Assume that the solubilities of $\mathrm{KCl}$ and ${\mathrm{KNO}}_3$ are the same at a given temperature. A saturated solution of $\mathrm{KCl}$ is taken at that temperature and solid ${\mathrm{AgNO}}_3$ is added to it. The amount of ${\mathrm{AgNO}}_3$ added is such that all the ions present in the solution get precipitated as $\mathrm{AgCl}$. What will be the state of the solution in terms of saturation? 
 

The oxygen dissolved in water exerts a partial pressure of $20 \mathrm{kPa}$ in the vapour above water. The molar solubility of oxygen in water is ______ $\times {10}^{-5} \mathrm{mol} {\mathrm{dm}}^{-3}.$

(Round off to the Nearest Integer).

[Given : Henry's law constant $={\mathrm{K}}_{\mathrm{H}}=8.0\times {10}^4 \mathrm{kPa}$ for ${\mathrm{O}}_2.$ Density of water with dissolved oxygen$=1.0 \mathrm{kg} {\mathrm{dm}}^{-3}$]

${\mathrm{CO}}_2$ gas is bubbled through water during a soft drink manufacturing process at $298 \mathrm{K}$. If ${\mathrm{CO}}_2$ exerts a partial pressure of $0.835 \mathrm{bar}$ then $\mathrm{x} \mathrm{m} \mathrm{mol}$ of ${\mathrm{CO}}_2$ would dissolve in $0.9 \mathrm{L}$ of water. The value of $\mathrm{x}$ is _______. (Nearest integer)

(Henry's law constant for ${\mathrm{CO}}_2$ at $298 \mathrm{K}$ is $1.67\times {10}^3 \mathrm{bar}$)

Henry's constant (in kbar) for four gases $\mathrm{\alpha },\mathrm{\beta },\mathrm{\gamma }$  and $\delta$ in water at $298 \mathrm{K}$ is given below :

$\begin{array}{ccccc}& \mathrm{\alpha }& \mathrm{\beta }& \mathrm{\gamma }& \mathrm{\delta }\\ {\mathrm{K}}_{\mathrm{H}}& 50& 2& 2\times {10}^{-5}& 0.5\end{array}$

(density of water $={10}^3 \mathrm{k} {\mathrm{gm}}^{-3}$ at $298 \mathrm{K}$ ) This table implies that :

From the graph, the value of Henry's constant for the solubility of $\mathrm{HCl}$ gas in cyclohexane is