Name: __________________________________________
Period: ________
Double Replacement Reactions Lab
Introduction:
Chemistry is a science that investigates the nature of matter and its interactions. Chemical reactions are the changes
that occur when one type of matter interacts with another. During chemical reactions, you can sometimes observe
macroscopic changes such as the appearance of a new color, the formation of a solid, or the formation of gas bubbles.
Although you cannot see the atoms and molecules reacting, you can observe macroscopic indications that changes are taking
place among the atoms and molecules. Chemistry attempts to explain macroscopic changes in terms of the behavior of atoms
and molecules on the submicroscopic level. In this lab you will write chemical equations to describe double replacement
chemical reactions, observe the notable macroscopic changes during the reactions, and then use your observations to identify
unknown solutions.
Equipment / Materials:
Small-scale reaction surface (acetate cover)
Solutions 0.1M Concentration:
 ammonium hydroxide (NH4OH)
 iron (III) chloride (FeCl3)
 sodium carbonate (Na2CO3)
 nitric acid (HNO3)
 calcium chloride (CaCl2)
 silver nitrate (AgNO3)
 sodium hydroxide (NaOH)






sulfuric acid (H2SO4)
copper (II) sulfate (CuSO4)
potassium iodide (KI)
sodium phosphate (Na3PO4)
hydrochloric acid (HCl)
lead (II) nitrate (Pb(NO3) 2)
Procedure:
Part 1
1.
2.
Use small-scale pipets to put 1 drop of each chemical in the indicated spaces on the Experimental Page. Use good
technique so that you DO NOT CONTAMINATE THE PIPETS! For background contrast, view the drops on the black
and white backgrounds provided in each box. Stir each mixture by tapping the acetate cover with your fingers.
Make careful notes in your data table after observing each reaction. You must be efficient and try to complete as many
combinations in one class period as possible. You must also be patient, however, as some chemical reactions are slow.
You may want to go back once or twice to look at those combinations that didn’t immediately react to make sure there
is still no change.
Pre-Lab Exercise:
1.
What is the Purpose of this Lab?
2.
Summarize the following:
 Procedure Part 1

Clean up Summary
Data - Part 1: Thirteen Known Solutions
HCl
Pb(NO3)2
Na3PO4
KI
CuSO4
H2SO4
NaOH
AgNO3
CaCl2
HNO3
Na2CO3
FeCl3
*
NH4OH
NH4OH
*
*
FeCl3
FeCl3
*
*
*
Na2CO3
Na2CO3
HNO3
HNO3
*
CaCl2
CaCl2
AgNO3
AgNO3
*
*
NaOH
NaOH
H2SO4
H2SO4
CuSO4
CuSO4
*
KI
KI
Na3PO4
Na3PO4
HCl
Clean Up:
Avoid contamination by cleaning up in a way
that protects you and your environment.
Carefully clean the small-scale reaction surface
by absorbing the contents onto a paper towel.
Then wipe the reaction surface with a damp
paper towel and dry it. Dispose of all the paper
towels in the trashcan. Wash your hands
thoroughly with soap and water.
HCl
Pb(NO3)2
3.
For each of the TEN combinations of chemicals with a star (*) on your data table: USE A SEPARATE SHEET OF PAPER!!
a. Write the ions in a box to the right of the equation.
b. Write the products for each double replacement reaction. Make sure to balance the charges using the correct subscripts.
c. Find the PHASE LABELS for all of the reactants and products. Use the Solubility Chart and your notes.
d. Predict if the double displacement reactions will occur or not.
Remember, when
e. If the reaction will not occur write “nrx” or “no reaction”. If the reaction will occur
H
2CO3 is predicted as a
balance the chemical reaction. This means use coefficients AND complete f-h.
product, the H2CO3
f. Write the complete Ionic equation (separate all the aqueous formulas into ions)
decomposes into water
g. Cross out spectator ions (Ions that appear on both sides of the equation
and carbon dioxide.
h. Rewrite the equation as a net ionic equation (only showing the ions that react!)
POST LAB:
A. You need to provide a total of 5 reactions that occurred during Part 1. .
 All reactions must have the following
components.
 DO NOT use reactions from the pre-lab
i. Balanced chemical equation with
 DO NOT Use a Non Reaction.
physical states
 The first 3 reactions produce precipitates.
th
ii. complete ionic equation with crossed
 The 4 reaction produces only water.
th
out spectator ions
 The 5 reaction must produce a gas.
iii. net ionic equation
Remember:
H2CO3 becomes H2O and CO2
1) Balanced Equation (precipitate)
Complete Ionic Equation
Net Ionic Equation
2) Balanced Equation (precipitate)
Complete Ionic Equation
Net Ionic Equation
3) Balanced Equation (precipitate)
Complete Ionic Equation
Net Ionic Equation
4) Balanced Equation (water only)
Complete Ionic Equation
Net Ionic Equation
5)
Balanced Equation (gas)
Complete Ionic Equation
Net Ionic Equations
B. Infer why the precipitate cannot be dissolved by water.
 Use and underline the terms soluble, insoluble, charged particles, water, and attraction.
 Include ONE example from your data that shows this phenomenon.
C. In question A you were asked to find three different types of products. 1. Explain how you knew each
type of a reaction occurred. Use evidence in the explanation. 2. Provide an explanation and example of
a reaction that occurred but had no observable reaction.