Double Replacement Reactions Lab
Purpose:
To observe 16 double replacement reactions, predict the product using
solubility table and write balanced chemical equations for each.
Introduction:
Formula Equation
FeCl3(aq) + Pb(NO3)2(aq) → PbCl2(s) +
Low



Fe(NO3)3(aq)
High Solubilty
Two ionic compounds in solution react.
Metals switch with Anions.
At least one new compound has low solubility and is solid
Make sure that you do each of the following:
 Write proper formulas using a Periodic Table.
 Write correct phase symbols using a solubility chart.
 Balance each equation.
Data and Observations
1.
CuSO4(aq) + Na2CO3(aq) →
Blue precipitate
2.
KI(aq) + Pb(NO3)2(aq) →
Yellow precipitate
3.
Na2CO3(aq)
+
CoCl2(aq) →
Pink precipitate
4.
Na2CO3(aq)
+
Ni(NO3)2(aq) →
Mint green precipitate
5.
Na2CO3(aq) +
Hg(NO3)2(aq) →
Yellow precipitate
6.
NaOH(aq) +
NiCl2(aq) →
Mint green precipitate
7.
Na2SO4(aq) + Pb(NO3)2(aq) →
White precipitate
8.
Na2S (aq)
+
Fe(NO3)3(aq) →
Brown precipitate
9.
NaOH (aq) +
Fe(NO3)3(aq) →
Orange precipitate
10.
NaOH (aq) + CoCl3(aq) →
Blue precipitate
11.
CaCl2(aq) + Sr(NO3)2(aq) → No Reaction
12.
ZnCl2(aq) +
NaCl(aq) → No Reaction
13.
NaCl(aq) + AgNO3(aq) →
White precipitate
14.
KI(aq)
+
AgNO3(aq) →
Yellow precipitate
15.
KI(aq)
+
Hg(NO3)2(aq) →
Orange precipitate
16.
NaCl(aq) +
Pb(NO3)2(aq) →
White precipitate
Conclusion
 Use past tense and no pronouns.
 Read the purpose and state that the objectives of purpose were accomplished.
 Describe a double-replacement reaction
 Describe how to predict a double-replacement reaction.
 Describe the properties of the ionic compounds made in this lab.
 Describe what double-replacement reactions are used for.
 Make one more intelligence and profound comment.