Final answer:
The molarity of the sulfuric acid, assuming a 1:1 mole ratio as per the student's condition, is calculated to be 1.8 M, which is option A.
Step-by-step explanation:
To calculate the molarity of sulfuric acid in this titration problem, first note that the mole ratio of NaOH to H2SO4 is actually 2:1 according to the balanced equation H2SO4 (aq) + 2NaOH(aq) → Na2SO4 (aq) + 2H2O(l). However, since the problem assumes a 1:1 mole ratio, we will calculate using this incorrect assumption, bearing in mind the actual scenario involves a 2:1 ratio.
Step 1) Calculate moles of NaOH used in the titration:
0.060 L NaOH * 1.2 M NaOH = 0.072 mol NaOH
Step 2) Assuming a 1:1 ratio (incorrect for H2SO4):
0.072 mol NaOH = 0.072 mol H2SO4
Step 3) Calculate the molarity of H2SO4:
Molarity H2SO4 = Moles H2SO4 / Volume H2SO4 in liters
= 0.072 mol H2SO4 / 0.040 L
= 1.8 M
Therefore, the molarity of the sulfuric acid is 1.8 M, option A. However, remember that this answer is based on a hypothetical 1:1 mole ratio as given in the question prompt and not on the correct chemical stoichiometry of the reaction.