What is the normality of a ${\rm{KMn}}{{\rm{O}}_4}$ solution to be used as an oxidant in acid medium, which contain 15.8 g of the compound in 100 mL of solution? Mol. wt. of ${\rm{KMn}}{{\rm{O}}_4}$ is 158 :

In a solution containing 0.1 moles of a solute and 5 moles of solvent, what is the mole fraction of the solvent?

When one mole of ${\rm{KMn}}{{\rm{O}}_4}$ reacts with $HCl$, the volume of chlorine liberated at $NTP$ will be:

Which method is employed for concentrating sulfide ores?

A 0.5 molal aqueous solution of urea ($CON_2H_4$) is prepared. What is the mole fraction of urea?

The number of moles of $KMn{O_4}$ that will be needed to react completely with one mole of oxalate ion in acidic solution is

What weight of ${\rm{HN}}{{\rm{O}}_3}$ is needed to convert 5 g of iodine into iodic acid according to the reaction, ${{\rm{I}}_2} + {\rm{HN}}{{\rm{O}}_3} o {\rm{HI}}{{\rm{O}}_3} + {\rm{N}}{{\rm{O}}_2} + {{\rm{H}}_2}{\rm{O}}?$ ?

The least count of burette used normally in laboratory is :

For the reaction, $2{\rm{F}}{{\rm{e}}^{3 + }} + {\rm{S}}{{\rm{n}}^{2 + }} o 2{\rm{F}}{{\rm{e}}^{2 + }} + {\rm{S}}{{\rm{n}}^{4 + }}$ The normality of ${\rm{SnC}}{{\rm{l}}_2}$ (mol.wt. = 189.7) solution prepared by dissolving 47.5 g in acid solution and diluting with ${{\rm{H}}_2}{\rm{O}}$ to a total of 2.25 litre is :

Which concentration term is independent of temperature?

A 1 molal aqueous solution contains 0.5 moles of solute. What is the mass of the solvent (water) in kilograms?