Find the Unknown Concentration of an Unknown Acid

Question

A total of 25.0 mL of 0.150 M potassium hydroxide (KOH) was required to neutralize 15.0 mL of sulfuric acid (H₂SO₄) of unknown concentration. Balanced Equation as well please.

Answer 1

2KOH + H2SO4 ==> K2SO4 + 2H2O ... balanced equation

moles KOH used = 0.025 L x 0.150 mol/L = 0.00375 moles

moles H2SO4 = 0.00375 mol KOH x 1 mol H2SO4/2 mol KOH = 0.001875 moles H2SO4 present

Concentration H2SO4 = 0.001875 moles/0.015L = 0.125 M