Iodine reacts with hypo to give _____.

What is the weight of sodium bromate and molarity of solution necessary to prepare $85.5 \mathrm{mL}$ of $0.672 \mathrm{N}$ solution, when the half-cell reaction is ${\mathrm{BrO}}_3^{-}+6{\mathrm{H}}^{+}+6{\mathrm{e}}^{-}\to {\mathrm{Br}}^{-}+3{\mathrm{H}}_2\mathrm{O}$?

Give answer after multiplying with 100 and rounding off to the nearest integer value.

The ${\mathrm{Mn}}_3{\mathrm{O}}_4$ formed on strong heating of a sample of ${\mathrm{MnSO}}_4· 4{\mathrm{H}}_2\mathrm{O}$ was dissolved in $100 {\mathrm{cm}}^3$ of $0.1 \mathrm{N} {\mathrm{FeSO}}_4$ containing dilute ${\mathrm{H}}_2{\mathrm{SO}}_4$. The resulting solution reacted completely with $50 {\mathrm{cm}}^3$ of ${\mathrm{KMnO}}_4$ solution. $25 {\mathrm{cm}}^3$ of this ${\mathrm{KMnO}}_4$ solution required $30 {\mathrm{cm}}^3$ of $0.1 \mathrm{N} {\mathrm{FeSO}}_4$ solution for complete reaction. Calculate the amount of ${\mathrm{MnSO}}_4·4{\mathrm{H}}_2\mathrm{O}$ in the sample.

Give answer after multiplying with 100 and rounding off to the nearest integer value.

How many gram of ${\mathrm{H}}_2\mathrm{S}$ will react with $6.32 \mathrm{g}$ of ${\mathrm{KMnO}}_4$ to produce ${\mathrm{K}}_2{\mathrm{SO}}_4$ and ${\mathrm{MnO}}_2?$

$20 \mathrm{mL}$ of $\frac{\mathrm{M}}{60}$ solution of ${\mathrm{KBrO}}_3$ was added to a certain volume of ${\mathrm{SeO}}_3^{2-}$ solution. ${\mathrm{Br}}_2$ evolved was removed by boiling and the excess of ${\mathrm{KBrO}}_3$ was back titrated with $5.1 \mathrm{mL}$ of $\frac{\mathrm{M}}{25}$ solution of ${\mathrm{NaAsO}}_2$. Calculate the weight of ${\mathrm{SeO}}_3^{2-}$ in the solution.

give the answer up to three places of decimal.

A sample of hydrazine sulphate $\left({\mathrm{N}}_2{\mathrm{H}}_4{\mathrm{SO}}_4\right)$  was dissolved in $100 \mathrm{mL}$ of water. $10 \mathrm{mL}$ of this solution was reacted with excess of ferric chloride solution and warmed to complete the reaction. Ferrous ion formed was estimated and it required $20 \mathrm{mL}$ of $\mathrm{M}/50$ potassium permanganate solution. Estimate the amount of hydrazine sulphate in one litre of the solution. Reactions:

$4{\mathrm{Fe}}^{+++}+{\mathrm{N}}_2{\mathrm{H}}_4\to {\mathrm{N}}_2+4{\mathrm{Fe}}^{++}+4{\mathrm{H}}^{+}$

${\mathrm{MnO}}_4^{-}+5{\mathrm{Fe}}^{++}+8{\mathrm{H}}^{+}\to {\mathrm{Mn}}^{++}+5{\mathrm{Fe}}^{+++}+4{\mathrm{H}}_2\mathrm{O}$