Two solutions, $\mathrm{}\mathrm{A}$ and $\mathrm{B},\mathrm{}$ each of $100\mathrm{}\mathrm{L}$ was made by dissolving $4\mathrm{}\mathrm{g}$ of $\mathrm{N}\mathrm{a}\mathrm{O}\mathrm{H}$ and $9.8\mathrm{}\mathrm{g}$ of ${\mathrm{H}}_2\mathrm{S}{\mathrm{O}}_4$ in water, respectively. The $\mathrm{p}\mathrm{H}$ of the resultant solution obtained from mixing $40\mathrm{}\mathrm{L}$ of solution $\mathrm{A}$ and $10\mathrm{}\mathrm{L}$ of solution $\mathrm{B}$ is ____________. $(\log 2=0.3)$

The value of ${\mathrm{K}}_{\mathrm{c}} \mathrm{us} 64 \mathrm{at} 800 \mathrm{K}$ for the reaction

${\mathrm{N}}_2\left(\mathrm{g}\right)+3{\mathrm{H}}_2\left(\mathrm{g}\right)\to 2 {\mathrm{NH}}_3 \left(\mathrm{g}\right)$

The value of ${\mathrm{K}}_{\mathrm{c}}$ for the following reaction is :

${\mathrm{NH}}_3 \left(\mathrm{g}\right)\to \frac{1}{2} {\mathrm{N}}_2 \left(\mathrm{g}\right)+\frac{3}{2} {\mathrm{H}}_2 \left(\mathrm{g}\right)$

If the solubility product of ${\mathrm{AB}}_2$ is $3.20\times {10}^{-11} {\mathrm{M}}^3$, then the solubility of ${\mathrm{AB}}_2$ in pure water is _______ $\times {10}^{-4} \mathrm{mol} {\mathrm{L}}^{-1}$

[Assuming that neither kind of ion reacts with water]

The variation of equilibrium constant with temperature is given below :

$\begin{array}{cc}\mathrm{Temperature}& \mathrm{EquilibriumConstant}\\ {\mathrm{T}}_1=25°\mathrm{C}& {\mathrm{K}}_1=10\\ {\mathrm{T}}_2=100°\mathrm{C}& {\mathrm{K}}_2=100\end{array}$

The values of $\mathrm{\Delta H}°, \mathrm{\Delta G}°$ at ${\mathrm{T}}_1$ and $\Delta \mathrm{G}°$ at ${\mathrm{T}}_2$ (in $\mathrm{kJ} {\mathrm{mol}}^{-1}$ ) respectively, are close to [use $\mathrm{R}=8.314{\mathrm{JK}}^{-1}{\mathrm{mol}}^{-1}$]