35. In the unbalanced equation below, which of the following is the number of moles of NaOH required to neutralize 1 mole of H2SO4?
Answer: A
2 moles of NaOH are required to neutralize 1 mole of H2SO4.
When sulfuric acid (H2SO4) reacts with sodium hydroxide (NaOH), it requires 2 moles of NaOH to completely neutralize 1 mole of H2SO4, resulting in the formation of water and sodium sulfate.
A) 2 moles
This option is correct because the balanced chemical equation for the neutralization reaction shows that 1 mole of H2SO4 reacts with 2 moles of NaOH to produce 2 moles of water and 1 mole of sodium sulfate.
B) 1.5 moles
This option is incorrect because 1.5 moles of NaOH would not completely neutralize 1 mole of H2SO4. The stoichiometry of the reaction does not support this ratio, as it requires exactly 2 moles for complete neutralization.
C) 0.5 moles
This option is also incorrect. Using only 0.5 moles of NaOH would result in an incomplete reaction, where not all of the H2SO4 would be neutralized, leaving excess acid in the solution.
D) 1 mole
This option is incorrect because 1 mole of NaOH is insufficient to neutralize 1 mole of H2SO4. The balanced equation clearly indicates that 2 moles of NaOH are necessary for complete neutralization.
Conclusion
The requirement of 2 moles of NaOH for the neutralization of 1 mole of H2SO4 is derived from the stoichiometry of the balanced chemical equation. All other options fail to provide the appropriate amounts needed for complete neutralization, confirming that A is the only correct choice.