$$HBr$$ and $$HI$$ reduce sulphuric acid, $$HCl$$ can reduce $$KMn{O_4}$$ and $$HF$$ can reduce
A.
$${H_2}S{O_4}$$
B.
$$KMn{O_4}$$
C.
$${K_2}C{r_2}{O_7}$$
D.
none of the above
Answer :
none of the above
Solution :
$$\,HI$$ and $$HBr$$ (in that order) are the strongest reducing
hydracids and hence they reduce $${H_2}S{O_4}$$ . $$HCl$$ is quite stable and hence is oxidised by strong oxidising agent like $$KMn{O_4}$$ . $$HF$$ is not a reducing agent. In the smallest
$${F^ - }$$ ion, the electron which is to be removed during oxidation is closest to the nucleus and therefore most difficult to be removed. Therefore, $$HF$$ is a poor reducing agent.
Releted MCQ Question on Inorganic Chemistry >> P - Block Elements
Releted Question 1
The reddish brown coloured gas formed when nitric oxide is oxidised by air is