You have separate solutions of HCl and H2SO4 with the same concentrations in terms of Molarity. You wish to neutralize a solution of NaOH. Which acid would require more volume (in mL) to neutralize the base?
a.) the HCl solution
b.) the H2SO4 solution
c.) You need to know the acid concentrations to answer this question
d.) You need to know the volume and concentration of the NaOH solution to answer this question
e.) c and d
2006-11-09 00:51:00 · 3 answers · asked by Anonymous in Science & Mathematics ➔ Chemistry
To neutralise 2 moles of NaOH you need 1 mole of H2SO4
To neutralise 2 moles of NaOH you need 2 moles of HCl
Using the formula: moles = MV/1000 ;M = molarity; V = volume in dm3, then:
a) HCl would require twice the volume as H2SO4 to neutralise an 2 moles of NaOH.
2006-11-09 01:07:44 · answer #1 · answered by Anonymous · 0⤊ 0⤋
The answer is a.
HCl is monoprotic, H2SO4 is diprotic. In other words, there is one equivalent of acid for HCl, 2 for H2SO4, so while the concentration of the two is the same, the normality of the H2SO4 solution is twice that of the HCl solution. It will take twice as much HCl to neutralize the NaOH than it would H2SO4.
2006-11-09 01:01:02 · answer #2 · answered by TheOnlyBeldin 7 · 0⤊ 0⤋
I think it is a) HCl
2006-11-09 01:01:42 · answer #3 · answered by James Chan 4 · 0⤊ 0⤋