Ncert Exercises & Solutions

1.12 If the density of methanol is 0.793 kg L–1, what is its volume needed for making 2.5 L of its 0.25 M solution?

Molar mass of methanol ( ${CH}_{3} OH$ ) = (1 × 12) + (4 × 1) + (1 × 16)
= 32 g ${mol}^{- 1}$
= 0.032 kg ${mol}^{- 1}$
Molarity of methanol solution = $\frac{0.793 kg / L}{0.032 kg / mol}$
= 24.78 mol/L

(Since density is mass per unit volume)

Applying,

$M_{1} V_{1} = M_{2} V_{2}$

(Given solution) (Solution to be prepared)

(24.78 mol/L) $V_{1}$ = (2.5 L) (0.25 mol/L)
$V_{1}$ = 0.0252 L
$V_{1}$ = 25.22 mL

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