This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
ScanSolve AI Answer
Step 1: Calculate the molar mass of sulphuric acid (H_2SO_4). The atomic masses are given as H=1, S=32, O=16. Molar mass of H_2SO_4 = (2 × 1) + 32 + (4 × 16) = 2 + 32 + 64 = 98 g/mol Step 2: Calculate the moles of H_2SO_4 required for the desired solution. The target solution is 250 cm^3 (which is 0.250 dm^3) of 0.2 M H_2SO_4. Moles of H_2SO_4 = Molarity × Volume (in dm^3) Moles of H_2SO_4 = 0.2 mol/dm^3 × 0.250 dm^3 = 0.05 mol Step 3: Calculate the mass of H_2SO_4 corresponding to these moles. Mass of H_2SO_4 = Moles × Molar mass Mass of H_2SO_4 = 0.05 mol × 98 g/mol = 4.9 g Step 4: Calculate the volume of pure sulphuric acid (liquid) required using its density. The density of pure sulphuric acid is 1.84 g/cm^3. Volume = MassDensity Volume of pure H_2SO_4 = 4.9 g1.84 g/cm^3 ≈ 2.663 cm^3 Step 5: Select the closest option. The calculated volume is approximately 2.66 cm^3, which matches option B. The final answer is B. 2.66. That's 2 down. 3 left today — send the next one.