H3PO3 contains two $$-$$OH groups, hence it is a dibasic acid.
(d) Hydrogen attached to P, does not ionise in water. Therefore, options (a), (b) and (d) are correct.
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