Formulas
pH = - log [H+]
pOH = - log [OH-]
pH + pOH = 14
K Unit 15 CFU
1.Write the names for the following acids.
a. HNO3__nitric acid__
b. HF __hydrofluoric acid_________
[H+] = 10-pH
[OH-] = 10-pOH
c. H2SO3 __sulfous acid_______
Formulas
d. H3N___hydronitric acid_____
p
2. Write the formulas for the following acids.
a. Hydroiodic acid__HI________
b. Hydrosulfuric acid__H2S ____
c. Sulfuric acid___H2SO4______
d. Nitrous acid __HNO2 ____
3. Phenophthalein is an indicator that turns pink when added to a basic solution. In which solution would
phenolphthalein turn pink?
a. NaCl
b. HBr
c. H2O
d. KOH
4. What is the range of pH values for each of the following solutions?
a. Acidic: __less than 7_____
b. Basic: __greater than 7_______
c. Neutral: __equal to 7____
5.
Which of the following solutions will cause litmus paper to turn blue?
a. NaOH
b. NaCl
c. HCl
d. H2O
6. Circle the most acidic pH in each of the following pairs.
a. 11 or 6.5
b. 7.0 or 3.5
c. 5.1 or 2.5
d. 3.0 or 9.0
7. Which solution is the least concentrated?
a. 10 M H2SO4
b. 2.0 M H2SO4
c. 0.3 M H2SO4
d. 6.5 M H2SO4
8. Define a Bronsted-Lowry base.
a. donates a proton (H+)
b. donates a hydroxide ion (OH-)
c. accepts a proton (H+)
d. accepts a hydroxide ion (OH-)
9.
A student records the pH values of three samples and is asked to predict the pH of a fourth sample.
The student is told that Sample Z is less acidic than Sample Y but more acidic than Sample W.
Which of the following is a valid conclusion about the pH of Sample Z?
a. It is less than 3.3.
b. It is between 3.3 and 5.2.
c. It is between 5.2 and 7.1.
d. It is greater than 7.1.
10. Calculate the pH for the following hydrogen ion concentrations [H+] and identify if it is Acid, Base, or Neutral.
a. [H+] = 4.17 x 10-10 __9.4_
b. [H+] = 3.7 x 10-2 ___1.4_________
c. [H+] = 1.0 x 10-7 ___7.0_________
d. [H+] = 2.0 x 10-5 ___4.7_________
11. Write the formulas for the following bases.
a. Potassium hydroxide ___KOH_____ c. Magnesium hydroxide __Mg(OH)2__
b. Calcium hydroxide ___Ca(OH)2_____ d. Lithium hydroxide ___LiOH_____
12. Write the names for following bases.
a. Be(OH)2 __beryllium hydroxide__ c. Sr(OH)2 _strontium hydroxide___
d. RbOH __rubidium hydroxide_____
b. NaOH __sodium hydroxide___
13.Which of the following is an observable property of many acids? (CIRCLE ALL THAT APPLY)
a.
b.
c.
d.
They become slippery when reacting with water.
They react with metals to release hydrogen gas.
They react with carbonates to form CO2.
They combine with bases to neutralize and produce salt and water.
14. Which diagram represents a weak acid? (CIRCLE ALL THAT APPLY)
15. Letter d in the diagram above represents a strong acid because the acid…
a.
b.
c.
d.
Partially dissociates.
does not dissolve in water.
Completely dissociates.
does not conduct an electric current.
16. If a solution being tested is a weak base, what will happen when you plug in a conductivity tester?
a. The light bulb will remain unlit.
b. The light bulb will be dimly lit.
c. The light bulb will be brightly lit.
17. The apparatus below is best used for which purpose? ___titration_________
18. Which of the following is a binary acid? (CIRCLE ALL THAT APPLY)
a. HF
b. HNO2
c. HNO3
d. H3N
e. H2S
f. HCN
19. Which of the following is a polyprotic acid? (CIRCLE ALL THAT APPLY)
a. HBr
e. Ca(OH)2
b. H2S
f. H3N
c. H2SO4
e. HCl
d. KOH
f. HNO3
20. Calculate the molarity of a solution which has 6.3 moles of NaOH and a solution volume of 1.5 liters.
mol
6.3mole
M
M 
= 4.2 M NaOH
L
1 .5 L
21. A student has a 5.0 M solution of hydrochloric acid. He wants to dilute it and make 214 milliliters of
1.2 M hydrochloric acid. What volume of 5.0 M solution is needed?
M1V1=M2V2 (5M)(X) = (1.2M)(214mL) X= 51mL HCl
22. What process is shown in the diagram below?
a. Evaporation
b. A precipitation reaction
c. The dissociation of water
d. A neutralization reaction
23. Which of the following properties apply to bases? (CIRCLE ALL THAT APPLY)
a. Bitter taste
b. Sour taste
c. Feels slippery
d. turns litmus red
24. What does pH measure?
a. Base density
b. Hydroxide ion concentration
c. Acid density
d. Hydrogen ion concentration
25. According to the Arrhenius definition, an acid is a substance that ________________.
c. accepts a H+
d. accepts a (OH)-1
a. donates a H+
b. donates a (OH)-1
26. According to the Arrhenius definition, a base is a substance that ________________.
a. donates a H+
b. donates a (OH)-1
c. accepts a H+
d. accepts a (OH)-1
27. Complete and balance the equation for this acid-base reaction:
H2SO4(aq) + 2KOH(aq)
2H2O(l) + K2SO4(aq)
28. Find the hydroxide-ion concentration for the following:
a. pH = 6.0 __1 x 10-8______
b. pH = 9.0 __1 x 10-5__________
c. pH = 2.3 __1.995 x 10-12__________
d. pH = 8.7 ___5.012 x 10-6______
29. TRUE or FALSE Basic solutions have more hydroxide ions than hydronium ions.
30. Write the Bronsted Lowry equation for HClO3 and H2O. What are the names of the acid-conjugate base
pair?
HClO3(aq) + H2O(l)
H3O+(aq) + ClO3–(aq) chloric acid is the acid and the chlorate ion is the conjugate base
31. List where the following acids and bases are commonly found.
sulfuric acid - __car batteries_________
acetic acid - __vinegar____________
magnesium hydroxide - __laxative______
carbonic acid - __carbonated drinks/soda__________
hydrochloric acid - __gastric juice in stomach_______
ascorbic acid - _citrus fruit_______
ammonium hydroxide - ___window cleaner_____
32. In a titration experiment, if 53.2 mL of an HBr solution reacts with 42.9 mL of a 1.38-M KOH solution, what
is the concentration of the HBr solution?
+
(#H )(MA)(VA) = (#OH-)(MB)(VB)
(1)(x)(53.2mL) = (1)(1.38 M)(42.9mL) x=1.11M HBr
33. Determine the pOH in a 0.235 M LiOH solution.
M of a base is equal to the [OH-], so –log(.235) = 0.629