In the unbalanced equation below, which of the following is the number of moles of NaOH required to neutralize 1 mole of H2SO4?

Rationale

2 moles of NaOH are required to neutralize 1 mole of H2SO4.

In the reaction between sulfuric acid (H2SO4) and sodium hydroxide (NaOH), the balanced equation shows that two moles of NaOH are needed to neutralize one mole of H2SO4, due to the diprotic nature of sulfuric acid.

A (2 moles) CORRECT

This choice is correct because the balanced chemical equation for the neutralization reaction is: H2SO4 + 2 NaOH → Na2SO4 + 2 H2O. This indicates that for every mole of H2SO4, two moles of NaOH are required for complete neutralization.

B (1.5 moles) YOUR ANSWER

Choosing 1.5 moles of NaOH would not suffice for neutralizing 1 mole of H2SO4. Since the stoichiometric ratio is 2:1, 1.5 moles would leave some H2SO4 unreacted, resulting in incomplete neutralization.

C (0.5 moles) YOUR ANSWER

This choice is incorrect as 0.5 moles of NaOH would be inadequate to neutralize even a fraction of 1 mole of H2SO4. The reaction requires two moles of NaOH for complete neutralization, making this option insufficient.

D (1 mole) YOUR ANSWER

One mole of NaOH is also insufficient for the neutralization of 1 mole of H2SO4, as it would only neutralize half of the sulfuric acid present. The required stoichiometry demands two moles of NaOH to fully react with one mole of H2SO4.

Conclusion

In summary, the neutralization of sulfuric acid by sodium hydroxide follows a clear stoichiometric relationship where 2 moles of NaOH are necessary to neutralize 1 mole of H2SO4. Understanding this ratio is crucial in stoichiometry to ensure complete reactions in acid-base chemistry.

In the unbalanced equation below, which of the following is the number of moles of NaOH required to neutralize 1 mole of H2SO4?

2 moles of NaOH are required to neutralize 1 mole of H2SO4.

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