ACID AND BASE QUIZ

1. There are three different theories of acid and base. According to the Arrhenius theory, the correct strong acids are ….
a. HBr and HF
b. HNO3 and HI
c. HOCl and HOCl2
d. HCOOH and HF
e. CH3COOH and H2SO4
2. Organic acids contain a carboxyl group— a group that contains an acidic hydrogen that can ionize. The formula for the carboxyl group is ….`
a. –NH2
b. –OH
c. –CH3
d. –OCH3
e. –COOH
3. From the following acids, the correct weak acids are ….
a. H2SO4, HI
b. HCl, HBr
c. HNO2, HF
d. HNO3,H2SO3
e. HClO4, HClO
4. Which of the following is the weakest acid?
a. HCl
b. HClO
c. HBr
d. HBrO
e. HI
5. Which of the following acids is a diprotic, weak acid?
a. carbonic acid
b. hydrochloric acid
c. perchloric acid
d. acetic acid
e. sulphuric acid
6. A base used in the manufacture of soap is ….
a. calcium hydroxide
b. sodium hydroxide
c. ammonia
d. zinc hydroxide
e. barium hydroxide
7. Of the following solution, … is turning blue litmus red.
a. orange juice
b. lemon juice
c. vinegar
d. ammonia
e. table salt
8. A common substance that contains acetic acid is ….
a. vinegar
b. ammonia water
c. salad oil
d. soap
e. table salt
9. Of the following, _____ is not a characteristic of an acid.
a. tasting sour
b. turning red litmus blue
c. turning blue litmus red
d. contain H atom in its formulae
e. producing hydrogen ions in solution
10. Of the following, _____ is not characteristic of a base.
a. turning red litmus blue
b. tasting bitter
c. producing hydroxide ions in solution
d. producing a solution with a pH < 7 11. When dissolved in water, salts …. a. are nonelectrolytes b. have a bitter taste c. are electrolytes d. release hydrogen ions e.release hydroxide ions 12. A base can be prepared by the reaction between …. a. an active nonmetal with water b. a gas with water c. a sulfide with water d. an active metal with water 13. Of the following, the property that most closely relates to acids is …. a. bitter taste b. contains hydroxide polyatomic ion c. sour taste d. salty taste 14. When an acid is dissolved in water, it usually forms …. a. hydrogen ions b. hydroxide ions c. no ions d. chloride ions e. simple molecules 15. The acid used in the storage battery in your car is …. a. nitric acid b. hydrochloric acid c. tartaric acid d. sulfuric acid e. acetic acid 16. The sour taste of lemons and limes is due to a substance called …. a. acetic acid b. citric acid c. hydrochloric acid d. carbonic acid e. oxalate acid 17. In the following reaction, … is a base. HClO4(aq)+KOH(aq) --> KClO4(aq)+H2O(l)
a. KOH
b. H2O
c. HClO4
d. KClO4
e. KClO4 and H2O
18. The conjugate base of acetic acid (CH3COOH) is ….
a. CH3COO-
b. CH3COOH2+
c. CH2COO2-
d. CHCOO3-
e. CCOOH2-
19. The conjugate acid of the weak base methylamine (CH3NH2) is ….
a. CH3N2-b. CH3NH-c. CH3NH3+d. CH3NH3-e. CH3NH42+
20. Hydrazine (N2H4), formerly used as a rocket fuel, is a base. What is its conjugate acid?
a. N2H4- d. N2H5+ b. N2H3+ e. N2H5 c. N2H5-
21. In terms of base strength, OH- is … CH3COO-.
a. stronger than
b. weaker than
c. the same as
d. different with
e. similar with
22. Which definition of an acid is more restrictive? In other words, which definition includes fewer substances in its definition of an acid?
a. Lewis
b. Arrhenius
c. Brønsted-Lowry
d. Arrhenius and Lewis
e. Arrhenius and Bronsted-Lowry
23. Conjugate acid-base pair is ….
a. an acid and base that react to form water
b. a pair of acids with similar structures
c. two substances related by the donation/acceptance of a proton
d. two substances that have the same acid-base effect in water.
24. Which of the following pairs does not represent a conjugate acid-base pair?
a. HClO4 / ClO4-
b. HCl / Cl-
c. H2SO4 / SO42-
d. H2O / OH-
e. NH3 / NH4+
25. Identify the Brønsted-Lowry acids and bases (conjugate pairs) in the following equation. (A= B-L acid; B= B-L base)
HC2H3O2 + CN- = HCN + C2H3O2–
a. B A B A
b. B B A A
c. A B A B
d. A B B A
e. B A A B
26. The conjugate of a weak base is …
a. a strong base
b. a weak base
c. a strong acid
d. a weak acid
e. None of these
27. Which of these is the weakest conjugate base?
a. NH2–
b. Cl-
c. C2H3O2–
d. CN-
e. SO42–
28. NH3 + H2O Û NH4+ + OH-
The correct statement is ….
a. NH3 is acid
b. NH4+ is conjugate acid of NH3
c. H2O is base
d. OH- is conjugate base of NH4+
e. NH3- and H2O are conjugate acid and conjugate base
29. H2O + HCO3- Û H2CO3 + OH- The bases are ….
a. H2O and HCO3-
b. H2CO3 and H2O
c. H2CO3 and OH-
d. H2O and OH-
e. HCO3- and OH-
30. From the above equation, the correct statement is ….
a. H2O is a weak acid
b. HCO3- is neutral
c. OH- is a weak base
d. H2CO3 is a weak acid
31. H2O + HCN ↔ CN- + H3O+
In this equation ….
a. HCN is a base
b. H2O and HCN are a weak base and a weak acid
c. H3O+ is a base
d. CN- is a conjugate acid of HCN
32. H2O + HSO4- ↔ SO42- + H3O+
The wrong statement is ….
a. as an acid, HSO4- is weaker than H3O+
b. as a base, HSO4- is stronger than H3O+
c. as an acid, H2O is weaker than H3O+
d. H2O is stronger than SO42-
33. Known 5 equations below:
1. H2O + NH3 ↔ NH4+ + OH-
2. H2O + HF ↔ H3O+ + F-
3. H2O + NH3 ↔ NH2- + H3O+
4. H2O + HCN ↔ CN- + H3O+
5. H2O + HSO4- ↔ SO42- + H3O+
Occording to Bronsted–Lowry, H2O as an acid and a base are in number ....
a. 1 and 2
b. 2 and 3
c. 2 and 4
d. 2 and 5
e. 4 and 5
34. The difference between acid and conjugate base is ….
a. a proton
b. a neutron
c. an electron
d. a nucleus
e. none of these
35. A substance that may act as both an acid and a base is ….
a. a hydride
b. a hydroxide
c. disproportionate
d. amphoteric
e. a salt
36. Which of the following would be the most basic substance in aqueous solution?
a. HSO4-
b. F-
c. I-
d. Cl-
e. NO3-
37. Which of the following would be the most acidic substance in aqueous solution?
a. Na+
b. SO42-
c. H2O
d. NH2-
e. NH4+
38. According to the Lewis theory, a base ….
a. is a proton acceptor.
b. is a proton donor.
c. makes available a share in a pair of electrons.
d. is any compound that contains electron pairs.
e. accepts a share in a pair of electrons.
39. Which statement concerning the autoionization (self-ionization) of water is FALSE?
2 H2O(l) <==> H3O+ + OH-(aq)
a. This reaction is an acid-base reaction according to the Bronsted-Lowry theory.
b. ater is amphiprotic.
c. A H2O molecule may react as an acid by donating a proton.
d. In this reaction H3O+ and OH- are a conjugate acid-base pair
e. A H2O molecule may react as a base by accepting a proton.
40. To prepare 1.0 L of a 0.100 M solution of phosphoric acid, the volume (mL) of the concentrated solution (15 M) which needed is ….
a. 6.7 b. 6.67 c. 20.0 d. 2.2 e. 2.0
41. Barium hydroxide is a strong base. Compute [Ba2+] and [OH-] for a solution that is prepared by dissolving 6.0 x 10-2 mole of barium hydroxide in 500.0 mL of water. (Ar Ba = 137.33, O = 16.00, H = 1.008)
a. 1.2 x 10-2, 2.4 x 10-2
b. 1.2 x 10-1, 1.2 x 10-1
c. 1.2 x 10-1, 2.4 x 10-1
d. 1.2 x 10-2, 1.2 x 10-2
e. 2.5 x 10-1, 1.2 x 10-1
42. Calculate the [ClO4-], and [H3O+] in an aqueous solution containing 0.025 moles of HClO4 in 500.0 mL of water.
a. 2.0 x 10-12, 5.0 x 10-2
b. 5.0 x 10-2, 2.0 x 10-12
c. 5.0 x 10-2, 5.0 x 10-2
d. 2.0 x 10-13, 5.0 x 10-1
e. 5.0 x 10-2, 2.0 x 10-2
43. The normality of a solution of sulfuric acid that is 0.200 M is ….
a. 0.200N b.0.400N c. 0.100N d. 0.196N e. 0.980N
44. A bottle of wine vinegar contains 6.5HC2H3O2 by mass. If vinegar has a density of 1.03 g/ml, how many grams of HC2H3O2 are in a 400 ml bottle?
a. 13g b. 35g c. 27g d. 260g e. 6g
45. Glacial acetic acid has a density of 1.05 g/ml. If 46.2 of HC2H3O2 will dissolve in 1.0g of water, the molarity of the solution is ….
a. 14M b. 17M c. 4M d. 5M e. 36M
46. Glacial acetic acid is a saturated solution. If 46.2 g of HC2H3O2 will dissolve in 1.0g of water, the mass percent acetic acid is ….
a. 90 b. 98 c. 102 d. 47 e. 2
47. When 25.00 mL of 0.250 M potassium hydroxide solution reacts with 20.00 mL of 0.500 M sulfuric acid solution, _____ moles of water will be produced.
a. 5.00 x 10-3
b. 13.0 x 10-3
c. 100 x 10-3
d. 6.25 x 10-3
e. 3.75 x 10-3
48. How many mL of water must be added to 50 mL of 0.100M HCl to dilute it to 0.033M?
a. 151 b. 75 c. 101 d. 61 e. 201
49. What is the normality of 100g of H2SO4 dissolved in 1L of H2O?
a. 1.0 b. 2.1 c. 0.55 d. 10.5 e. 3.6
50. How many millimoles of H+ are there in 50.0 mL of 0.10 M HCl?
a. 50.0 mol
b. 20.0 mol
c. 5.0 mol
d. 2.0 mol
e. 0.5 mol
51. How many mmol OH- are there in 20.0 mL of 0.010 M Ba(OH)2?
a. 0.40 mmol
b. 0.20 mmol
c. 0.02 mmol
d. 0.04 mmol
e. 0.08 mmol
52. What is the molarity of 250.0 mL of a solution which contains 25.0 mmol of H+?
a. 2.5 M d. 1.0 M
b. 0.5 M e. 0.25 M
c. 0.1 M
53. Given the following Ka values, determine which species is the strongest base.
H2SO3 1.2 x 10-2 HNO2 4.5 x 10-4 HCNO 3.5 x 10-4
a. H2SO3
b. NO2-
c. HNO2
d. HSO3-
e. CNO-
54. The Ka values for HCNO and HNO2 are 2.2 x 10-4 and 4.5 x 10-4 respectively. Therefore it follows the HCNO is a acid than HNO2 and CNO- is a _____ base than NO2-.
a. stronger, stronger
b. stronger, weaker
c. weaker, weaker
d. weaker, stronger
55 The Ka values for HS- and HPO42- are 1.2 x 10-13 and 4.8 x 10-13 respectively. Therefore it follows the HS- is a _____ acid than HPO42- and S2- is a _____ base than PO43-.
a. stronger, stronger
b. stronger, weaker
c. weaker, weaker
d. weaker, stronger
56. Based upon the following values of Ka, place the acids in order from weakest to strongest ….
HCN (Ka = 6.2 x 10-10)
HCOOH (Ka =1.78 x 10-4)
HC2H3O2 (Ka = 1.8 x 10-5)
HNO2 (Ka = 4.6x10-4)
a. HC2H3O2-HCN-HNO2-HCOOH
b. HCN-HC2H3O2-HCOOH-HNO2
c. HCN-HNO2-HC2H3O2-HCOOH
d. HCOOH-HNO2-HCN-HC2H3O2
e. HNO2-HCOOH-HC2H3O2-HCN
57. Which of the following is not true for the dissociation of a strong acid?
a. The equilibrium lies far to the right
b. equilibrium lies far to the left
c. [H+] >> [HA]
d. Ka is large
e. The conjugate base will be weak
58. What change will be observed for the following reaction if a few drops of NaOH are added?
HNO2+H2O NO2-+H3O+
a. an increase in the fraction of acid dissociated
b. a decrease in the fraction of acid dissociated
c. no change in the fraction of acid dissociated
59. What change will occur for the following reaction if a few drops of HCl are added?
CH3CO2H + H2O --> CH3CO2- + H3O+
a. a decrease in the fraction of acid dissociated
b. an increase in the fraction of acid dissociated
c. no change in the fraction of acid dissociated
60. Given Ka values of 1.8 x 10-4 and 6.8 x 10-4 for HCO2H and HNO2 respectively, the equilibrium constant for the following reaction is ….
HCO2- + HNO2 --> HCO2H + NO2-
a.0.26
b.8.6 x 10-4
c.5.0 x 10-4
d.1.2 x 10-7
e.3.8
61. Given Ka values of 1.0 x 10-10 and 6.8 x 10-8 for C6H5OH and C5H5NH+ respectively, the equilibrium constant for the following reaction is ….
C6H5O- + C5H5NH+
C6H5OH + C5H5N
a. 0.15
b. 6.8 x 10-8
c. 6.8 x 10-2
d. 1.5 x 10-3
e. 6.8 x 102
62. Given Ka values of 5.6 x 10-10 and 1.7 x 10-5 for NH4+ and CH3CO2H respectively, calculate the equilibrium constant for the following reaction.
NH4+ + CH3CO2- --> NH3 + CH3CO2H
a. 3.3
b. 0.30
c. 1.7 x 10-5
d. 3.0 x 104
e. 3.3 x 10-5
63. What is the hydronium ion concentration of a 0.380 M acid solution of an acid whose ionization constant is 1.58x10-9
a. 4.16 x 10-9
b. 2.45 x 10-5
c. 1.26 x 10-5
d. 6.00 x 10-10
e. 6.45 x 10-5
64. What is the hydronium ion concentration of a 0.1 M solution of Zn2+ solution of zinc perchlorate? The acidity constant of the following reaction is 3 x 10-10.
Zn2+(aq) + 2 H2O --> Zn(OH)+(aq) + H3O+
a. 5 x 10-6
b. 2 x 10-4
c. 2 x 10-6
d. 2 x 10-5
e. 5 x 10-5
65. What is the hydronium ion concentration of a 0.02 M solution of Cu2+ solution of copper(II) perchlorate? The acidity constant of the following reaction is 5x10-9
Cu2+(aq) + 2 H2O --> Cu(OH)+(aq) + H3O+
a. 1 x 10-5
b. 5 x 10-4
c. 7 x 10-5
d. 7 x 10-4
e. 1 x 10-4
66. What is the ionization constant of an acid if the hydronium ion concentration of a 0.400 M solution is 1.40 x 10-4 M?
a. 1.22 x 10-9
b. 4.90 x 10-8
c. 1.96 x 10-8
d. 1.40 x 10-3
e. 1.40 x 10-6
67. What is the acidity constant for the following reaction given that the hydronium ion concentration of a 0.04 M solution of Ni2+ solution of nickel(II) perchlorate is 4.5x10-6?
Ni2+(aq) + 2 H2O --> Ni(OH)+(aq) + H3O+
a. 4 x 10-6
b. 2 x 10-10
c. 2 x 10-12
d. 5 x 10-10
e. 5 x 10-12