Name _____________
UNIT 9 (SOLUTIONS AND ACIDS AND BASES) PACKET
SOLUTION WORKSHEET A
1) What is the significance of the statement “like dissolves like”? What does “like” refer
to?
2) Distinguish between electrolyte and a nonelectrolyte. Distinguish between a weak
electrolyte and a strong electrolyte. Give an example of each.
3) Identify the solvent and the solute in vinegar, a dilute aqueous solution of acetic acid.
4) Why do the temperatures on
the graph only go from 0º C to
100º C ?
5) Which substance is most
soluble at 60º C ?
6) Which two substances have
the same solubility at 80º C ?
7) Which substance’s solubility
changes the most from 0º C to
100º C ?
8) Which substance’s solubility
changes the least from 0º C to
100º C ?
9) What is the solubility of
potassium nitrate at 90º C ?
10) At what temperature does
potassium iodide have a
solubility of 150 g/ 100 cm3
water ?
11) You have a solution of
sodium nitrate containing 140
g at 65º C. Is the solution
saturated, unsaturated, or
supersaturated ?
12) You have a solution of
potassium chlorate containing
4 g at 65º C. How many
additional grams of solute
must be added to it, to make
the solution saturated?
1.
2.
3.
4.
5.
Molarity Worksheet B
Calculate the molarity, M, of the following solutions:
a. 3.0 moles of NaCl are dissolved in 1 liter of solution.
b. 0.5 moles of MgF2 are dissolved in 2 liters of solution.
c. 3 moles of NaOH are dissolved in 0.25 liters of solution.
How many liters of a 4.0 M CaCl2 solution would contain 2 moles of CaCl2?
How many liters of a 0.5 M CaCl2 solution would contain 3.5 moles of CaCl2?
How many liters of a 2.5 M CaCl2 solution would contain 1.0 mole of CaCl2?
How many moles of KCl are there in 2 liters of a 3.0 M solution?
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Name _____________
6. What is the molarity, M, of a solution in which 116 grams of KF are dissolved in 2 liters
of solution?
7. How many grams of KF are in 2 liters of a 3.0 M solution of KF? What is the [CaF2(aq)]
of a solution when 39 g of CaF2 are dissolved in enough water to make 2200 mL of
solution? ([ ] is how chemists say concentration or molarity)
8. How many grams of NH3 are dissolved in 85 mL of a 0.75 M solution?
Concentration Worksheet C(Dilutions)
1. 25 mL of 5.6 M HCl are placed in a volumetric flask. The flask is filled to 250 mL with
water. What is the molarity of the new solution?
2. 5.6 mL of NaOH are added to a flask and the flask is filled with water to the 200 mL
mark. The concentration of the new solution is found to be .098 M. What was the initial
molarity of the solution before the dilution was completed?
3. A chemist has 300 mL of a 2.5 M KCl solution. The solution is diluted by adding 1.2 L
of water to the original volume. What is the [KCl] of the diluted solution?
4. A chemist has 2 liters of a 3.2 M hydrochloric acid solution. If the solution is left out in
the room and enough water evaporates so that there is only 1.2 liters of solution left, what
is the final molarity of this concentrated acid?
5. When a chemist adds 1.0 L of water to 3.0 liters of a 0.8 M HF solution, what is the new
concentration of the total HF solution?
6. How much water will a chemist need to add to 200 mL of a 3.3 M KCl solution if they
want to make a 1.0 M solution of KCl?
Acid-Base & pH Worksheet D
1. Listed below are some of the properties of acids and bases. Fill in the blanks with the
appropriate word, acids or bases:
a) _______ produce hydrogen ions (H+) in solution
b) _______ have a bitter taste
c) _______ produce hydroxide ions (OH-) ions
d) _______ react with bases to form salts
e) _______ have a sour taste
f) _______ have a slippery, soapy feel
g) ____ react with acids to form salts
h) _______ react with many metals
2. List 3 strong acids and explain why these acids are considered strong acids.
3. List 2 weak acids and explain why these acids are considered weak acids.
4. List 2 strong bases and explain why these bases are considered strong bases.
5. List 1 weak base and explain why it is considered a weak base.
6. Write a balanced equation for the dissociation (ionization) of the following acids and
bases in water. Then identify the acid, base, conjugate acid and conjugate base for each
equation.
a) HClO4
b) C2H3O2c) NH3
d) HSO4e) HCl
f) CO32-
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Name _____________
pH and pOH Worksheet E
Calculate the appropriate values for pH, pOH, hydronium ion and hydroxide ions in this table.
[H+] (Mol/L)
[OH-] (Mol/L)
pH
pOH
Acid, Base, or
neutral
1.34  10
-6
2.54  10
-10
2.6
5.9
2.76  10
-1
9.25 E -2
12.5
2.89
3.45 E -7
2.75 E -6
5.55
4.67 E -8
2.55 x 10
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14
1
7
Neutralization and Titration Worksheet F
1. When an acid and base neutralize each other, what two substances are formed?
2. Write and balance the neutralization reactions for the following
a. HBr + KOH

b. HCl + LiOH

c. HF
+ Ba(OH)2
d. H2SO4 + LiOH
e. H3PO4 + NaOH 
f. H2SO4 + Al(OH)3
g. H3PO4 + Mg(OH)2
h. Phosphoric acid + silver hydroxide
i. Nitric acid + Iron III hydroxide
j. Ammonia reacts with Sodium hydroxide
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3.
4.
5.
6.
Name _____________
When titrating an acid with a base, how do you see that you have reached the end of the
titration?
What indicator is clear in an acid and pink in a base?
A student pours exactly 26.9 mL of HCl acid of unknown molarity into a beaker. The
student then adds 2 drops of the indicator spelled correctly in question #4 above and
titrates the acid to neutrality using 43.7 mL of 0.13 M NaOH base.
a. Write and balance the neutralization reaction of the acid and base.
b. What is the molarity of the acid?
In a laboratory, you make a base by adding 75 grams of NaOH to 380 mL of water. Then
you titrate 15 mL of your base using a nitric acid (HNO3) that is 2.2 M.
a. Calculate the molarity of the NaOH base
b. How many mL of the 2.2 M HNO3 acid will be required to titrate the 15-mL of
base?
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