In the reaction between NaOH and H2SO4, how many moles of NaOH are required to completely react with 1 mole of H2SO4 according to the balanced chemical equation?

• A. 1 mole
• B. 0.5 mole
• C. 2 moles
• D. 3 moles

Answer: (C)

Verified step by step guidance

1. Write the balanced chemical equation for the reaction between sodium hydroxide (NaOH) and sulfuric acid (H2SO4). The reaction is: \(\mathrm{H_2SO_4 + 2\ NaOH \rightarrow Na_2SO_4 + 2\ H_2O}\).
2. Identify the mole ratio between H2SO4 and NaOH from the balanced equation. Here, 1 mole of H2SO4 reacts with 2 moles of NaOH.
3. Since the problem states you have 1 mole of H2SO4, use the mole ratio to find the moles of NaOH required: multiply 1 mole of H2SO4 by the ratio \(\frac{2\ \text{moles NaOH}}{1\ \text{mole H_2SO_4}}\).
4. Calculate the moles of NaOH needed: \$1 \times 2 = 2$ moles of NaOH.
5. Conclude that 2 moles of NaOH are required to completely react with 1 mole of H2SO4 according to the balanced chemical equation.