suppose an industrial control chemist analyzes a sample from a copper One way in

Question

suppose an industrial control chemist analyzes a sample from a copper One way in which the useful metal copper is produced is by dissolving the mineral azurite, which contains copper(I) carbonate, in concentrated sulfuric acid The sulfuric acid reacts with the copper(II) carbonate to produce a blue solution of copper(II) sulfate. Scrap metal precipitates out ,and pure copper mical reaction: Fe(s) + CuSO4(aq) ? Cu(s) + FeSO4(aq) processing plant in the following way. He adds powdered iron to a 400. ml. Suppose an industrial quality-control chemist analyzes a sample from a copper copper(I) sulfate sample from the plant until no more copper will precipitate. He then washes, dries, and weighs t of 142. mg Calculate the original concentration of copper'() sulfate in the sample. Be sure your answer has the correct number of significant digits 1

Explanation / Answer

Molar mass of Cu = 63.5 g/mol

Number of moles of Cu = Mass/molar mass = 142 * 10^(-3)/63.5 = 2.236 * 10^(-3) moles

Number of moles of Cu = Number of moles of CuSO4

Molarity = Number of moles/Volume of solution (in L) = 2.236 * 10^(-3)/0.400 = 5.5905 * 10^(-3) M

To change it into g/L, we need to multiply it with molar mass of CuSO4

Molar mass of CuSO4 = 159.609 g/mL

Concentration in g/L = 5.5905 * 10^(-3) * 159.609 g/L = 8.923 * 10^(-1) g/L

Since volume contains 1 significant digit, hence try 9 * 10^(-1) g/L

Or as per weight, try 8.92 * 10^(-1) g/L

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