If you have 184.1 mL of a 1.045 solution of NaOH, how many mL of a 0.550 M solution of H2SO4 do you need in order to neutralize it?

Answer 1

Write a correctly balanced equation for the reaction taking place:

2NaOH(aq) + H2SO4(aq) ==> 2H2O(l) + Na2SO4(aq)

moles NaOH present = 184.1 ml x 1 L/1000 ml x 1.045 mol/L = 0.1924 moles NaOH

moles H2SO4 required for neutralization = 0.1924 moles NaOH x 1 mol H2SO4/2 mol NaOH = 0.0962 moles

Volume of 0.550 M H2SO4 required:

(x L)(0.550 mol/L) = 0.09620 moles

x = 0.1749 L x 1000 ml/L = 174.9 mls