# Explain how to answer this :

Given that Conc. HNO_{3}_{ }= 63%

& density of HNO_{3} = 1.4 g/ml

Now, Take 1.0 L of this solution having mass = 1,400 g

Mass of HNO_{3} in 1.0 L = $\frac{63}{100}x1400=882g$

Molar mass HNO_{3} = 1 + 14 + 3 x 16 = 63 g/mol

moles of HNO_{3} in 882g = $\frac{882g}{63gmo{l}^{-1}}$ = 14.0 mol

Molarity of solution = 14.0 M

Calculate volume required to produce 250mL of 1.20M solution by using molarity equation

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

14.0 M x V1 = 1.20 M x 250 mL

V1 = $\frac{1.20Mx250mL}{14.0M}$

V1 = 21.4 mL

Volume required = 21.4 mL

Hence option (B) is correct

Regards

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