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

Question

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

Luna Chen · Accepted Answer

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

The following acid-base reaction is carried out by us. #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" are equal to 67.02x10^-3*Lx6.000*mol*L^-1, or 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#? However, it seemed that TENFOLD had been diluted in this solution. 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#.. In other words, the problem specification is incorrect, and your question was chemically unreasonable.

Natalie Anton · Answer

undefined To determine the concentration of sulfuric acid in the given scenario, we need additional information such as the mass or volume of the sulfuric acid and the volume of the solution it is dissolved in. Without this information, it is not possible to calculate the concentration accurately. Could you please provide more details about the scenario?

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]#?

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