The mole fraction of a solute in a $100$ molal aqueous solution is $.......... \times 10^{-2}$ (Round off to the nearest integer). [Given: Atomic masses: $H = 1.0 \ u$,$O = 16.0 \ u$]

If the mole fraction of ethanol in a solution made by mixing $x \ g$ of water and $69 \ g$ of ethanol is $0.6$,then $x = \dots \dots \dots \dots$

$200 \, mL$ of $0.6 \, N$ $H_2SO_4$ and $100 \, mL$ of $0.3 \, N$ $HCl$ are mixed together. The acidic normality of the resultant solution is $........ N$.

The volume of ethyl alcohol (density $1.15 \text{ g/cc}$) that has to be added to prepare $100 \text{ cc}$ of $0.5 \text{ M}$ ethyl alcohol solution in water is: (in $\text{ cc}$)

$63 \ g$ of a compound (Mol. Wt. $= 126$) was dissolved in $500 \ g$ of distilled water. The density of the resultant solution is $1.126 \ g / mL$. The molarity of the solution is: (in $M$)

If $80 \ g$ of copper sulphate $CuSO_{4} \cdot 5H_{2}O$ is dissolved in deionised water to make $5 \ L$ of solution. The concentration of the copper sulphate solution is $x \times 10^{-3} \ mol \ L^{-1}$. The value of $x$ is .... .
[Atomic masses: $Cu = 63.54 \ u, S = 32 \ u, O = 16 \ u, H = 1 \ u$]