Question

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 a 150. 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 122. mg. Calculate the original concentration of copper(II) sulfate in the sample. Be sure your answer has the correct number of significant digits. 602 xs ? Explanation Check

Answer 1

solution: mass of volume of copper obtained = 122 mg 11000 mg = 9) = 0.1229 copper (I) sulfate solution 150 ml = 0.150L (1000ml = 1L) so 150mL cu sou solution contains 122 mg of copber so, no. of moles of copper - 122 mg molar mass of 'ey' moler mass of cul = 63.546 g/mol - 0.122 g 63.540 g/mol = 0.00192 mol of cy.

reaction - Fe(s) + Cusou (49) >140) + fesoylag) Stoichiometrically :- Imol of 'cu obtained from Imol of cusoy So, 0.00192 mol of cy' obtained from = 0.00192 mol of cusou No. of moles of cusoy present - 0.00192 mol. so, vol. of cusou solution = 0.150L (15ome) concentrain of cusoy sol" = no. of mole of cusoy volume of cusoy solution = 0.00192 mol = 10.0128 molil 0.150 L Concentration of cusoy sol" = 0.0128 motit oro.0128 m