a solution containing one mole of NaCl and 1.5 mole of H2SO4 will be neutralized by
Answers
A little over 1 mole of H+. H2SO4, a strong acid, will basically completely dissociate, and form its conjugate base, HSO4-. That gives one mole of H+ ions. That will react with the OH- to yield water. They will effectively neutralize each other so the pH if the solution should be 7 given that the solvent is water. However HSO4- also acts a weak acid so it will dissociate further reducing pH. You didn't give the volume of the NaOH and H2SO4 solutions that are reacting, so for simplicity sake, I'm going to assume 500ml of each at two molar concentration. We need to look at the Ka expression of HSO4- to find how much of it dissociates. After the strong acid and base neutralize we get a 1 molar solution of HSO4-.
KHSO4=[H+][SO4^2-]/[HSO4-]
KHSO4 is equal to 1.2 * 10^-2
Concentration of H+ and SO4^2- are equal, we can label that number x. Concentration
We obtain 1.2*10^-2= (x^2)/1
X=(1.2*10^-2)^0.5 = .1095 M
Given that the solution is 1 liter, the amount of produced H+ from HSO4- is .1095 moles.
Thus 1 mole of H2SO4 in a 1 liter solution of 1 M NaOH will yield 1.1095 moles of protons of which 1 mole is neutralized.