Worksheet 1
Chapter 4: Solution Chemistry and the Hydrosphere
Precipitation Reactions
1.
a. MgSO4(aq) +
NaOH(aq)

b. K2CO3(aq) +
AlCl3(aq)

c. SrBr2(aq) +
Zn(NO3)2(aq)

d. CuSO4(aq)+
NaOH(aq)

e. KI(aq)
Pb(NO3)2(aq)

+
Acid-Base Neutralization Reactions
2. Complete and balance each of the equations below:
NaOH(aq) 
a.
HCl(aq) +
b.
H2SO4(aq) +
KOH(aq) 
c.
H3PO4(aq) +
Ca(OH)2(aq) 
3. Complete and balance each of the equations below:
a.
HCl(aq) +
Na2CO3(s) 
b.
HNO3(aq) +
CaCO3(s) 
c.
H2SO4(aq) +
KHCO3(s) 
d.
HClO4(aq) +
Sr(HCO3)2(s) 
4. Determine the Brønsted-Lowry acid and base in each of the following reactions:
a.
CH3COOH(aq)
b.
NH3(aq)
+
c.
H2O(l)
+
+
NH4+(aq)
NH3(aq)
H2O(l)
H2SO4(aq)
NH4+(aq)
+
H3O+(aq)
CH3COO–(aq)
+
OH–(aq)
+
HSO4–(aq)
5. List the two conjugate acid-base pairs in the examples above:
a. __________________________ and __________________________
b. __________________________ and __________________________
c. __________________________ and __________________________
Chemical Reactions
Combination Reactions: A+ Z  AZ
6. Complete and balance each of the equations below:

a.
Na(s) +
Cl2(g)

b.
Al(s) +
O2(g)

c.
Zn(s) +
S8(s)

d.
Mg(s) +
N2(g)




Decomposition Reactions: AZ  A + Z
7. Classify and balance decomposition reactions. (You won’t need to predict products.)

a. _____ KHCO3(s) 
 _____ K2CO3(s) + _____ H2O(l) + _____ CO2(g)

b. _____ Al2(CO3)3(s) 
 _____ Al2O3(s) + _____ CO2(g)
c. _____ KClO3(s)
, MnO2


  _____ KCl(s) + _____ O2(g)
Single Replacement (or Displacement) Reactions: A + BZ  AZ + B
Activity Series: Li > K > Ba > Sr > Ca > Na > Mg > Al > Mn > Zn >
Fe > Cd > Co > Ni > Sn > Pb > (H) > Cu > Ag > Au
AlCl3(aq)

8.
Mg(s) +
9.
Al(s) +
CdSO4(aq)

10.
Cd(s) +
AgNO3(aq)

11.
Ag(s) +
Mg(NO3)2(aq)

Replacement Reactions that produce hydrogen gas: A + HB  AB + H2

12.
Zn(s) +
HCl(aq)
13.
Al(s)
HNO3(aq)
14.
Cu(s) +
+


HI(aq)
ACTIVE METALS: Li > K > Ba > Sr > Ca > Na

15.
Ca(s)
+
H2O(l)
16.
Na(s)
+
H2O(l) 
17.
Fe(s)
+
H2O(l)

COMBUSTION REACTIONS: CxHy + O2(g)

 H2O(g) + CO2(g)
CxHyOz + O2(g)

18.
C3H8(g) +
O2(g)

19.
C6H6O(l) +
O2(g)

20.
C2H2(g) +

O2(g) 



 H2O(g) + CO2(g)
21. For each of the following,
i. Identify the type of reaction using the letters designated below:
– Combination (C)
– Precipitation (P)
– Decomposition (D)
– Acid-Base Neutralization (N)
– Combustion (B)
– Single Replacement/Displacement (SR)
TYPE ii. Balance the equation
_____ a. _____ Mg(NO3)2(aq) + _____ K3PO4(aq)  _____ Mg3(PO4)2(s) + _____ KNO3(aq)
_____ b. _____ Ni(OH)3(s) + _____ HCl(aq)  _____ H2O(l) + _____ NiCl3(aq)

_____ c. _____ Al(HCO3)3(aq) 
 _____ CO2(g) + _____ H2O(g) + _____ Al2(CO3)3(s)
_____ d. _____ Fe(s) + _____ Pb(NO3)2(aq)  _____ Pb(s) + _____ Fe(NO3)3(aq)
22. For each of the following sets of reactants, write the formulas for the products (including
physical states) and balance the equation if the reaction occurs, or write “NR” for no reaction.
a.
HClO4(aq)
b. 
HCl(aq)
c. 
Na2S(aq)
d. 
Zn(s) +
e.
Sr(s) +
+
+
Al(s)


MgCO3(s)
+
Fe(NO3)3(aq)
P4(s)



H2O(l)

Guidelines for Writing Net Ionic Equations
1. Balance the chemical/molecular equation.
2. Convert the molecular equation to total ionic equation
– Leave solids, liquids, gases, and weak acids and bases as compounds
– Show strong acids and all aqueous ionic compounds as ions in solution.
3. Cancel spectator ions to get net ionic equation
– If canceling spectator ions eliminates all ions  NO REACTION (NR)
– If coefficients can be simplified, do so to get the lowest ratio.
4. Make sure total charges on both sides of the equation are equal.
23. Write the net ionic equation for each of the following:
a. molecular:
Na2SO4(aq) +
Ba(NO3)2(aq) 
NaNO3(aq) +
BaSO4(s)
total
ionic
eq.:
net
ionic
eq.:
b. molecular:
KBr(aq) +
Cu(NO3)2(aq) 
CuBr2(aq) +
KNO3(aq)
total
ionic
eq.:
net
ionic
eq.:
c. molecular:
HNO3(aq) +
Ba(OH)2(aq) 
total
ionic
eq.:
net
ionic
eq.:
d. molecular:
H2SO4(aq) +
KOH(aq) 
total
ionic
eq.:
net
ionic
eq.:
e. molecular:
total
ionic
eq.:
net
ionic
eq.:
Mg(s) +
Al(NO3)3(aq) 
H2O(l) +
Ba(NO3)2(aq)