Question

What volume of 2.5 M H2So4 is required to neutralise a solution containing 2.5 g NaOH?

Answer 1

Let the required volume of H2SO4 be v Litres

Number of equivalents of H2SO4 = Normality of H2SO4 * Volume of H2SO4

= (Molarity of H2SO4 * n factor of H2SO4) * v

= 2.5 * 2 * v

Number of equivalents of NaOH = Moles of NaOH * n factor of NaOH

= 2.5/40 * 1

Since number of equivalents of two reacting species are always equal

Therefore

2.5 * 2 * v = 2.5/40

v = 1/80 Litres or 12.5 millilitres

Hope it helps