The original concentration of copper(II) sulfate in the sample is 5.586 × 10⁻³ M.
Write the balanced chemical equation for the reaction between iron and copper(II) sulfate.
Calculate the number of moles of copper precipitated from the mass of copper precipitated.
Use stoichiometry to determine the number of moles of copper(II) sulfate in the original solution.
Calculate the concentration of copper(II) sulfate in the original solution.
Round the concentration to the correct number of significant digits.
Solution:
The balanced chemical equation for the reaction between iron and copper(II) sulfate is:
Fe(s) + CuSO4(aq) → Cu(s) + FeSO4(aq)
From the balanced chemical equation, we can see that 1 mole of iron reacts with 1 mole of copper(II) sulfate to produce 1 mole of copper.
The number of moles of copper precipitated is:
moles of copper precipitated = mass of copper precipitated / molar mass of copper
moles of copper precipitated = 142.0 mg / 63.55 g/mol = 0.002233 mol
Using stoichiometry, we can determine that the number of moles of copper(II) sulfate in the original solution is equal to the number of moles of copper precipitated.
Therefore, the number of moles of copper(II) sulfate in the original solution is 0.002233 mol.
The concentration of copper(II) sulfate in the original solution is:
concentration of copper(II) sulfate = moles of copper(II) sulfate / volume of solution
concentration of copper(II) sulfate = 0.002233 mol / (400.0 mL / 1000.0 L) = 0.005583 M
Rounding the concentration to the correct number of significant digits (since the mass of copper precipitated has 3 significant digits), we get:
concentration of copper(II) sulfate = 5.586 × 10⁻³ M.
Question
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