Solubility curve of a hydrated salt in water with temperature is given. The curve indicates that the solution process is

The Henry law constant for ${\mathrm{O}}_2\left(\mathrm{g}\right) \mathrm{and} {\mathrm{N}}_2\left(\mathrm{g}\right)$ in water at $0°\mathrm{C} \mathrm{are} 2.5 \times {10}^4 \mathrm{bar} \mathrm{and} 5.0 \times {10}^4 \mathrm{bar}$ respectively. Calculate $∆{\mathrm{T}}_{\mathrm{f}}$, of solution made by dissolving air at 1 bar pressure. [Given: $$\begin{gathered} \left[\mathrm{mole} \% \mathrm{of} {\mathrm{O}}_2 \mathrm{in} \mathrm{air} =20\% \mathrm{and} \mathrm{mole} \% \mathrm{of} {\mathrm{N}}_2 \mathrm{in} \mathrm{air} = 80\%. \\ {\mathrm{K}}_{\mathrm{f}} \mathrm{of} {\mathrm{H}}_2\mathrm{O}= 1.86 \mathrm{K} \mathrm{kg} {\mathrm{mol}}^{-1}\right] \end{gathered}$$

${\mathrm{H}}_2{\mathrm{O}}_2$ and ${\mathrm{H}}_2{\mathrm{SO}}_4$ have large dielectric constant but the not a good solvent why?

Given liquid solution contains two components $\mathrm{A}$ and $\mathrm{B}$. Component $\mathrm{A}$ follows Henry's law for the mole fraction range $0\le X_A\le 0.1$ at constant temperature (and low pressure, where, it can be taken $\left[\frac{{\mathrm{x}}_{\mathrm{A}}\mathrm{d}\left({\mathrm{lnP}}_{\mathrm{A}}\right)}{{\mathrm{dx}}_{\mathrm{A}}}\right]+\left(1-{\mathrm{x}}_{\mathrm{A}}\right)\left[\frac{\mathrm{d}\left({\mathrm{lnP}}_{\mathrm{B}}\right)}{{\mathrm{dx}}_{\mathrm{A}}}\right]=0$) . Then component $\mathrm{B}$ must follow Raoult's law for the molefraction range $\mathrm{b}\le {\mathrm{X}}_{\mathrm{B}}\le 1$. What is the value of $\mathrm{b}$?

Explain the solubility of ionic compounds in polar solvents.

Water is a non-polar solvent.

Give two examples each of polar and non-polar solvents.

Which of the following are non-polar solvents?

${\mathrm{H}}_2\mathrm{S}$, a toxic gas with a rotten egg-like smell is used for the qualitative analysis. If the solubility of ${\mathrm{H}}_2\mathrm{S}$ in water at $\mathrm{STP}$ is $0.195 \mathrm{m}$, Calculate Henry's law constant. (Write the answer without units)

Henry’s law states that at a constant temperature, the solubility of a gas in a liquid is inversely proportional to the partial pressure of the gas present above the surface of liquid or solution.

Henry's Law states that amount of gas that is dissolved in a liquid is directly proportional to the _____ pressure of that gas above the liquid when the temperature is kept constant.

The values of the Henry's law constant of $\mathrm{Ar}, {\mathrm{CO}}_2, {\mathrm{CH}}_4$ and ${\mathrm{O}}_2$ in water at $25°\mathrm{C}$ are $40.30, 1.67, 0.41$ and $34.86 \mathrm{kbar}$, respectively. The order of their solubility in water at the same temperature and pressure is

What is the concentration of dissolved oxygen at ${50}^{\circ }\mathrm{C}$ under pressure of one atmosphere if partial pressure of oxygen at ${50}^{\circ }\mathrm{C}$ is $0.14 \mathrm{atm}$.
(Henry’s law constant for oxygen$=1.3\times {10}^{–3} \mathrm{mol} {\mathrm{dm}}^{–3}{\mathrm{atm}}^{–1}$)

Solubility (in $\mathrm{M}$) of gas in liquid increases on:-

Which of the following is correct match for separation?

Is the nature of solute important when preparing a solution of a specified concentration?

Which of the following factors affect the solubility of a gaseous solute in the fixed volume of liquid solvent?

[A] Nature of solute [B] Temperature [C] Pressure

Henry’s law is denoted as

What are the examples of miscible and immiscible liquids ?