1. Acid/Base Review
Honors Chemistry

2. What is the name of H2SO3?
Hyposulfuric acid
Hydrosulfuric acid
Sulfuric acid
Sulfurous acid
Hydrosulfite acid

3. What is the property of a base?
Bitter taste
Watery feel
Strong color
Unreactive
nonelectrolyte

4. What is the charge on the hydronium ion?2- 1- 1+ 2+

5. If the hydroxide ion concentration is 10-10M, what is the pH of the solution?4 7 10 14

6. If the pH is 9, what is the concentration of hydroxide ion?
10-1 M
10-5 M
10-7 M
10-8 M
10-14M

7. How many free hydrogen ions are there in one liter of water?
None, they are all hydrated
Approximately 10-7 mol
Approximately 10-1 mol
Approximately 100 mol

8. A liter of impure water has 10-4 mol of hydroxide ions
A liter of impure water has 10-4 mol of hydroxide ions. What is the concentration of hydronium ions in this sample of water?
10 -4 M M
10 –7 M
No determination can be made from the information given

9. What is the concentration of hydronium ions in a neutral solution
No determination can be made from the information given

10. For a solution to be classified as acidic, the …
hydrogen-ion concentration must be M.
hydrogen-ion and hydroxide-ion concentration must be equal
hydrogen-ion concentration must be greater that the hydroxide-ion concentration
hydrogen-ion concentration must be 7M or greater

11. A solution in which the hydroxide-ion concentration is 1 x 10 –4 M is_________?
Acidic
Basic
Neutral
None of the above

12. Which of these solutions is the most basic?
[H +]= 1 x 10 –2 M
[OH –] = 1 x 10 –4 M
[H +] =1 x 10 –11 M
[OH –] = 1 x 10 –13 M

13. In a neutral solution, the [H+] is ___?
10-14 M
Zero
1 x 107 M
Equal to [OH-]

14. What is the pH when the hydrogen ion concentration is 7.0 x 10 –3 M
1.9
2.2 3 4

15. An indicator is what type of compound?
Oxidizing agent
Weak base or acid
Strong base or acid
Salt
Reducing agent

16. What is an acid according to Arrhenius?
A substance that ionizes to yield protons in aqueous solutions
A substance that is a hydrogen ion donor
A substance that accepts an electron pair
A substance that is a hydrogen ion acceptor
A substance that donates an electron pair

17. Which of these is an Arrhenius base?
LiOH
NH3
H2PO4-
HC2H3O2

18. What is transferred between a conjugate acid-base pair?
An electron
A proton
A hydroxide ion
A hydronium ion

19. What is the term used to describe a substance that can be both an acid and a base?
amphoteric
amphoprotric
Bronsted acid / base
Arrhenius acid / base

20. In the reaction, NH4+ + H20  NH4 + H30+, water behaves as a(n)
Arrhenius acid
Arrhenius base
Bronsted-Lowry acid
Bronsted-Lowry base

21. In the reaction, CO32- + H20  HC03- + OH-, the carbonate ion behaves as a(n)
Arrhenius acid
Arrhenius base
Bronsted-Lowry acid
Bronsted-Lowry base

22. Which of the following represents a Bronsted-Lowry conjugate acid- base pair?
SO32- and SO2
CO32- and CO
H30 and H2
NH4+ and NH3

23. What is an acid, according to Lewis?
A substance that ionizes to yield protons in aqueous solution
A substance that is a hydrogen ion donor
A substance that accepts an electron pair
A substance that is a hydrogen ion acceptor
A substance that donates an electron pair

24. What is the concentration of hydrochloric acid if 20
What is the concentration of hydrochloric acid if 20.0 ml of acid is neutralized by 30.0 ml of 0.20 N sodium hydroxide?
0.06M
0.14 M
0.30 M
0.60 M

25. How many milliliters of 0. 20N NaOH are required to neutralize 30
How many milliliters of 0.20N NaOH are required to neutralize 30.0 mL of 0.50N HCI?
12 mL
50 mL
75 mL
100 mL

26. How many grams of sodium hydroxide are in 500 mL of a 0
How many grams of sodium hydroxide are in 500 mL of a 0.1N NaOH solution?
2 g
4 g
20 g
40 g

27. What does a buffer do? Keeps the pH of a solution constant
Keeps the salt concentration of a solution constant
Keeps the sodium concentration constant
Keeps the chloride concentration constant