Download Balancing Reactions 1

Balancing Reactions 1
1. Write equations for the ionization of the following acids.
a. Hydrochloric acid
b. Nitric acid
c. Chloric acid
2. Write equations for the ionization of the following acids. Which ones ionize only
slightly?
a. HF
b. H2SO3
c. CH3COOH
d. HNO3
3. Classify each substance as either a strong or weak electrolyte:
a. NaCl
j. Ba(OH)2
b. MgSO4
k. LiOH
c. HCl
l. C2H5COOH
d. H2C2O4
m. NH3
e. Ba(NO3)2
n. KOH
f. H3PO4
o. Mg(CH3COO)2
g. CsOH
p. HCN
h. HNO3
q. HClO4
i. HI
4. Assign Oxidation numbers to the element specified in each group of compounds.
a. N in:
i. NO
v. N2H4
ii. N2O3
vi. NH2OH
iii. N2O4
vii. HNO2
iv. NH3
viii. HNO3
b. Cr in:
i. CrO2-1
iii. CrO4-2
-1
ii. Cr(OH)4
iv. Cr2O7-2
5. Write balanced formula unit equations for the following redox reactions:
a. Aluminum reacts with sulfuric acid, H2SO4, to produce aluminum sulfate
and hydrogen.
b. Nitrogen reacts with hydrogen to form ammonia, NH3
c. Zinc sulfide, ZnS, reacts with oxygen to from zinc oxide and sulfur
dioxide
d. Carbon reacts with nitric acid to produce nitrogen dioxide carbon dioxide
and water.
e. Sulfuric acid reacts with hydrogen iodide to produce sulfur dioxide,
iodine, and water.
6. For question 5, write the total ionic equation and the net ionic equation.
a.
b.
c.
d.
e.
7. What is being oxidized and what are being reduced in question 6?
a.
b.
c.
d.
e.
8. What are your reducing agents and what are your oxidizing agents in question 6?
a.
b.
c.
d.
e.
9. Write the net ionic equation for the following reactions. Identify what is being
oxidized and what is being reduced.
a. Ni(s) +
Cl2(g) 
NiCl2(s)
b. 3Fe(NO3)2(aq) +
2Al(s) 
3Fe(s) +
c. Cl2(aq)
+
2NaI(aq)

2NaCl(aq) + I2(aq)
d. PbS(s)
+
4H2O2(aq)

PbSO4(s)
2Al(NO3)3(aq)
+
4H2O(l)