1.The Cu2+ ions in this experiment are produced by the reactionof 1.0g of copper turnings with excess nitric acid. How many molesof Cu2+ are produced?
2. Why isn't hydrochloric acid used in a direct reaction withcopper to prepare the CuCl2 solution?
3. How many grams of metallic copper are required to react withthe number of moles of Cu2+ calculated in Problem 1 to form theCuCl? The overall reaction can be taken to be: Cu2+(aq) + 2Cl-(aq)+ Cu(s) -----> 2CuCl(s)
4. What is the maximum mass of CuCl that can be prepared fromthe reaction sequence of this experiment, using 1.0g of Cu turningsto prepare the Cu2+ solution?
5. A sample of the compound prepared in this experiment ,weighing 0.1021g, is dissolved in HNO3, and diluted to a volume of100 ml. A 10ml aliquot of that solution is mixed with 10 mL 6M NH3.The [Cu(Nh3)4]2+ in the resulting solution is found to be 5.16 x10^-3 M.
a. How many moles of Cu were in the original sample, which hadbeen effectively diluted to a volume of 200 mL.
b. How many grams of Cu were in the sample?
c. How many grams of Cl were in the sample? How many moles?
d. What is the formula of the copper chloride compound?
