Question

100. mL of 0.200 MHCl is titrated with 0.250 MNaOH. What is the pH of the solution at the equivalence point?

Can you include the steps please?

Answer 1

Titration of strong acid (HCl) with strong base (NaOH) -

Initial concentration of H⁺ ions = [Concentration] [Volume]= 0.200 M * 0.100 L = 0.02 mol

At equivalnece point,, moles of H⁺ = moles of OH^- = 0.02 mol

The volume of NaOH added will produce the concentration OH- equal to 0.02 mol (H+ concentration).

Volume of NaoH added = 0.02 mol / 0.25 M = 0.08 L

At equivalence point all the H⁺ ions with react with OH^- ions added.

So, remaining H⁺ concentration in the solution = 0.02 mol -0.02 mol = 0

So, P^H = 7.0 (i.e neutral solution) at .equivalence point.