The weight of oxalic acid that will be required to prepare a $1000 \ mL$ $(N / 20)$ solution is

$20 \, mL$ of a solution of a weak monobasic acid neutralizes $22.18 \, mL$ of a solution of $NaOH$,and $20 \, mL$ of $N/10$ $HCl$ neutralizes $21.5 \, mL$ of the same $NaOH$ solution. The normality of the acid is nearly $.......$ $N$.

Of all the three common mineral acids,only sulphuric acid is found to be suitable for making the solution acidic in redox titrations involving $KMnO_4$ because:

In the iodometric estimation in the laboratory,which process is involved?

Why is it necessary to wash the precipitate before measuring it quantitatively?

The primary standard solution for the estimation of $Na_2S_2O_3$ is: