Question
$${H_3}P{O_3}\,{\text{and}}\,{H_3}P{O_4}$$ the correct choice is:
A.
$${H_3}P{O_3}$$ is dibasic and reducing
B.
$${H_3}P{O_3}$$ is dibasic and non-reducing
C.
$${H_3}P{O_4}$$ is tribasic and reducing
D.
$${H_3}P{O_3}$$ is tribasic and non-reducing
Answer :
$${H_3}P{O_3}$$ is dibasic and reducing
Solution :
The structure of $${H_3}P{O_3}$$ is as follows: There are only two $$ - OH$$ groups and hence dibasic. The oxidation number of $$P$$ in this acid is $$ + 3$$ . Whereas $$P$$ can have $$ + 5$$ oxidation state also. Therefore, $${H_3}P{O_3}$$ can be oxidised which means $${H_3}P{O_3}$$ is a reducing agent.
The structure of $${H_3}P{O_3}$$ is as follows: There are only two $$ - OH$$ groups and hence dibasic. The oxidation number of $$P$$ in this acid is $$ + 3$$ . Whereas $$P$$ can have $$ + 5$$ oxidation state also. Therefore, $${H_3}P{O_3}$$ can be oxidised which means $${H_3}P{O_3}$$ is a reducing agent.