Acids, Bases and Salts Unit Plan
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Worksheets Quiz
1. Properties of Acids, Bases & Salts WS
1
2. Arrhenius, Bronsted
Acids, Ka and Strength. WS 2 1
3. Arrhenius, Bronsted
Bases, Kb and Strength WS 3
4. Acid & Base Reactions.
Amphiprotic. Acid Chart. WS 4 2
5. Leveling effect, Anhydrides
and Relationships. WS 5
6. Hydrolysis of Salts. Quiz. WS 6 3
7. Acid, Base & Salt
Reactions. Hydrolysis. WS 7 ClassifyingEverything
Activity
8. Yamada’s Indicator Lab.
Hydrolysis. WS 8 4
9. Ionization of Water, [H+]
& [
10. pH for Strong Acids and Bases.
Hydrolysis Quiz WS 9
11. pH Calculations for
Weak Acids. WS 10
5
12. Ka from pH for Weak Acids. WS 11
13. Indicators Lab.
14. Kbs from Kas for Weak Bases. WS 12 6
15. pH for Weak Bases pH [H+] [
16.Amphiprotic Ions- Kas and Kbs. WS
14 7
17. Titration Lab. Primary Standards. Acids Midtermreview Test
18. Titration Lab
19. Buffers & Indicators WS 15 8
20. Titration Curves. WS 16 9/10
21. Review #1 Web Site Review Sheet Quizmebc
22. Review #2 Practice Test # 1 Practice Test 2
23. Test
Text book Hebden Read
Unit IV
WS #1 Properties of Acids and Bases
1.
Add 1 drop of each solution to 1 drop of the acid-base indicator in a spot
plate. Record the colour in the data table below. Describe each solution as an
acid or base in the space provided. Write the acid colour and base colour in
the table below.
Indicator--> Phenolphthalein Litmus Bromothymol
Blue Acid or Base
Solution:
HCl Clear Red Yellow Acid
NaOH Pink Blue Blue Base
Vinegar Clear Red Yellow Acid
Ammonia
Pink Blue Blue Base
(NH3)
Lemon
Juice Clear Red Yellow Acid
Seven-up Clear Red Yellow Acid
Baking
Soda Pink Blue Blue Base
(NaHCO3)
Indicator Acid
Colour Base Colour
Phenolphthalein Clear Pink
Litmus Red Blue
Bromothymol
Blue Yellow Blue
Wash and dry your spot plate
before going on to step 2.
2. Wear safety goggles for this
experiment. Pour approximately 50 mL of 1 M HCl into a fleaker. Add one level
spoonful of Mg and cover with a plastic funnel. After 1 minute and not before
light the top of the funnel using a match. Write the equation for the reaction
below.
2HCl(aq)
+ Mg(s) →
H2(g) + MgCl2(aq)
Wash and dry your fleaker
before going on to step 3.
3.
Taste a lemon and describe the taste in one word Sour
4.
Taste some baking soda and describe the taste in one word. Bitter
6.
Test two drops of HCl for conductivity in a spot plate. Result: Good Conductor
Write an equation that accounts for the conductivity of HCl.
HCl → H+ +
Cl-
7.
Test two drops of NaOH for conductivity in a spot plate. Result: Good Conductor
Write
an equation that accounts for the conductivity of NaOH (dissociation).
NaOH → Na+ +
Clean, dry and put away the
spot plate
8. List five properties of acids that are in
your textbook.
Acids conduct electricity, taste sour, neutralize bases, change the color of indicators, and react with some metals to produce hydrogen.
9. List five properties of bases that are in
your textbook.
Bases conduct electricity, taste bitter, neutralize acids, change
the color of indicators, and feel slippery.
10.
Make some brief notes on the commercial acids: HCl and H2SO4 (p
112).
HCl
H2SO4
11.
Make some brief notes on the commercial base NaOH (p 114).
12.
Describe the difference between a concentrated and dilute acid (hint:
concentration refers to the molarity). Describe their relative conductivities.
Concentrated means relatively high molarity and dilute means relatively low molarity.
13.
Describe the difference between a strong and weak acid (p 121-124). Use two
examples and write equations to support your answer. Describe their relative
conductivities.
A strong acid completely ionizes and a weak acid partially ionizes.
14.
Describe a situation where a strong acid would have the same conductivity as a
weak acid (hint: think about concentration).
A weak acid could have a high molarity and the strong acid could have a low molarity.
Complete this worksheet for next period. Read pages 107-126
for homework.
WS #2 Conjugate Acid-Base Pairs
Complete
each acid reaction. Label each reactant or product as an acid or base. The
first on is done for you.
1. HCN
+ H2O ⇄ H3O+ + CN-
Acid Base Acid Base
2. H3C6O7
+ H2O ⇄ H2C6O7- + H3O+
acid base base acid
3. H3PO4 + H2O ⇄ H2PO4- + H3O+
acid base base acid
4. HF
+ H2O ⇄ F- + H3O+
acid base base acid
5. H2CO3 + H2O ⇄ HCO3- + H3O+
acid base base acid
6. NH4+ + H2O ⇄ NH3 + H3O+
acid base base acid
7. CH3COOH + H2O ⇄ CH3COO- + H3O+
acid base base acid
8. HCl + H2O → Cl- + H3O+
acid base base acid
9. HNO3 + H2O → H3O+ + NO3-
acid base acid
base
Write
the equilibrium expression (Ka) for the first seven above reactions.
10.
Ka = [H3O+] [ CN-] 14. Ka = [H3O+]
[HCO3-]
[HCN] [H2CO3]
11. Ka = [H3O+]
[H2C6O7-] 15. Ka = [H3O+]
[NH3]
[H3C6O7] [NH4+]
12.
Ka = [H3O+] [H2PO4-] 16. Ka = [H3O+]
[CH3COO-]
[H3PO4] [CH3COOH]
13.
Ka = [H3O+] [F-]
[HF]
17.
Which acids are strong? The six on the top of the
acid chart are strong.
18.
What does the term strong acid mean? They
complete ionization into ions. Such as:
HCl + H2O → Cl- + H3O+
19.
Why is it impossible to write an equilibrium expression for a strong acid? Ka = [H3O+] [Cl-]
[HCl] is equal
to zero and in math numbers divided by zero are undefined. [HCl]
20. Which acids are weak?
All acids listed on the acid chart below the top six.
23.
What does the term weak acid mean?
Incomplete ionization. Such as: HF + H2O ⇄ F- + H3O+
24.
Explain the difference between a strong and weak acid in terms of electrical
conductivity.
A strong acid is a good conductor. A weak acid conducts but not so good.
Acid Conjugate
Base Base Conjugate Acid
14. HNO2
NO2- 15. HCOO- HCOOH
16. HSO3- SO32- 17. IO3- HIO3
18. H2O2 HO2- 19. NH3 NH4+
20. HS- S2- 21. CH3COO- CH3COOH
22. H2O OH- 23. H2O H3O+
Define:
22. Bronsted acid- a proton donor
23.
Bronsted base- a proton acceptor
24.
Arrhenius acid- a substance that ionizes in water
to produce H+
25.
Arrhenius base- a substance that ionizes in water
to produce OH-
26.
List the six strong acids. HCLO4 HI HBr
HCl HNO3 H2SO4
27.
Rank the acids in order of decreasing strength.
HCl HSO4- H3PO4 HF H2CO3
H2S
28.
What would you rather drink vinegar or hydrochloric acid? Explain.
Vinegar. It is a weak acid and produces much less H30+
ion which is the corrosive part of an acid.
Making a
Universal Indicator Lab Activity
Mix
the following indicators in a 50 mL beaker. Stir with an eyedropper.
Yamada’s
Universal Indicator
5 drops thymol blue
8 drops methyl orange
5 drops phenolphthalein
10 drops bromothymol blue
20 drops of water
Part 1. In a spot plate add two
drops of each buffer solution to a cell. Add one drop of Yamada’s indicator to
each. Record each colour on another lab sheet by colouring the cell the same
colour. Make sure you are accurate because you will use this information for
future labs and projects.
<----------
Acid Strength Increases ------ Neutral
----Base Strength Increases ------->
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pH = 1 |
pH = 3 |
pH = 5 |
pH = 7 |
pH = 9 |
pH =11 |
pH
= 13 |
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