what was the concentration of CuSO4 in the sample?
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 wants to analyze a sample of the copper (II) sulfate from a processing plant to find the concentration of copper (II) sulfate in it. He adds pure iron to the sample until no more copper will precipitate. If he ends up using 59mg of pure iron, and the sample has a volume of 490ml, then what was the concentration of CuSO4 in the sample?
Be sure your answer has the correct number of significant digits.
molar mass Fe = 55.84 g/mol
mol=mass/molar mass=0.059/55.84= 1.056e-3 mol of Fe
1 mol of iron is to 1 mol of CuSO4
so mol Fe= mol CuSO4= 1.056e-3 mol
Concentration CuSO4=mol/ volume=1.056e-3/0.490= 2.2e-3 M
only 2 significant digits
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