Acids and Bases
Chapter 8 Acids and Bases
This section lists the properties of acids and bases. It also explains how to name an
acid or base when given the formula.
1. Circle the letters of all the terms that complete the sentence correctly.
The properties of acids include ______.
a. reacting with metals to produce oxygen
b. giving foods a sour taste
c. forming solutions that conduct electricity
d. causing indicators to change color
2. Is the following sentence true or false? Acids react with compounds containing
hydroxide ions to form water and a salt. _____________________
3. Bases are compounds that react with acids to form __________ and a(n)
____________________.
4. Circle the letters of all the terms that complete the sentence correctly.
The properties of bases include ______.
a. tasting bitter
b. feeling slippery
c. changing the color of an indicator
d. always acting as a strong electrolyte
Names and Formulas of Acids and Bases (pages 578-579)
5. What is an acid?
6. When the name of an anion in an acid ends in -ide, the acid name begins with the prefix
_____________________.
7. Give the general form of the chemical formula of an acid and tell what the letters in the formula
stand for. ____________________________________
H. Cannon, C. Clapper and T. Guillot
Klein High School
Acids and Bases
Acids and Bases (continued)
8. Complete this table of anion and the acids they can form.
9. Is the following sentence true or false? The rules for naming acids cannot be used in reverse to
write the formulas of acids from their names.______________.
10. A base is a compound that produces __________dissolved in water
11. How do you write the formula for bases?
Hydrogen Ions and Acidity
This section classifies solutions as neutral, acidic, or basic, given the hydrogen-ion or hydroxide-ion
concentration. It explains how to convert hydrogen-ion concentrations into pH values and hydroxideion concentrations into pOH values.
Hydrogen Ions from Water
1. What does a water molecule that loses a hydrogen ion become?
2. What does a water molecule that gains a hydrogen ion become?
3. The reaction in which two water molecules produce ions is called
the___________ of water.
4. In water or aqueous solution,___________ are always joined to as
hydronium ions(H3O)
5. Is the following sentence true or false? Any aqueous solution in which [H'] and
[OH ] are equal is described as a neutral solution.
____________________
8-2
HC/CC/TG KHS
Acids and Bases
1. Which definition of acids and bases is solvent dependent? What is the
required solvent?
2. What is another term that describes a hydrogen ion?
3. Write the equation, with the correct formulas, for the production of the
hydronium ion.
4. What is the relationship between an acid-conjugate base or a baseconjugate acid?
Identify the acid, base, conjugate acid, and conjugate base.
5. H2SO3 + OH- Å Æ HSO3- + H2 O
6. HSO3- + OH-
Å Æ S03- +
H2O
7. HCHO2 + H2O Å Æ CHO2- + H3O+
8. C5 H5 N + H2O Å Æ C5 H5 NH+ + OH-
Write the conjugate of the following:
12. ClO-
9. NH4+
`
10. OH-
13. HCl
11. H30+
14. H2O
15. Write the conjugate acid and the conjugate base of HS-
8-3
HC/CC/TG KHS
Acids and Bases
16. Is the following sentence true or false? Most pH values are whole numbers.
17. If [H+] is written in scientific notation but its coefficient is not 1, what do you need to
calculate pH?
18. Is the following sentence true or false? You can calculate the hydrogen-ion concentration
of a solution if you know the pH.
____________________
19. When do you use indicators and when do you use a pH meter to measure pH?
20. Why is an indicator a valuable tool for measuring pH?
21. Why do you need many different indicators to span the entire pH spectrum?
22. Look at the figure below. Fill in the missing pH color change ranges
for the indicators.
23. A pH meter uses a combination electrode connected to a millivoltmeter.
What two electrodes make up this combination electrode?
8-4
HC/CC/TG KHS
Acids and Bases
Acids and Bases
1. Define or explain the following theories about acids and bases.
a. Arrhenius Theory _____________________
________________________________
b. Bronsted-Lowry Theory __________________
________________________________
2. What term describes an acid, base, or salt, which, when dissolved in water,
conducts electric current?
3. What is the polyatomic ion, H3O+, which is formed when a hydrogen ion (H+)
combines with a water molecule?
4. The _____________ of an acid is the particle that remains after a proton has been
released by the acid.
5. The ___________ of a base is formed when the base acquires a proton from the
acid.
6. Which type of acid contains only two elements?
7. What do we call an acid that contains three or more elements ?
8. What type of substance is one that can react as either an acid or a base?
9. What is the most common example of the above type of compound?
Match the following terms with the correct description.
_____
10. a base that dissociates completely in
solution
_____
11. an oxide that produces an acid when
dissolved in water
_____
12. an acid that ionizes completely in
solution
_____
13. an oxide that produces a base when
dissolved in water
_____
14. an acid that dissociates slightly when
in solution
_____
15. a base that only partially dissociates in
solution
A. weak acid
B. weak base
C. strong acid
D. weak acid
E. acidic anhydride
F. basic anhydride
8-5
HC/CC/TG KHS
Acids and Bases
Name the following binary acids:
a. HF
b. HCl
c. HI
d. H2S
e. H3N
f. HBr
16. Name the following ternary acids and bases:
a. H3AsO4
b. H3AsO3
c. NaOH
d. H3BO3
e. H3PO4
f. H3PO3
g. HNO3
17. Write the formula for the conjugate base of each of the acids below:
a. H2O
b. HNO3
c. HF
d. HC2H3O2
8-6
HC/CC/TG KHS
Acids and Bases
Acid/Base Quest
18. Write the formula for the conjugate acid of each of
the following bases listed:
a. NH3
b. HSO4c. HSd. C2H5NH
19. Classify each of the following as a strong acid, strong base, weak acid or weak
base:
a. NaOH
b. HCl
c. NH4+
d. NH3
e. Clf. HI
21. Identify the Bronsted acids and bases in the following reaction.
H2SO4 + H2O Å Æ HSO4- + H3O
20.
Write the formulas for the anhydrides of the following:
a. H2CO3
b. H2SO3
c. H2SO4
d. NaOH
e. Ca(OH)2
f. HNO3
8-7
HC/CC/TG KHS
Acids and Bases
1. How many ml of .085M NaOH are needed to neutralize 25.Oml
of .15M HCl?
2. How many ml of 1.25M KOH are needed to neutralize 5O.Oml
of .50M HCl?
3. How many ml of .25M LiOH are needed to neutralize 25.Oml
of .1OM H2SO4?
4. How many ml of .18M A1 (OH) 3 are needed to neutralize 25.0ml
of .25M HN03?
5. If 28mL of LiOH is used to neutralize 22m1 of .50M HBr, what is
the concentration (M) of the basic solution?
6. If 25.0ml of Ca(OH)2 is used to neutralize 35ml of 1.0M HCl,
what is the concentration (M) of the basic solution?
7. If 15ml of A1 (OH)3 is used to neutralize 9.5ml of 2.5M HF,
what is the concentration (M) of the basic solution?
8. If it takes 28cm3 of .50M KOH to titrate 50.0cm3 of HCl to
the endpoint, what is the concentration of the HClsolution?
9. If it takes 75ml of 1.50M Ba(OH)2 to titrate 58.OmL of HBr to
the endpoint, what is the concentration of the HBr solution?
10. If it takes 45.0ml of 2.0M Al (OH)3 to titrate 60.0ml of H2S04 to
the endpoint, what is the concentration of the H2SO4 solution?
8-8
HC/CC/TG KHS
Acids and Bases
RELATIVE STRENGTHS OF ACIDS AND BASES
1. The concentration of a 200ml boric acid solution is .8m. How many moles
of acid are in this solution? How many grams of boric acid is this?
2. A volume of 20ml of an aqueous solution of strontium hydroxide has a
drop of indicator added to it. The solution turns color after 25bil of a
standard .05m hydrofluoric acid is added. What was the original
concentration of the strontium solution, and how many grams of the base
were dissolved in the 20ml sample?
3. A solution whose volume is 500ml is made by dissolving sulfuric acid made
by dissolving sulfuric acid in water. What is the normal concentration of the
solution?
4. A 240ml solution of standard .2n hydrofluoric acid completely neutralizes
a 100ml solution of sodium hydroxide of unknown concentration. What is the
normal concentration of the sodium hydroxide solution?
5. If 25ml of a .1M potassium hydroxide solution are required to neutralize
15ml of a solution of hydrobromic acid (a) What is the molarity of the acid?
(b) how many grams of hydrobromic acid and dissolved in 15ml of acid?
6. A standard solution of sulfuric acid has 15g of solute dissolved in 200ml
of solution. If it is used to titrate a potassium hydroxide solution producing
potassium sulfate as a salt product. What is the molarity of the base if
35ml of it are neutralized by 15ml of the acid?
7. How many grams of solute are there in 35ml of solution if calcium
hydroxide that can be completely neutralized by 15ml of .1M sulfuric acid?
8. What is the molarity of a solution of HCl if 25ml are titrated to an end
point by 10ml of a .2M solution of NaOH? How many grams of HCl are there
in the 25ml of HCl solution?
8-9
HC/CC/TG KHS
Acids and Bases
PURPOSE: To test various solutions with different Indicators to
determine the approximate pH, and to develop a table of the
comparative strengths of these acid solutions.
PROCEDURE: 1. Place one dropper-full of each solution listed in the
Data Table into separate test tubes. To each tube, add
one drop of an indicator. Hold the tubes against a white
background and observe the color in each.
2. Repeat with each of the other indicators.
3. After studying your results with each set of solutions
and comparing against the Table of Indicator Colors,
TABLE OF INDICATORS
Methyl Orange
Methyl Red
Bromthymol Blue
Phenolphthalein
Indicator Colors
Acid Color
pH
Transition Color
red-orange 3.2
orange
pink
4.8
orange
yellow
5.0
green
colorless
8.2
pink
pH
4.4
6.0
7.6
10.6
Base Color
yellow
yellow
blue
purple
DATA TABLE
List solutions in order of decreasing strength:
10
HC/CC/TG KHS
Acids and Bases
11
HC/CC/TG KHS
Acids and Bases
PH Problems
1. Find the pH of solutions with the following H+ concentrations.
a.l.80x10 –3M
b.5.69xlO-'°M
..
c. 6.71 x l0-6M
d. 9.47 x l0-6M
2. Find the H+ concentration of the following solutions.
a.pH=3.7
b.pH-10.64
c.pH-6.83
d.pH-2.95
e.pH=9.65
3. Determine the pH of solution with the following OH contrations
a. 7.134 X 10-13M
b. 1,37 X 10 –8M
c. 11.62 X 10-10M
d. 0.32 X 10-2M
4. How many cm3of 0.0947M NaOH are needed to neutralize 21.4 cm3
of 0.106M HCl?
5. A titration of a 25.0ml sample of a HCl solution of unknown
molarity reaches the equivalence point when 38.28ml of a 0.4370M
NaOH solution has been added. What is the molarity of the HCl
solution?
6. A student titrates a 20.0ml sample of a solution of HBr with
unknown molarity. The titration requires 25.05ml of a 0.1819M
solution of NaOH. What is the molarity of the HBr solution?
7. A 50.0ml sample of a sodium hydroxide solution is
titrated with a 1.605M solution of sulfuric acid. The titration requires
24.09ml of the acid solution to reach the equivalence point?
12
HC/CC/TG KHS
Acids and Bases
pH/pOH Problems
Find the pH of solution with the following hydrogen ion
concentrations
1. 1.00X 10 –3M
2.1.00 X 10-6M
3.6.49 X 10 –10M
4.7.01 X 10-6M
5.9.47 X 10-8M
6.6.89 X 10 –14M
Find the hydrogen ion concentration of the following solutions
7. pH = 3.000
8. pH = 10.000
9. pH = 6.607
10. pH= 2.523
11. pH= 6.149
12. pH = 7.662
Find the pOH of the following solutions
13. pOH = 2.00
14. pOH = 7.00
15. pOH = 1.23
16. pOH = 1.263
17. pOH = 4.976
18. pOH = 9.714
19. pOH = 3.004
13
HC/CC/TG KHS