The oxygen dissolved in water exerts a partial pressure of $20 \ kPa$ in the vapour above water. The molar solubility of oxygen in water is ............ $\times 10^{-5} \ mol \ dm^{-3}$ (Round off to the Nearest Integer). [Given: Henry's law constant $K_H = 8.0 \times 10^{4} \ kPa$ for $O_2$,Density of water $= 1.0 \ kg \ dm^{-3}$]

What happens when a saturated solution of sugar is heated?

Given the solubility curves of $KNO_3$ and $KCl$,which of the following statements is not true?

Given below are two statements:
Statement $I$: The Henry's law constant $K_{H}$ is constant with respect to variations in solution's concentration over the range for which the solution is ideally dilute.
Statement $II$: $K_{H}$ does not differ for the same solute in different solvents.
In the light of the above statements, choose the correct answer from the options.

The air is a mixture of a number of gases. The major components are oxygen and nitrogen with approximate proportions of $20 \%$ and $79 \%$ by volume at $298 \ K$. The water is in equilibrium with air at a total pressure of $10 \ atm$. At $298 \ K$,if the Henry's law constants for oxygen and nitrogen are $3.30 \times 10^{7} \ mm \ Hg$ and $6.51 \times 10^{7} \ mm \ Hg$ respectively,calculate the mole fractions of these gases in water.

$5.5 \text{ mg}$ of nitrogen gas dissolves in $180 \text{ g}$ of water at $273 \text{ K}$ and $1 \text{ atm}$ pressure due to nitrogen gas. The mole fraction of nitrogen in $180 \text{ g}$ of water at $5 \text{ atm}$ nitrogen pressure is approximately: