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B-3
It is important to use the amounts of reagents specified in the experiment and to become familiar with the
equipment described in the experimental procedure. Your laboratory instructor is present to answer
your questions. Please do not hesitate to ask your instructor for help is you are unsure of what to do.
Some of the chemical reagents are potentially dangerous, therefore, you must avoid splashing or spilling
chemicals on yourself or your neighbors. In this course, you must wear your safety glasses at all
times in the laboratory. You will not be allowed to stay in the laboratory room without safety glasses
covering your eyes.
ADVANCE STUDY ASSIGNMENT
1.
Imagine that you prepared some copper(II) sulfate crystal (assume 100 % yield) from copper
metal. You then dissolved this copper(II) sulfate crystal in 10.0 mL of water. Five drops of this
solution were subsequently used to investigate some reactions. Assuming that 1 drop = 0.050
mL, what percent by volume of the copper(II) sulfate solution is lost because of these 5 drops?
Answer: 2.5%
2.
If you started with 1.321 g of copper metal in Experiment A, and recovered 0.768 g of copper
metal at the end of Experiment B, what is your percent recovery? Answer: 58.1%
3.
Write a balanced molecular or net ionic equation for the reaction that leads to each of the
products listed in the reaction schemes on page B-1. Include the phase for each species.
a.
Equation for the formation of the tetraamminecopper(II) complex ion from Cu
2+
(aq)
.
b.
Equation for the formation of copper(II) hydroxide from copper(II) sulfate.
c.
Equation for the formation of copper(II) oxide from copper(II) hydroxide.
d.
Equation for the formation of copper(II) sulfate from copper(II) oxide.
e.
Equation for the formation of copper (metal) from copper(II) sulfate and zinc metal.
