[Bobby Sixkiller]

A solution contains HNO3 and HCL of unknown concentrations. To determine the concentrations we take out a sample of 20.0 cm3 of the solution to the titration:

a) First we titrate the sample with NaOH-solution to the titrationpoint (sorry if my English is bad ). 32,3 cm3 0,110 M NaOH-solution is used. Determine two ways to reach to titrationpoint.

I've written down the reaction equations but I still can't figure out two ways?

b) Then, we titrate the sample with a standard solution of silver nitrate.
     The consumption was 15,2 cm3 0,100 M AgNO3. Explain, without calculations, how the   indicator used here works.

I honestly have no idea why.

c) Find the concentration of HCL and HNO3 in the original solution.


Thanks

[Astrokel]

hello there,

I've written down the reaction equations but I still can't figure out two ways?

How do you know when you have reach end point? What do you need to add into the solution to notice the end point have reached? And what is usually used to determine end point of a weak base and weak acid titration?

Explain, without calculations, how the   indicator used here works.

What precipitate is formed here?

[Bobby Sixkiller]

Thank you so much,

that cleared things alittle up

[AWK]

During AgNO₃ titration K₂CrO₄ is used as an indicator. At the end of titration brown precipitate of Ag2CrO4 is formed.

I've written down the reaction equations but I still can't figure out two ways?

Just write down two reaction sepatately
HCl + NaOH = ...
and
HNO₃ + NaOH = ...
In the first titration you will obtan sum of HCl + HNO₃ moles and in the socond one only moles of HCl