Name_____________________________________________
North Shore Chemistry
Period: ___________
Date: ____________
Lab: Reactions in Aqueous Solutions
42
Purpose
In this investigation you will observe and consider the results of mixing aqueous solutions of
ionic compounds. You will mix 0.1 M solutions of hydrochloric acid (HCl), silver nitrate (AgNO3),
copper(II) sulfate (CuSO4), potassium chloride (KCl), sodium carbonate (Na2CO3), barium nitrate
(Ba(NO3)2), and sodium hydroxide (NaOH).
Safety
 Wear safety goggles and aprons
Materials
 Reaction template
 Condiment cups to store solutions
 0.1 M hydrochloric acid
 0.05 M silver nitrate
 0.1 M copper sulfate
 0.1 M potassium chloride
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0.1 M sodium carbonate
0.1 M barium nitrate
0.1 M sodium hydroxide
Transfer pipets
Paper towels
Procedure
1. Using pipets, place one drop of each chemical on its respective row or column. Do not
touch the pipets to the solutions on the sheet and DO NOT MIX UP THE PIPETS FROM
ONE CHEMICAL TO ANOTHER.
2. Examine each combination. Take a picture of the results with your cell phone to help you
answer the analysis questions. If you do not have a cell phone, record your observations
on the grid provided in the Analysis Questions.
3. Dispose of the mixtures on your transparency by wiping it clean with a dry paper towel.
Throw the towel in the trash can.
4. Wash your hands thoroughly before leaving the laboratory.
Analysis Questions
1. In your grid labeled “Analysis”:
a. Write the name AND chemical formula for each reactant.
b. Write the formulas of the possible products of each combination.
c. Remember to balance the positive and negative charges within each compound!
2. Circle the products that were insoluble.
Discussion Questions
1. Before you began, you had seven reactant solutions of ionic compounds that were clear
and did not separate when left standing. What is the term used to describe the ionic
solutions which are dissolved in water?
2. How did you know whether a chemical reaction occurred when a pair of solutions was
mixed?
3. What tests, besides visual observation, might be useful in deciding whether a reaction
occurred?
4. Explain in your own words why a precipitate forms. What evidence supports this claim?
5. What are some advantages and disadvantages of conducting this investigation on a
transparency instead of using test tubes or beakers?
6. Predict the solubility of each of the following:
Soluble or insoluble?
(aq) or (s)?
CaCO3
Mg(OH)2
HgCl
Pb(NO3)2
7. Predict whether a reaction occurs when each of the following pairs of solutions are mixed.
If a reaction does occur, write the molecular equation for each of the the following
reactions and identify which product(s) are soluble (aq) and insoluble (s).
a. Sodium carbonate and nitric acid (HNO3)
b. Silver nitrate and sodium chloride
c. Barium nitrate and sodium chloride
8. Suppose you were given three different solutions containing Na3PO4, Ba(NO3)2, and K2CO3,
respectively. Based on the results of this lab, hypothesize about which combinations of
these solutions will produce insoluble precipitates.
Analysis
Sodium
hydroxide
HCl
AgNO3
CuSO4
KCl
Na2CO3
Ba(NO3)2
Barium
nitrate
Sodium
carbonate
Potassium
chloride
Copper(II)
sulfate
Silver
nitrate