# How Many Moles of NaOH Are Required to Neutralize 2.4 Mol H2SO4?

**It takes 4.8 moles of sodium hydroxide (NaOH) to neutralize 2.4 moles of sulfuric acid (H _{2}SO_{4}).** The process for solving the correct number of moles of NaOH involves the use of the mole ratio between NaOH and H

_{2}SO

_{4}.

The reaction between an acid, such as H_{2}SO_{4}, and a base, such as NaOH, is known as a neutralization reaction, which produces a salt compound and water. The balanced reaction between NaOH and H_{2}SO_{4} can be represented by the chemical equation 2 NaOH + H_{2}SO_{4} → Na_{2}SO_{4} + 2 H_{2}O.

Based on the equation, the mole ratio between NaOH and H_{2}SO_{4} is 2:1, meaning that it takes twice the amount of NaOH as H_{2}SO_{4}, for the base to completely neutralize the acid and produce sodium sulfate and water. Hence, the number of moles of NaOH needed to burn 2.4 moles of H_{2}SO_{4} is calculated by multiplying 2.4 moles by 2.