Calculate the concentration of dissolved gas in water at $25^{\circ} C$ if the partial pressure of the gas at the same temperature is $0.15 \ atm$. $\left[K_H = 0.15 \ mol \ dm^{-3} \ atm^{-1}\right]$ (in $M$)

What happens when a saturated solution of sugar is heated?

If $N_2$ gas is bubbled through water at $293 \ K$,how many millimoles of $N_2$ gas would dissolve in $1 \ L$ of water? Assume that $N_2$ exerts a partial pressure of $0.987 \ bar$. The Henry's law constant for $N_2$ at $293 \ K$ is $76.48 \ kbar$.

Solubility of $N_2$ gas in water at $25\,^{\circ}C$ and $0.78\, atm$ is $5.4 \times 10^{-4}\, M$. Calculate Henry's law constant for $N_2$ in water at $25\,^{\circ}C$.

Which of the following ionic solids exhibits a decrease in its solubility in water with an increase in temperature?

Assertion: $A$ mixture of $He$ and $O_2$ is used for respiration for deep sea divers.
Reason: $He$ is soluble in blood.