If 200 mL of a standard 0.15 M NaOH solution is required to neutralize 30 ml of H2SO4, what is the molarity of acid?
The correct option is B 0.5 M We have, 200 mL of a 0.15 M NaOH solution and 30 mL of H2SO4solution of unknown molarity.
Let’s assume the molarity of H2SO4 solution to be M. For complete neutralization, Number of millimole of H+ ions = Number of millimole of OH− ions Since, 1 mol of H2SO4 produces 2 mol of H+ ions. i.e. H2SO4 is a diprotic acid 1×200×0.15=2×30×M M = 0.5 Therefore the molarity of the acid solution is 0.5 M