Question

How many moles of sulfuric acid are required to neutralize 0.80 mol of sodium hydroxide?

H2SO4 + 2NaOH -> Na2SO4 + 2H2O

I got 0.40 mol. Is this right?

Answer 1

correct

Answer 2

ok, thanks

Answer 3

[AI-generated answer — Explain Bot]

To find the number of moles of sulfuric acid required to neutralize sodium hydroxide, you need to use the stoichiometry of the balanced chemical equation.

The balanced equation shows that one mole of sulfuric acid (H2SO4) reacts with two moles of sodium hydroxide (NaOH). This means that the molar ratio between sulfuric acid and sodium hydroxide is 1:2.

Given that you have 0.80 mol of sodium hydroxide, you can calculate the number of moles of sulfuric acid required as follows:

0.80 mol NaOH * (1 mol H2SO4 / 2 mol NaOH) = 0.40 mol H2SO4

So, your calculation of 0.40 mol of sulfuric acid required to neutralize 0.80 mol of sodium hydroxide is correct.