Name: __________________________________
Date: __________________
Class/Period: _____________________________
A Little Review . . .
Directions: Read each of the following questions carefully and answer in the space provided. If a question
requires a calculation, SHOW ALL WORK! No work, no credit, no kidding! Remember to use units and significant
figures where appropriate. Good luck!
Chemical Reactions
1. Fill in the blanks below with the name of one of the five types of chemical reactions: synthesis, decomposition,
single displacement, double displacement, and combustion.
a) one reactant breaks down into two or more products
____________________________
b) element + compound → element + compound
____________________________
c) hydrocarbon + oxygen → carbon dioxide + water
____________________________
d) two ions trade places with each other in compounds
____________________________
e) two or more substances make one product
____________________________
2. Identify the TYPE of chemical reaction below.
a) 2 H2 + O2 → 2 H2O
____________________________
b) 2 KIO3 → 2 KI + 3 O2
____________________________
c) Fe + CuSO4 → FeSO4 + Cu
____________________________
d) Li2SO4 + Pb(NO3)2 → 2 LiNO3 + PbSO4
____________________________
e) C3H8 + 5 O2 → 3 CO2 + 4 H2O
____________________________
The Mole and Mole Conversions
3. The SI unit used to measure an amount is a(n) ____________________.
4. What is molar mass? ___________________________________________________________________
5. Calculate the molar mass of:
a) CuSO4
________________
b) octane
6. a) ____________________ = 1 mole = ____________________
b) 6.02 x 1023 is called __________________________________.
________________
7. How many moles are in 315 grams of magnesium chloride?
___________
8. How many grams are in 7.6 moles of dinitrogen trioxide?
___________
9. How many atoms are in 8.40 moles of aluminum (Al)?
___________
10. How many molecules are in 88.0 grams of carbon dioxide?
___________
11. How many moles are in 7.05 x 1024 atoms of carbon (C)?
___________
12. How many grams are in 6.02 x 1023 formula units of LiCl?
___________
13. a) What is an empirical formula? _________________________________________________________
b) What is a molecular formula? __________________________________________________________
14. Compare the following formulas: C4O2H8 and C2OH4.
a) Which is the empirical formula? _________________ Why? _________________________________
b) Which is the molecular formula? _________________ Why? ________________________________
15. a) What is the empirical formula for C6H14? ____________________
b) What is the empirical formula for H2O2? ____________________
16. Explain how to find an empirical formula when given the percent composition of each element in the compound.
17. a) Determine the empirical formula for a compound containing 1.203% of calcium and 2.128% of chlorine.
b) A compound has the empirical formula CH2O. If its molar mass is 150 g/mol, what is the molecular formula
of the compound?
__________
Stoichiometry
18. a) What is stoichiometry? ______________________________________________________________
________________________________________________________________________________
b) Upon what is stoichiometry based? ______________________________________________
19. a) What is a mole ratio? _______________________________________________________________
b) Should a mole ratio ever be reduced? __________ Explain why or why not. ______________________
________________________________________________________________________________
20. Use the chemical reaction below to answer the following questions.
4 FeCl3 + 3 O2 → 2 Fe2O3 + 6 Cl2
a) What is the mole ratio between iron (III) chloride and chlorine in the equation below? _______________
b) What is the mole ratio between chlorine and oxygen? ______________________
21. Balance the equation below, and then use it to answer the following questions.
___ LiOH + ___ PbSO4 → ___ Pb(OH)2 + ___ Li2SO4
a) How many moles of Pb(OH)2 will be produced from 3.0 moles of LiOH assuming you have an excess of PbSO4.
___________
b) If you need to make 750 g of Pb(OH)2, how many moles of LiOH would you need?
___________
c) What mass (in grams) of Li2SO4 will be produced with 72.0 grams of LiOH?
___________
d) What mass (in grams) of PbSO4 is required to make 4.00 moles of Li2SO4?
___________
Limiting and Excess Reactant Stoichiometry
22. a) What is a limiting reactant? __________________________________________________________
b) What is an excess reactant? __________________________________________________________
23. You are making one ham sandwich at home for lunch. The recipe requires that you have 3 slices of ham, 2
pieces of bread, 2 pieces of Swiss cheese, and 1 tablespoon of mayonnaise. You find that you have 9 slices of
ham, 4 slices of bread, 2 pieces of Swiss cheese, and 10 tablespoons of mayonnaise. Which ingredient would
be the limiting reactant?
___________
24. Examine the general chemical reaction below, and use it to answer the question that follows.
3A + B → C
If you have 9 moles of A and 5 moles of B, which would be the limiting reactant?
___________
25. Examine the general chemical reaction below, and use it to answer the question that follows.
X2 + 2 Y → 2 XY
If you have 7 moles of X2 and 8 moles of Y, which would be the limiting reactant?
___________
Solutions
26. What is a solution? ___________________________________________________________________
27. a) What is a solute? __________________________________________________________________
b) What is a solvent? __________________________________________________________________
28. You have a 25% aqueous solution of potassium bromide. Identify the solute and solvent.
Solute: ___________________
Solvent: __________________
29. a) What substance is nicknamed the “universal solvent”? _______________________
b) Why is this substance given this nickname? _______________________________________________
________________________________________________________________________________
________________________________________________________________________________
________________________________________________________________________________
30. a) Explain the phrase “like dissolves like” using the words polar and nonpolar. ________________________
________________________________________________________________________________
________________________________________________________________________________
b) Explain why oil and water do not mix to form a solution. ______________________________________
________________________________________________________________________________
________________________________________________________________________________
31. a) Ionic solutes dissolve best in which type of solvent: ionic or covalent? _________________
b) Covalent solutes dissolve best in which type of solvent: ionic or covalent? _______________
c) Would sodium chloride dissolve best in water or hexane? __________________
d) Would carbon tetrachloride dissolve best in water or hexane? ______________
32. The three main types of solutions are saturated, unsaturated, and supersaturated. Use the description below
to identify the type of solution described.
a) To which type of solution could you add more solute to it and have it dissolve simply by agitating it?
_________________
b) Which type of solution will have some solute remaining unchanged at the bottom of the container?
_________________
c) Which type of solution dissolves more than the maximum amount of solute by increasing temperature?
_________________
33. Use the graph below to answer the following questions.
Solubility as a Function of Temperature
a) How much KCl dissolves in 100 g of water at 80C?
_______________
b) 90 g of NH4Cl dissolves at 90C in 100 g of water. Is
this solution saturated, unsaturated, or supersaturated?
_______________
c) Which of the solutes on the graph behave as gases?
_______________
d) At 80C, a saturated solution of potassium chlorate is
made. If the solution cools to 30C, how much solute will
precipitate out?
_______________
e) How much cerium sulfate will dissolve in 300. g of water
at 20C?
________________
34. What is the molarity of a solution containing 6.0 moles of solute dissolved in 2.00 L of solution? __________
35. What volume of solution is needed to make a 3.0 M solution containing 109.5 g of HCl?
___________
36. a) What is a colligative property? ________________________________________________________
________________________________________________________________________________
b) Label whether the following increase or decrease when a solute is added to a pure solvent:
i. Freezing point
_____________________________
ii. Boiling point
_____________________________
iii. Vapor pressure
_____________________________
Acids and Bases
37. List three physical properties of an acid and one chemical property.
physical property: _________________________________________________
physical property: _________________________________________________
physical property: _________________________________________________
chemical property: _________________________________________________
38. List three physical properties of a base and one chemical property.
physical property: _________________________________________________
physical property: _________________________________________________
physical property: _________________________________________________
chemical property: _________________________________________________
39. a) Distinguish between a strong acid and a weak acid.
b) Distinguish between a strong base and a weak base.
40. Compare and Contrast an Arrhenius acid and base and a Bronsted-Lowry acid and base by filling in the chart
below.
Acid
Base
Arrhenius Definition
Bronsted-Lowry Definition
41. Read the reaction below from left to right. Identify the acid, base, and conjugate acid (CA) and conjugate
base (CB).
HCl
_____
+
NH3
_____
↔
NH4+
_____
+
Cl-
_____
42. Examine the description below and determine whether it describes a strong acid, weak acid, strong base, or
weak base.
a) dissociates completely (~100%) and turns blue litmus red
___________
b) partially dissociates, stays clear in phenolphthalein, orange on pH paper
___________
c) dissociates completely (~100%) into OH- ions
___________
d) dimly lights up conductivity apparatus (light bulb) and turns pink in phenolphthalein
___________
e) brightly lights up conductivity apparatus (light bulb) and has a pH of 2.1
___________
f) dissociates completely (~100%) into H+ ions
___________
g) dimly lights up conductivity apparatus (light bulb) and turns red litmus blue
___________
h) dissociates completely (~100%), turns red litmus blue, and has a pH of 12.9
___________
43. a) What type of double displacement reaction occurs when an acid reacts with a base? _________________
b) What are ALWAYS the two products when an acid reacts with a base? ___________ and ____________
44. If you spilled oven cleaner containing sodium hydroxide on the kitchen counter, what could be used to
“counteract” this spill? ___________________________
45. A flask contains 1 L of 5 M Mg(OH)2. Which of the following would completely “counteract” this solution?
a) 1 L of 5 M HCl
b) 1 L of 5 M Mg(OH)2
c) 0.5 L of 2.5 M HCl
d) 0.5 L of 2.5 M Mg(OH)2
46. Draw the pH scale from 0 to 14 and label the acidic, basic, and neutral pH’s.
47. What is another word for a basic solution? ________________________