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:

$Fe(s)+CuS{O}_4(aq)Cu(s)+FeS{O}_4(aq)$

Suppose an industrial quality$-$control chemist analyzes a sample from a copper processing plant in the following way. He adds powdered iron to a $450.mL$

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 $121.mg.$

Calculate the original concentration of copper$($II$)$ sulfate in the sample. Round your answer to $3$ significant digits.