Concentrated \(\mathrm{HNO_3}\) used in the laboratory is \(68\%\) by mass and its density is \(1.5\ \mathrm{g\,mL^{-1}}\). If \(x\) mL of this acid was taken into a 5 L standard flask and filled up to the mark with distilled water to prepare \(5\) L of \(0.5\ \mathrm{M}\ \mathrm{HNO_3}\) solution. What is the value of \(x\) in mL?
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Use
\[
\boxed{\text{Mass}=\frac{\text{Required mass of solute}}{\%\text{ by mass}/100}}
\]
and then
\[
\boxed{\text{Volume}=\frac{\text{Mass}}{\text{Density}}.}
\]