[Bjc51192]

Hello, I got this question wrong on an exam. can you guys explain to me step by step  how to solve it?

A sample conaining both HCl and HNO3 had a density of 1.083g/ml. A 41.00 ml amount of this sample required 34.72 ml of 0.2489 M NaOH for titration. Another 41.00 ml amount of this sample required 22.51 ml of 0.1866 M AgNO3 for titration. Calculate the mass percent of HNO3 (molar mass = 63.018 g/mol) in the sample.

[opti384]

First determine the mass of the mixture of HCl and HNO3. Then think about what do the titrations with NaOH and AgNO3 mean.

[Bjc51192]

First determine the mass of the mixture of HCl and HNO3. Then think about what do the titrations with NaOH and AgNO3 mean.

can you work it out? I want to see how its done number wise

[opti384]

You have the density and the volume is given. From here you can determine the mass.

For the first titration, H⁺ will be neutralized with OH^- from the base NaOH.

For the second titration, Cl^- from HCl will form a precipitate with Ag⁺, thus forming AgCl.