Chapter 20 Study Guide
Name ______Date ______Class ______
20.1
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
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.
20
8. Look at Table 20.1 on page 578. Use it to help you complete this table of anions and the acids they form.
Formula of Anion / Name of AcidS–2
SO3–2
SO4–2
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 ______ions when dissolved in water.
11. How do you write the formula for bases?
Name ______Date ______Class ______
20.2
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. ______
6. What is the ion-product constant for water (Kw )? Give the definition, the expression, and the value.
7. A(n) ______solution is one in which [H + ] is greater than [OH – ]. A(n) ______solution is one in which [H + ] is less than [OH – ].
8. Match the type of solution with its hydrogen-ion concentration.
______acidic a. less than 1.0x10 –7 M
______neutral b. greater than 1.0x10 –7 M
______basic c. 1.0x10 –7 M
9. The ______of a solution is the negative logarithm of the hydrogen-ion concentration.
10. Match the type of solution with its pH.
______acidic a. pH 7.0
______neutral b. pH =7.0
______basic c. pH 7.0
11. Look at Table 20.2 on page 584. What is the [H + ], the [OH – ], and the pH of washing soda?
12. The pOH of a solution is the negative logarithm of the ______concentration.
13. What is the pOH of a neutral solution? ______
14. If you are making pH calculations, how should you express the hydrogen-ion concentration?
15. Is the following sentence true or false? Most pH values are whole numbers.______
16. If [H + ] is written in scientific notation but its coefficient is not 1, what do you need to calculate pH?
17. Is the following sentence true or false? You can calculate the hydrogen-ion concentration of a solution if you know the pH. ______
18. When do you use indicators and when do you use a pH meter to measure pH?
19. Why is an indicator a valuable tool for measuring pH?
20. Why do you need many different indicators to span the entire pH spectrum?
Name ______Date ______Class ______
20.2 (Continued)
21. A pH meter uses a combination electrode connected to a millivoltmeter. What two electrodes make up this combination electrode?
22. List three characteristics that limit the usefulness of indicators.
23. Complete the paragraph with the steps you would use to measure the pH of a solution with a pH meter.
First, ______the meter by immersing its ______in a solution of a known pH. Adjust the readout of the ______to this known pH. Then, rinse the electrodes with ______. Finally, dip the electrodes into the solution of unknown ______
24. Is the following sentence true or false? Measurements of pH obtained with a pH meter are typically accurate to within 0.001 pH unit of the true pH. ______
20.3
1. Match the number of ionizable hydrogens with the type of acid.
______one a. diprotic
______two b. triprotic
______three c. monoprotic
2. Is the following sentence true or false? Only the hydrogens in weak polar bonds are ionizable. ______
3. Hydrogen is joined to a very ______element in a very polar bond.
4. Alkali metals react with water to produce ______solutions.
5. How do concentrated basic solutions differ from other basic solutions?
6. How does the Brønsted-Lowry theory define acids and bases?
7. Is the following sentence true or false? Some of the acids and bases included in the Arrhenius theory are not acids and bases according to the Brønsted-Lowry theory. ______
8. Is the following sentence true or false? A conjugate acid is formed when a base gains a hydrogen ion.____
9. A conjugate ______is the particle that remains when an acid has donated a hydrogen ion.
10. What is a conjugate acid-base pair? ______
11. A substance that can act as both an acid and a base is said to be______.
12. In a reaction with HCl, is water an acid or a base?
13. What is a Lewis acid? ______
14. A Lewis base is a substance that can ______a pair of electrons to form a covalent bond.
15. Is the following sentence true or false? All the acids and bases included in the Brønsted-Lowry theory are also acids and bases according to the Lewis theory.______
Name ______Date ______Class ______
20.4
1. What factor is used to classify acids as strong or weak?
2. Strong acids are ______ionized in aqueous solution; weak acids ionize ______in aqueous solution.
3. Look at Table 20.7 on page 600.
Which acid is the weakest acid in the table?
Which base is the weakest base?
4. What do you use to write the equilibrium-constant expression?
5. An acid dissociation constant (Ka ) is the ratio of the concentration of the ______form of an acid to the concentration of the______form.
6. What is another name for dissociation constants?
7. Is the following sentence true or false? The stronger an acid is, the smaller its Ka value. ______
8. A diprotic acid has ______dissociation constants.
9. Look at Table 20.8 on page 602. What is the second dissociation constant for the triprotic phosphoric acid?
10. Weak bases react with water to form the hydroxide ion and the ______of the base.
11. A base dissociation constant (Kb ) is the ratio of the concentration of the ______times the concentration of the hydroxide ion to the concentration of the ______.
12. What does the magnitude of the base dissociation constant (Kb ) indicate?
13. The words concentrated and dilute indicate how much acid or base is ______in solution.
14. Is the following sentence true or false? The words strong or weak refer to the extent of ionization or dissociation of an acid or base. ______
15. Is the following sentence true or false? You can calculate the acid dissociation constant (Ka ) of a weak acid from experimental data. ______
16. To measure the equilibrium concentrations of all substances present at equilibrium for a weak acid, what two conditions must you know?