One way in which the useful metal copper is produced is by dissolving the mineral azurite, which contains copper(II) carbonate, in concentrated sulfuric acid. The sulfuric acid reacts with the copper(II) carbonate to produce a blue solution of copper(II) sulfate. Scrap iron is then added to this solution, and pure copper metal precipitates out because of the following chemical reaction:Fe(s)+CuSO4(aq)?Cu(s)+FeSO4(aq)Suppose an industrial quality-control chemist analyzes a sample from a copper processing plant in the following way. He adds powdered iron to a200.mL copper(II) sulfate sample from the plant until no more copper will precipitate. He then washes, dries, and weighs the precipitate, and finds that it has a mass of 95.mg.Calculate the original concentration of copper(II) sulfate in the sample. Round your answer to 2significant digits.

From the balanced reaction equation, we obtain the mass of iron reacted by stoichiometry. Then we obtain the number of moles of iron reacted using the mass of iron obtained in the step above. The number of moles of iron is then used to find the concentration of iron reacted with copper II tetraoxosulphate VI. Using the fact that the reactants ratio is 1:1, the initial concentration of CuSO4 can easily be obtained as shown in the image attached.