Name: ____________________________
Northwest Vista College
Chem 1311 - General Chemistry I
Spring 2012
Practice- Chapter 4 (25 pts)
Please write legibly. Show your work to get full credit, when appropriate!
1. (2 pts) Identify each of the following substances as a strong electrolyte, weak electrolyte, or
nonelectrolyte:
a) H2O
b) KCl
c) CH3COOH
d) C12H22O11
2. (1 pts) Characterize the following compounds as soluble or insoluble in water:
a) Ca3(PO4)2
b) Mn(OH)2
c) AgClO3
d) K2S
3. (3 pts) Write ionic & net ionic equations for the following reactions, include state labels:
a) AgNO3 (aq) + Na2SO4 (aq) 
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b) BaCl2 (aq) + ZnSO4 (aq) 
c) (NH4)2CO3 (aq) + CaCl2 (aq) 
4. (1 pts) Identify each of the following species as a Brønsted acid, base, or both:
a) HI
b) CH3COOc) H2PO4d) HSO4-
5. (3 pts) Balance the following equations and write the corresponding net ionic equations (if
appropriate):
(HBr is a strong acid)
a)
____ HBr (aq) + ____ NH3 (aq) 
(Ba(OH)2 is a strong base)
(H3PO4 is a weak acid)
(Mg(ClO4)2 is soluble)
b) ____ Ba(OH)2 (aq) + ____ H3PO4 (aq) 
c) ____ HClO4 (aq) + _____ Mg(OH)2 (s) 
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6. (4 pts) For the complete redox reactions given here, (i) break down each reaction into its
half-reactions; (ii) identify the oxidizing agent; (iii) identify the reducing agent.
a) 2Sr + O2 2SrO
b) 2Li + H2  2LiH
c) 2Cs + Br2  2CsBr
d) 3Mg + N2  Mg3N2
7. (3 pts) Give the oxidation number of the underlined atoms in the following molecules & ions:
a) ClF
g)
NaHCO3
b) IF7
h)
Li2
c) CH4
i)
NaIO3
d) K2CrO4
j)
KO2
e) K2Cr2O7
k)
PF6-
f) KMnO4
l)
KAuCl4
8. (1 pts) Calculate the mass of KI in grams required to prepare 5.00 x 10 2 mL of 2.80 M
solution.
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9. (1 pts) How many moles of MgCl2 are present in 60.0 mL of 0.100 M MgCl2 solution?
10. (2 pts) Calculate the molarity of each of the following solutions:
a) 29.0 g of ethanol (C2H5OH) in 545 mL of solution
b) 9.00 g of sodium chloride (NaCl) in 86.4 mL of solution
11. (1 pts) How would you prepare 60.0 mL of 0.200 M HNO3 from a stock solution of 4.00 M
HNO3?
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12. (1 pts) How many grams of NaCl are required to precipitate most of the Ag+ ions from 2.50
x 102 mL of 0.0113 M AgNO3 solution? Write the net ionic equation for the reaction.
13. (1 pts) A quantity of 18.68 mL of KOH solution is needed to neutralize 0.4218 g of KHP.
What is the concentration (in molarity) of the KOH solution?
(KHP - potassium hydrogen phthalate, KHC8H4O4)
14. (1 pts) Iron(II) can be oxidized by an acidic K2Cr2O7 solution according to the net ionic
equation:
Cr2O72- + 6Fe2+ + 14H+  2Cr3+ + 6Fe3+ + 7H2O
If it takes 26.0 mL o 0.0250 M K2Cr2O7 to titrate 25 mL of a solution containing Fe2+, what is
the molar concentration of Fe2+?
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