100g of a liquid A (molar mass 140 g/mol) and 100g of liquid B (molar mass 70 g/mol) form an ideal solution. What is the mole fraction of B in the vapor phase? (Assume $P^0_A = 70$ mmHg and $P^0_B = 140$ mmHg)

1 gram of sodium hydroxide was reacted with $25 \mathrm{mL}$ of $0.75 \mathrm{M}$ sulfuric acid ($\mathrm{H_2SO_4}$). What mass of sodium hydroxide remains unreacted?

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

Which of these is the correct formula for calculating molality?

How many g of ${\rm{KMn}}{{\rm{O}}_4}$ are needed to prepare 3.75 litre of 0.850 $N$ solution if ${\rm{KMn}}{{\rm{O}}_4}$ is reduced as, ${\rm{MnO}}_4^ - + 8{{\rm{H}}^ + } + 5{\rm{e}} o {\rm{M}}{{\rm{n}}^{2 + }} + 4{{\rm{H}}_2}{\rm{O}}$

What is the molarity of a solution containing 1 mole of solute in 500 mL of solution?

The number of moles of ${K_2}C{r_2}{O_7}$ that will be needed to react with one mole of nitrite ion in acidic solution is

What mass of ${\rm{Mn}}{{\rm{O}}_2}$ is reduced by 35 mL of 0.16 $N$ oxalic acid in acidic solution? The skeleton equation is, ${\rm{Mn}}{{\rm{O}}_2} + {{\rm{H}}^ + } + {{\rm{H}}_2}{{\rm{C}}_2}{{\rm{O}}_4} o {\rm{C}}{{\rm{O}}_2} + {{\rm{H}}_2}{\rm{O}} + {\rm{M}}{{\rm{n}}^{2 + }}:$

Which concentration term is independent of temperature?

The least count of burette used normally in laboratory is :

A mixture of two volatile liquids A and B follows Raoult's law. At a certain temperature, the partial pressures of A and B above the solution are 200 mmHg and 300 mmHg respectively. If the mole fraction of A in the liquid phase is 0.4, what is the vapor pressure of pure A at this temperature?