A sample of concentrated nitric acid has a density of 1.41gmL and contains 70.0% HNO3 by mass. (a).what mass of HNO3 per liter of solution? (b).what is the molarity of the solution

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Answer 1 · 2018-03-07T10:29:55

Well, we need to make the calculation... $"moles of solute"/"volume of solution"$

And we are given that $rho_"acid"=1.41*g*mL^-1$ ..

.............and so ...........

$"mass of a litre volume"-=1.41*g*mL^-1xx1000*mL*L^-1=1410*g$

And we can work out the concentration of the nitric acid solution, simply by taking a $1*mL$ volume....

$[HNO_3(aq)]="moles of acid"/"volume of solution"=$

$((1.41*gxx70.0%)/(63.01*g*mol^-1))/(1*mLxx10^-3*L*mL^-1)=15.7*mol*L^-1$

... $68-70%w/w$ is the concentration that we typically use in the lab.