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
Here's how to calculate the solubility of CuSO_4: Step 1: Calculate the number of moles of CuSO_4. First, determine the molar mass of CuSO_4. Atomic mass of Cu ≈ 63.5 \, g mol^-1 Atomic mass of S ≈ 32.0 \, g mol^-1 Atomic mass of O ≈ 16.0 \, g mol^-1 Molar mass of CuSO_4 = 63.5 + 32.0 + (4 × 16.0) = 63.5 + 32.0 + 64.0 = 159.5 \, g mol^-1. For simplicity, and to match the calculation in the provided explanation, we will use 160 \, g mol^-1 as the molar mass. Given mass of CuSO_4 = 20 \, g. Moles of CuSO_4 = MassMolar Mass Moles of CuSO_4 = 20 \, g160 \, g mol^-1 Moles of CuSO_4 = 0.125 \, mol Step 2: Calculate the volume of the solution in dm^3. The problem states that 20 \, g of CuSO_4 is dissolved in 100 \, g of water. We assume the density of water is 1 \, g cm^-3 and that the volume of water is approximately the volume of the solution. Volume of water = Mass of waterDensity of water Volume of water = 100 \, g1 \, g cm^-3 Volume of water = 100 \, cm^3 To convert cm^3 to dm^3, recall that 1 \, dm^3 = 1000 \, cm^3. Volume of solution = 100 \, cm^3 × 1 \, dm^31000 \, cm^3 Volume of solution = 0.1 \, dm^3 Step 3: Calculate the solubility in mol dm^-3. Solubility is defined as the number of moles of solute per unit volume of solution. Solubility = Moles of soluteVolume of solution in dm^3 Solubility = 0.125 \, mol0.1 \, dm^3 Solubility = 1.25 \, mol dm^-3 The final answer is D.