$1\mathrm{ }\mathrm{g}$ of a non-volatile non-electrolyte solute is dissolved in $100\mathrm{ }\mathrm{g}$ of two different solvents $\mathrm{A}$ and B whose ebullioscopic constants are in the ratio of $1:5$. The ratio of the elevation in their boiling points, $\frac{∆{\mathrm{T}}_{\mathrm{b}}\left(\mathrm{A}\right)}{∆{\mathrm{T}}_{\mathrm{b}}\left(\mathrm{B}\right)}$, is: (assuming they have the same molar mass)

If $80 \mathrm{g}$ of copper sulphate ${\mathrm{CuSO}}_4·5{\mathrm{H}}_2\mathrm{O}$ is dissolved in deionised water to make $5 \mathrm{L}$ of solution. The concentration of the copper sulphate solution is $x\times {10}^{-3}\text{ mol }{L}^{-1}.$ The value of $x$ is _____.

$[\text{Atomic masses }\mathrm{Cu} : 63.54\mathrm{u}, \mathrm{S} : 32\mathrm{u}, \mathrm{O} : 16\mathrm{u}, \mathrm{H} : 1\mathrm{u}]$

A company dissolves '$\mathrm{x}$' amount of ${\mathrm{CO}}_2$ at $298 \mathrm{K}$ in $1$ litre of water to prepare soda water. $\mathrm{x}=.......\times {10}^{-3} \mathrm{g}$. (nearest integer)

(Given: partial pressure of ${\mathrm{CO}}_2$ at $298 \mathrm{K}=0.835$ bar. Henry's law constant for ${\mathrm{CO}}_2$ at $298 \mathrm{K}=1.67 \mathrm{kbar}$. Atomic mass of $\mathrm{H},\mathrm{C}$ and $\mathrm{O}$ is $1,12$, and $6 \mathrm{g}{ \mathrm{mol}}^{-1}$, respectively)

Solute A associates in water. When $0.7 \mathrm{g}$ of solute $\mathrm{A}$ is dissolved in $42.0 \mathrm{g}$ of water, it depresses the freezing point by $0.2 °\mathrm{C}$. The percentage association of solute $\mathrm{A}$ in water, is

[Given: Molar mass of $\mathrm{A}=93 \mathrm{g}{ \mathrm{mol}}^{-1}$. Molal depression constant of water is $1.86 \mathrm{K} \mathrm{kg}{ \mathrm{mol}}^{-1}$]