Question

By titration, 13.5 mL of aqueous H2SO4 neutralized 21.8 mL of 0.0419 M LiOH solution. What was the molarity of the aqueous acid solution?

Answer 1

13.5 mL of 0.0339 M H₂SO₄ is titrated with 21.8 mL of 0.0419 M LiOH.

What is titration?

Titration is a process of chemical analysis in which the quantity of some constituent of a sample is determined by adding to the measured sample an exactly known quantity of another substance with which the desired constituent reacts in a definite, known proportion.

• Step 1: Write the balanced equation.

H₂SO₄ + 2 LiOH ⇒ Li₂SO₄ + 2 H₂O

• Step 2: Calculate the reacting moles of LiOH.

0.0218 L × 0.0419 mol/L = 0.000913 mol

• Step 3: Calculate the reacting moles of H₂SO₄.

The molar ratio of H₂SO₄ to LiOH is 2:1.

0.000913 mol LiOH × (1 mol H₂SO₄/2 mol LiOH) = 0.000457 mol H₂SO₄

• Step 4: Calculate the molarity of H₂SO₄.

[H₂SO₄] = 0.000457 mol/0.0135 L= 0.0339 M

13.5 mL of 0.0339 M H₂SO₄ is titrated with 21.8 mL of 0.0419 M LiOH.

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