QUARTER 4 EXAM REVIEW – CHEMISTRY
June 2015
Chapter 12 – Solutions
1. What are the different types of solutions?
2. What do the terms solute and solvent mean?
3. How can you distinguish between suspensions, solutions, and colloids?
4. What is the Tyndall effect?
5. What makes a solution an electrolyte or a nonelectrolyte?
6. How can the rate of dissolving a solid in a liquid be increased? What about a gas in a
liquid?
7. What is meant by saturated, supersaturated, and unsaturated?
8. What is meant by the rule “like dissolves like”?
9. Be able to calculate molarity, molality and % concentration or solve for any missing
parts of the equation.
10. What is the difference between exothermic and endothermic reactions? Which one
has a positive heat of solution? A negative heat of solution? Which one increases the
temperature of a solution? Which one decreases the temperature of a solution?
11. What do miscible and immiscible mean?
12. What is the % by mass of a solution prepared by dissolving 1.35 mol of calcium
chloride in 550 mL of water?
13. What is the molarity of a solution prepared by dissolving 5.75 g of potassium iodide
in enough water to make 125 mL of solution?
14. How many grams of glucose (C6H12O6) will be dissolved in 500. mL of water to
make a solution that is 0.65 m glucose?
Chapter 13 – Ions in Aqueous Solutions
hydration
conductors
precipitation
nonelectrolyte
net ionic equation
dissociation
nonconductors
precipitate
spectator ions
strong vs. weak electrolyte
ionization
aqueous solution
electrolyte
ionic equation
hydronium ion
1. Write the equation for the dissolving of 0.75 mol of aluminum nitrate in water. How
many moles of each ion are produced? How many TOTAL moles of ions are
produced? What process is this called?
2. Write the equation(s) for the reaction between HCl and water. What is this process
called?
3. Use the solubility rules to decide if a substance is soluble or insoluble in water. Do
this for sodium nitrate, barium phosphate, and calcium sulfide.
4. Write the balanced equation, the ionic equation, and the net ionic equation for the
reaction between aqueous solutions of aluminum sulfate and barium chloride. Also
identify the spectator ions.
5. What is the boiling point elevation of a solution made by dissolving 35.0 g of glucose
in 250 mL of water? What is the new boiling point of the solution?
6. What is the freezing point depression of a solution made by dissolving 7.6 g of
sodium chloride in 100 mL of water? What is the new freezing point?
Chapter 14 – Acids and Bases
Arrhenius acid
Bronsted-Lowry base
conjugate acid
amphoteric
Arrhenius base
Lewis acid
conjugate base
salt
Bronsted-Lowry acid
Lewis base
neutralization
1. Be able to identify the type of acid or base involved in a reaction. What type of base
is involved in the following reaction? HCl + H2O  H3O+ + Cl-
2. Be able to label the Bronsted-Lowry acid, the Bronsted-Lowry base, the conjugate
acid, and the conjugate base for a reaction. Be able to identify acid-base pairs and
determine the direction the reaction is favored. Do so for the following equation:
H2 CO3 + H2O
HCO3- + H3O+
3. Be able to write the balanced equation, the ionic equation, and the net ionic equation
for a neutralization reaction. Also identify the spectator ions. Do so for the reaction
between sulfuric acid and aqueous sodium hydroxide.
4. Be able to write the conjugate base or acid of a substance. What is the conjugate
base of HCl? What is the conjugate acid of water?
5. Write the 2-step ionization for sulfurous acid?
6. Be able to write the formula of an acid when given its name and vice versa. Be able
to do the same for bases. Determine whether and acid is monoprotic, diprotic, or
triprotic and whether a base is monobasic, dibasic, or tribasic.
7. What are the main characteristics of acids and bases?
Chapter 15 – Acid-Base Titration and pH
self-ionization
titration
ionization constant (K)
neutral
standard solution
pOH
indicator
acid
end point
pH
transition interval
base
equivalence point
1. What are the pH and pOH values for acids, bases, and neutral substances?
2. What is the pH for each of the following solutions:
A. [H3O+] = 1 x 10-4 M
E. 0.04 M H2SO4
B. [H3O+] = 1 x 10-4 M
F. 0.05 M NaOH
C. [OH-] = 1 x 10-4 M
G. [OH-] = 2.56 x 10-11 M
D. 0.0025 M HCl
H. 0.02 M Ca(OH)2
3. Be able to determine if a substance is acidic, basic, or neutral when given its
hydronium or hydroxide concentration.
4. What is the concentration of hydronium and hydroxide in pure water at 25oC?
5. Determine the hydronium and hydroxide concentrations from the following values:
A. pH = 9
D pH = 3
B. pH = 6.4
E pOH = 4
C. pOH = 10
F. pOH = 3.6
6. If the hydronium ion concentration is 1.5 x 10-6 M, what is the hydroxide
concentration?
7. If 45.0 mL of 0.100 M HCl is used to neutralize 31.0 mL of barium hydroxide, what
is the molar concentration of the base?