Calculate the conc. of nitric acid in a sample which has density of 1.41 g/l and mass percentage of nitric acid in it being 69%

Dear student
Given that the mass perentage of Nitric Acid = 69 %
So,Mass of nitric acid solution = 69 g (because 69% means 69 g dissolved in 100 ml of solvent)
And given Density of nitric acid solution = 1.41 g/ml
We knew that
Volume of nitric acid solution = $\frac{mass}{density} = \frac{100}{1.41} = 70.92 ml$

now,
No of moles of nitric acid 

=   $\frac{mass of nitric acid}{molar mass of nitric acid} = \frac{69}{63} = 1.09$

Molarity of the solution = $\frac{moles og nitric acid}{volume of solution in liters}$

 

                              = $\frac{1.09 x 1000}{70.92} = 15.37 \raisebox{1ex}{$moles $}\!\left/ \!\raisebox{-1ex}{$ liter$}\right.$

Hence Concentration of nitric acid = 15.37 molL^-1

Regards