State solid in water and nitric acid and then dilute

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Reference no: EM13172708

Suppose you have a copper nitrate solid. You are not sure, however, if the solid is copper (I) nitrate, CuNO3, or copper (II) nitrate, Cu(NO3)2. You dissolve a 0.1015 gram sample of this solid in water and nitric acid and then dilute it to a final volume of 100. mL. You treat a sample of this solution with ammonia and then measure the absorbance of the resulting blue-violet solution. By comparing the absorbance of this solution to that of standard copper solutions you determine the concentration of Cu2+ to be 5.41 x 10-3 M. Use this information (and the hints below) to find the mole ratio of Cu : NO3 and determine the chemical formula for the original copper nitrate sample. 1) Determine the total number of moles of Cu present in the original solid sample knowing that the solid was dissolved in enough water to make 100 mL of solution. Remember the molarity of this solution was experimentally determined using spectroscopy. 2) Calculate the mass of copper present in the original solid sample. 3) Calculate the mass of nitrate ions present in the original solid sample of copper nitrate by mass difference. 4) Determine the moles of NO3 present in the solid sample. 5) Determine the Cu:NO3 mole ratio and figure out the chemical formula of the compound. Please label each part so I know what work goes with which part of the question.

Reference no: EM13172708

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