To solve this problem, we need to find the number of moles of copper II sulfate in the sample and then convert it to grams. We can use the following steps:1. Calculate the number of moles of electrons transferred during the oxidation process.2. Determine the stoichiometry of the redox reaction.3. Calculate the number of moles of copper II sulfate.4. Convert the moles of copper II sulfate to grams.Step 1: Calculate the number of moles of electrons transferred during the oxidation process.The number of moles of electrons n can be calculated using the formula:n = Q / F * z where Q is the charge in coulombs 4.00 C , F is the Faraday constant 96485 C/mol , and z is the number of electrons transferred in the redox reaction. For the oxidation of copper II sulfate, the balanced half-reaction is:Cu + 2e CuSo, z = 2.n = 4.00 C / 96485 C/mol * 2 n = 4.00 C / 192970 C/moln 0.0000207 molStep 2: Determine the stoichiometry of the redox reaction.The balanced redox reaction for the titration of copper II sulfate with the titrant is:Cu + 2e CuSince 2 moles of electrons are required to reduce 1 mole of Cu, the stoichiometry of the reaction is 1:1.Step 3: Calculate the number of moles of copper II sulfate.Since the stoichiometry of the reaction is 1:1, the number of moles of copper II sulfate is equal to the number of moles of electrons:n CuSO = n e 0.0000207 molStep 4: Convert the moles of copper II sulfate to grams.To convert the moles of copper II sulfate to grams, we can use the molar mass of copper II sulfate CuSO , which is approximately 159.61 g/mol:mass CuSO = n CuSO * M CuSO mass CuSO 0.0000207 mol * 159.61 g/molmass CuSO 0.0033 gSo, the amount of copper II sulfate in the sample of solution is approximately 0.0033 grams.