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With lead
(I) nitrate solution. This precipitation reaction produces a bright yellow solid. (point values in
parentheses)
Part 1:
1. Copy the unbalanced reaction below into your lab notebook. Balance the reaction by adding
coefficients. (1)
KI (aq)
Pb(NO,), (aq)
KNO, (aq)
Pbl, (s)
2. a) Which trial are you assigned?
b) Copy the data table below into your notebook. Watch video A (make sure it's the correct trial!)
and collect your data. You may need to pause or rewatch the video, it goes quickly. (1.5)
Mass of Empty Beaker (g)
Mass of Beaker+ solid Pb(NO,)ใ(g)
Volume of 1.0 M KI (aq) (mL)
For the following calculations, show all your work for full credit.
3. What mass of solid Pb(N0,), was added to the beaker? (1)
4. If the solid Pb(NO,), was dissolved in 45 mL of water, what is the molarity of the Pb(NO,)ใ
solution? (2.5)
5. Which compound is the limiting reactant? (4)
6. What mass of lead (II) iodide (PbL,) should be produced? (2)
Part 2:
7. Watch video B (make sure it's the correct trial!) to see the complete reaction and collection of the
product. Copy the data table below and record your data. (1)
Mass of filter paper (g)
Mass of filter paper + dried precipitate (g)
8. What mass of precipitate was collected? Show your work. (1)
Calculate the percent yield for the reaction. Show your work. (2)
10. For your trial, which three ions were present in the filtered solution at the end of the reaction? In
other words, which three ions are still dissolved at the end of the reaction? Defend/explain your
9.
answer. (3)
11. Watch video C - watch both tests for your trial and record your observations. (1)
a) Add lead (II) nitrate -
b) Add potassium iodide -
12. These tests were conducted to prove the identity of the limiting reactant. Considering your
answers to the previous two questions, describe how these tests support the prediction you made
in question 5 about which compound is the limiting reactant. (2)
