An element forms an oxide with the formula X$_2$O$_3$. If the equivalent weight of the element is 9, what is its atomic weight?

The eq. wt. of ${{\rm{I}}_2}$ in the change ${{\rm{I}}_2} o {\rm{IO}}_3^ -$ is :

The number of equivalent per mole of ${{\rm{H}}_2}{\rm{S}}$ used in its oxidation to ${\rm{S}}{{\rm{O}}_2}$ is :

Milliequivalent of a solute in a solution can be given by:

When ${\rm{BrO}}_3^ -$ ion reacts with ${\rm{B}}{{\rm{r}}^ - }$ ion in acidic solution ${\rm{B}}{{\rm{r}}_2}$ is liberated. The equivalent weight of ${\rm{KBr}}{{\rm{O}}_3}$ is :

The equivalent weight of ${\rm{MnS}}{{\rm{O}}_4}$ is half of its molecular weight when it is converted to :

An element X forms a chloride with the formula XCl$_3$ and another chloride with the formula XCl$_5$. 0.1 moles of XCl$_3$ requires 60 mL of 1 N NaOH for complete hydrolysis, while 0.1 moles of XCl$_5$ requires 100 mL of 1 N NaOH. What is the equivalent weight of the element X in XCl$_3$ and XCl$_5$ respectively?

$M$ is the molecular weight of ${\rm{KMn}}{{\rm{O}}_4}.$ The equivalent weight of ${\rm{KMn}}{{\rm{O}}_4}$ when it is converted into ${{\rm{K}}_2}{\rm{Mn}}{{\rm{O}}_4}$ is :

Cerric ammonium sulphate and potassium permanganate are used as oxidising agents in acidic medium for oxidation of ferrous ammonium sulphate to ferric sulphate. The ratio of number of moles of cerric ammonium sulphate required per mole of ferrous ammonium sulphate to the number of moles of ${\rm{KMn}}{{\rm{O}}_4}$ required per mole of ferrous ammonium sulphate, is

If 1.5g of a metal displaces 2g of hydrogen, what is its equivalent weight?

When ${\rm{BrO}}_3^ -$ ion reacts with ${\rm{B}}{{\rm{r}}^ - }$ ion in acidic solution ${\rm{B}}{{\rm{r}}_2}$ is liberated. The equivalent weight of ${\rm{KBr}}{{\rm{O}}_3}$ is :