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If the density of methanol is 0.793 kg L...

If the density of methanol is 0.793 kg `L^(-1)`. What is its volume needed for making 2.5L of its 0.25M solution?

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We have given Density = 0.793 kg `L^(-1)= 0.793 xx 10^(3) g L^(-1)`
Find volume `V_(2)= 2.5L`
Final molarity `M_(2)= 0.25M`
Molarity of initial solution `M_(1)`= ?
Initial volume `V_(1)=` ?
Molar mass of methanol, `CH_(3)OH= (1 xx 12.01) (4 xx 1.0079) + 16.00= 32.0416= 32 g "mol"^(-1)`
Molarity `=(0.793 xx 10^(3) g L^(-1))/(32 g "mol"^(-1))= 24.781 mol L^(-1)`
Molarity equation `M_(1)V_(1)= M_(2)V_(2)`
`24.781 xx V_(1)= 0.25 xx 2.5`
`V_(1)= (0.25 xx 2.5)/(24.781)= 0.02522L= 25.22 mL`
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