To properly neutralize 10N NaOH, how much 2.5N Sulfuric Acid will you need?

To determine how much 2.5N sulfuric acid is needed to neutralize 10N sodium hydroxide, we use the concept of equivalent weight and the neutralization reaction ratio.

In a neutralization reaction, one equivalent of an acid neutralizes one equivalent of a base. Sodium hydroxide is a strong base, and sulfuric acid is a strong acid. The reaction between sulfuric acid (H₂SO₄) and sodium hydroxide (NaOH) is represented as follows:

[ H₂SO₄ + 2 NaOH \rightarrow Na₂SO₄ + 2 H₂O ]

From this equation, we see that one mole of sulfuric acid neutralizes two moles of sodium hydroxide, which indicates that the reaction ratio of H₂SO₄ to NaOH is 1:2.

Given that you have 10N NaOH, you need to find out how many equivalents of NaOH you have in a given volume. If you're working with 1 liter (1,000 mL) of 10N NaOH, it would contain 10 equivalents of NaOH. Since the neutralization ratio is 2:1, you would need:

[ \text{Equivalent of