Question

What is the concentration of sulfuric acid in the following scenario?

A `10.0*mL` volume of sulfuric acid, that had been prediluted TENFOLD, was titrated by a `67.02*mL` volume of `NaOH(aq)` of `6.000*mol*L^-1` concentration. What is `[H_2SO_4]`?

Answer 1

Unfeasibly high............

Explanation:

We perform the following acid base reaction.........

`H_2SO_4(aq) + 2NaOH(aq) rarr Na_2SO_4(aq) + 2H_2O(l)`

We add `67.02xx10^-3L` of sodium hydroxide with a concentration of `6.000*mol*L^-1`......

`"Moles of NaOH"=67.02xx10^-3*Lxx6.000*mol*L^-1=0.40212*mol`

And thus in the initial tritrand, the sulfuric acid solution, there were `0.20106*mol` sulfuric acid. Why did I HALVE the concentration with respect to `NaOH`?

But this solution had apparently been diluted TENFOLD..........

And thus there were `(0.20106*mol)/(10.00xx10^-3*L)>=200*mol*L^-1` in the initial solution......This concentration is UNFEASIBLY HIGH. In the lab we can get `98%` `w/w`, which is approx. `18*mol*L^-1` with respect to `H_2SO_4`..

So your question was chemically unreasonable, and the problem specification is WRONG.