If 1 litre of 2.2M sulphuric acid is poured into a bucket containing 10 litres of water and the resulting…

Analyze the question: This is a dilution problem. Acid of known concentration is added to water, so the amount of acid stays the same but the total volume increases.

Concept: Moles of solute stay constant during dilution:

C₁V₁ = C₂V₂

Solution:

• Moles of H₂SO₄ = 2.2 mol/L × 1 L = 2.2 mol
• Total volume after mixing = 1 L + 10 L = 11 L
• New concentration = 2.2 mol ÷ 11 L = 0.2 mol/L

Check with the formula: 2.2 × 1 = C₂ × 11, so C₂ = 2.2/11 = 0.2 M

Answer: The correct option is C (0.2M).

Common traps:

• Option D (0.11M) comes from dividing by 20 or from mistakes in the volume. Don't do that.
• Option B (1.1M) would be correct only if you added 1 L of water (total volume 2 L).
• Many students forget to add the original 1 L of acid to the 10 L of water. The final volume is 11 L, not 10 L.

Tip: For dilution questions, always find the final total volume first (acid + water). Then use C₁V₁ = C₂V₂. Here 2.2 divided by 11 gives a neat 0.2, which is a good sign you have the right volume.