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

How many gram of ${{\rm{I}}_2}$ are present in a solution which requires 40 mL, of 0.11 N ${\rm{N}}{{\rm{a}}_2}{{\rm{S}}_2}{{\rm{O}}_3}$ to react with it, ${{\rm{S}}_2}{\rm{O}}_3^{2 - } + {{\rm{I}}_2} o {{\rm{S}}_4}{\rm{O}}_6^{2 - } + 2{{\rm{I}}^ - }?$

In chromatography, the component that travels the furthest on the chromatogram is the one that is:

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

100 mL of 0.1 M solution of a reductant is diluted to 1 litre, which of the following changes?

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

A standard solution is one whose :

A solution is prepared by dissolving 20g of a non-volatile solute in 180g of water. If the vapor pressure of pure water at this temperature is 23.76 mmHg and the solution exhibits a vapor pressure of 23.52 mmHg, what is the molar mass of the solute? (Molar mass of water = 18 g/mol)

In the following change, $3{\rm{Fe}} + 4{{\rm{H}}_2}{\rm{O}} o {\rm{F}}{{\rm{e}}_3}{{\rm{O}}_4} + 4{{\rm{H}}_2}$. If the atomic weight of iron is 56, then its equivalent weight will be :

Which of these is the correct formula for calculating molality?

If we dissolve 20g of NaOH in 200ml of water, what will be the mass percentage of NaOH in the solution (assuming the density of water is 1g/ml)?