Part I: Use the virtual lab to answer the questions below.
1. The solution labeled “1.00 g NaCl” contains 1.00 g of NaCl dissolved in water. Use the solution viewer to
determine the number of grams of Na+ and Cl– in the solution, and confirm that these add to 1.00 g.
You will need to make sure the units in the table are in grams. Use the drop-down menu to select grams.
a. Mass of each species:
Mass Na+ =
Mass Cl– =
Total mass =
b. Why does the mass of Na+ and Cl– in solution add up to 1.0 g?
c. Why are there not equal masses of Na+ and Cl– in solution?
Norfolk State University Chemistry
CHM 221L – 90
Fall 2020
2. The solution labeled “1.00 g AgNO3” contains 1.00 g of solid AgNO3. Add 100.0 mL of water to this
solution. (Recall that to add 100.0 mL of water to the flask labelled “1.00 g AgNO3“, you drag the 3.0 L
water jug on top of the flask, and using the ‘Precise’ mode, enter 100.0 mL, and click pour).
Again, use the solution viewer to determine the number of grams of Ag+ and NO3– in the solution.
a. Mass of each species:
Mass Ag+ =
Mass NO3– =
Total mass =
b. Why does the mass of Ag+ and NO3– in solution add up to 1.0 g?
c. Why does NO3– not form N5+ and 3 O2– in solution?
3. Now pour the entire contents of the flask labelled ‘1.00 g of solid AgNO3’ into the flask containing the 1.00
g solution of NaCl.
a. Write down the mass of each species in solution and the mass of solid AgCl formed.
Table 1: Mass of each species after reaction
| Na+ | Cl– | NO3– | Ag+ | AgCl (s) |
| Species Mass (g) |
b. Are these masses consistent with your results from Questions 1 and 2? Explain why or why not.
Norfolk State University Chemistry
CHM 221L – 90
Fall 2020
Part II. The solution labeled “Solution 1” in the virtual lab stockroom contains 2.00 grams of Sodium Chloride.
1. How many grams of Silver Nitrate must be added to the solution to completely react with Sodium Chloride
according to the reaction below? Show your calculations with clear units and labels for each compound.
NaCl (aq) + AgNO3 (aq) NaNO3 (aq) + AgCl (s)
2. Use the virtual lab to add your calculated amount of Silver Nitrate from Question 1 to ‘Solution 1’. Check
to make sure the reaction was complete, by making sure the amount of Ag+ and Cl– in the solution are both
less than 0.01g.
a. Mass of each species:
Mass Ag+ =
Mass Cl– =
Mass solid AgCl =
3. Add an additional 1.0 g of silver nitrate to ‘Solution 1’. Again, check the masses of each of the following
species:
Mass of each species:
Mass Ag+ =
Mass Cl– =
Mass solid AgCl =
What do you notice about the masses of the above species compared to the masses in the previous step
(Q2). Do your results make sense? Explain why or why not.
Norfolk State University Chemistry
CHM 221L – 90
Fall 2020
Part III. The solution labeled “Solution 2” in the virtual lab stockroom contains 3.00 grams of AgNO3.
1. If excess NaCl is added to the solution, how many grams of AgCl(s) will be formed? Show your calculations
below:
2. Use the virtual lab to check your answer Part III Question 1 (above). Explain the laboratory procedure you
used to perform this check, and clearly explain your reasoning.
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