Question

Determine each of the following for a 0.063 M KOH solution. Determine [H3O+] for this solution? PH? Write a balanced equation for the reaction with H2SO4. Express answer as a chemical equation. Also calculate the volume in milliliter of KOH solution required to neutralize 33.0 mL of a 0.043 MH2SO4 solution

Answer 1

concentration of KOH = 0.063 M

pOH = -log[OH-]

       = -log0.063

        = 1.2

pH = 14-1.2 = 12.8

[H3O+] = 10^-pH

             = 10^-12.8

             = 1.58*10^-13 M

H2SO4(aq) + 2KOH(aq) -----> K2SO4(aq) + 2H2O(l)

1 mol H2SO4(aq) = 2 mol KOH(aq)

no of mol of H2SO4 reacted = 33*0.043 = 1.42 mmol

no of mol of KOH reacted = 1.42*2 = 2.84 mmol

volume of KOH reacted = n/M = 2.84/0.063 = 45 ml