30 mL of CH₃OH (d = 0.8 g/cm3) is mixed with 60 mL of C₂H₅OH (d = 0.92 g/cm³) at 25°C to form a solution of density 0.88 g/cm³. 

Select the correct option(s) :

30 mL of CH₃OH ............
CH₃OH is solute (less amount)
Mass of CH3OH = 30 × 0.8 = 24 g
Mass of C₂H₅OH = 60 × 0.92 = 55.2 g
Mass of solution = 79.2 g

$\begin{array}{l}\text{ Volume of solution }=\frac{79.2}{0.88}=90\mathrm{mL}\\ \text{ Molarity }=\frac{{\mathrm{n}}_{{\mathrm{CH}}_0\mathrm{O}}}{\mathrm{V}\left(\mathrm{L}\right)}=\frac{24/32}{90}\times 1000=8.33\mathrm{M}\\ \text{ Molality }=\frac{24/32}{55.2}\times 1000=13.59\mathrm{m}\\ \text{ Mole fraction of solute }=\frac{\frac{24}{32}}{\frac{24}{32}+\frac{55.2}{46}}=0.38\\ \text{ Mole fraction of solvent }=1-0.38=0.62\end{array}$