`H_(2)C_(2)O_(4)` and `NaHC_(2)O_(4)` behave as acids as well as reducing agents. Which of the following are correct statements?

Options

A. Equivalents weights of `H_(2)C_(2)O_(4)` and `NaHC_(2)O_(4)` are equal to their molecular weights when acting as reducing agents.
B. Equivalents weight of `H_(2)C_(2)O_(4)` and `NaHC_(2)O_(4)` are equal to half their molecular weights when acting as reducing agents.
C. 100 " mL of " 1 M solution of each is neutralised by equal volumes of 1 Nca (OH)_(2)`
D. 100 " mL of " 1 M solution of each is oxidised by equal volumes of 1 M `KMnO_(4)`.

Answer

B, D

Explanation

`H_(2)C_(2)O_(4)`: As acid `n=2`
As reducing agent `n=2`
`NaHC_(2)O_(4)`: As acid `n=1`
As reducing agent, `n=2`
`E_(H_(2)CO_(2)O_(4))]_("as reducing agent")=(M)/(2)`:
`E_(NaHC_(2)O_(4))]_("as reducing agent")=(M)/(2)`
On reaction with `KMnO_(4)`
`H_(2)C_(2)O_(4)` and `NaHC_(2)O_(4)`: both are acting as reducing agents with same n factor of 2.
`m" Eq of "KMnO_(4)-=m" Eq of "H_(2)C_(2)O_(4)`
`m" Eq of "KMnO_(4)-=m" Eq of "NaHC_(2)O_(4)`