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]#?

1 Answer
Jul 2, 2017

Answer:

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.