For the titration of sulfuric acid (H₂SO₄) with sodium hydroxide (NaOH), how many moles of sodium hydroxide would be required to react with 1.50 L of 0.500 M sulfuric acid to reach the endpoint?

Question

Quizplus · Accepted Answer

The balanced equation for the reaction is:
H2SO4 + 2NaOH → Na2SO4 + 2H2O

From the balanced equation, we can see that 1 mole of sulfuric acid reacts with 2 moles of sodium hydroxide. Therefore, the number of moles of sodium hydroxide required to react with the given amount of sulfuric acid can be calculated as follows:

moles of NaOH = moles of H2SO4 × 2
moles of H2SO4 = Molarity × Volume = 0.500 mol/L × 1.50 L = 0.750 mol
moles of NaOH = 0.750 mol × 2 = 1.50 mol

Therefore, the answer is C) 1.50 mol.

For the Titration of Sulfuric Acid (H2SO4) with Sodium Hydroxide

For the Titration of Sulfuric Acid (H₂SO₄) with Sodium Hydroxide