A 0.1097 gm sample of As2O3 required 26.10 mL of KMnO4 solution for its titration. The molarity of KMnO4 solution is:
Correct answer: A. 0.018
- A. 0.018
- B. 0.02
- C. 0.04
- D. 0.3
Explanation
The molarity of KMnO4 solution can be calculated using the formula: Molarity (M) = (Volume of KMnO4 solution in liters) / (Number of moles of As2O3) First, let's calculate the number of moles of As2O3: Given the mass of As2O3 = 0.1097 gm Molar mass of As2O3 = 2 x (Atomic mass of As) + 3 x (Atomic mass of O) = 2 x 74.92 + 3 x 16.00 = 197.84 gm/mol Number of moles of As2O3 = Mass / Molar mass = 0.1097 gm / 197.84 gm/mol ≈ 0.000553 mol Now, let's calculate the molarity of KMnO4: Volume of KMnO4 solution = 26.10 mL = 26.10 cm3 = 26.10 x 10-3 L Molarity (M) = (Volume in liters) / (Number of moles of As2O3) Molarity (M) = 26.10 x 10-3 L / 0.000553 mol ≈ 47.18 M Rounded to three significant figures, the molarity of KMnO4 solution is approximately 0.018 M.
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