2. Rank the following acids from strongest to weakest:
H2O, H2S, H2SO4, HClO3, HClO2
A) H2SO4 > HClO3 > HClO2 > H2O > H2S
B) H2SO4 > HClO3 > HClO2 > H2S > H2O
C) H2SO4 > H2S > H2O > H2S > HClO3, HClO2
D) H2SO4 > HClO2 > HClO3 > H2S > H2O
E) H2O > H2S > H2SO4 > HClO3 > HClO2
3. Which one of the following salts gives a basic aqueous solution?
4. Which one of the following salts gives a neutral aqueous solution?
5. The percentage of ionization for an acid will_________ as the concentration ___________.
A) decrease; decreases
B) increase; increases
C) decrease; increases
D) increase; decreases
7. Which one of the following would be expected to change the value of the equilibrium constant?
A) Increasing the amount of reactant.
B) Increasing the amount of product.
C) The addition of a catalyst.
D) Reduce the temperature of the reaction.
8. What is the pH of a 0.0001 M HBr solution?
9. Which of the following statements is correct?
A) Nonmetals usually form basic oxides.
B) Nonmetals have the lowest electronegativity.
C) Metals usually form basic hydroxides.
D) Nonmetals usually form ionic compounds with other nonmetals
E) All of the above are correct.
10. What is the pH of a solution that is 1.7 x 10-4 M in H+?
E) None of these.
11. Which of the following compounds can act as either a Brønsted acid or a Brønsted base?
B) I and II
C) II and III
D) I and V
12. Which one of the following is the strongest acid?
A) CH3COOH (Ka = 1.8 x 10-5)
B) HCOOH (Ka = 1.0 x 10-4)
C) HClO (Ka = 3.0 x 10-8)
D) HF (Ka = 6.8 x 10-4)
13. Consider the following reaction:
H2PO4- (aq) + HCO3-(aq) ↔ H2CO3(aq) + HPO42-(aq)
Brønsted would identify the acidic species as:
A) H2PO4- and H2CO3
B) H2PO4- and HPO42-
C) HCO3- and H2CO3
D) HCO3- and HPO42-
E) H2CO3 and HPO42-
14. Given Ka values of 4.8 x 10-10 and 6.8 x 10-4 for HCN and HNO2 respectively, calculate the equilibrium constant for the following reaction:
HCN + NO2- ↔ CN- + HNO2
A) 7.05 x 10-7
B) 3.26 x 10-14
C) 1.41 x 106
D) 2.0 x 10-6
15. Which of the following is not a conjugate acid/base pair?
A) NH4+ and NH3
B) H2O and OH-
C) H3O+ and OH-
D) NH3 and NH2-
E) All of these are conjugate acid/base pairs.
16. What is the hydrogen ion concentration for pure water?
A) 1.0 x 10-14
B) 1.0 x 10-7
C) 1.0 x 1014
D) 1.0 x 107
17. For the reaction shown, which of the following statements would be true, given the listed value for K?
HNO2 (aq) + CH3COO- (aq) CH3COOH (aq) + NO2- (aq) K = 25
A) CH3COO- is the weakest acid.
B) HNO2 is the weakest acid.
C) CH3COOH is the weakest acid.
D) NO2- is the strongest base
E) The solution will contain more HNO2 than CH3COOH at equilibrium
18. Which of the following compounds is not an Arrhenius acid?
19. If the pH of a solution is increased by one point, the proton concentration:
A) is decreased by a factor of one.
B) is decreased by a factor of ten.
C) is increased by a factor of one.
D) is increased by a factor of ten.
E) does not change.
20. Which of the following is not a Brønsted base?
21. Calculate the pH of 0.020 M hypochlorous acid, Ka = 3.0 x 10-8, solution
22. If 5 g of Ba(OH)2 is dissolved in enough water to make 750 mL of solution, what is the pH?
23. The pH of a 0.10 M solution of a weak base is 9.82. What is the Kb for this base?
A) 2.1 × 10-4
B) 4.3 × 10-8
C) 6.6 × 10-4
D) 2.0 × 10-5
E) 8.8 × 10-8
24. What can be correctly concluded from the fact that the following the acid-base reaction proceeds ot the right, as written?
NH2-(aq) + HSO4-(aq) NH3(aq) + SO42-(aq)
A) NH3 is stronger base then NH2-
B) NH3 is a stronger acid than HSO4-
C) NH3 is a weaker acid than NH2-
D) NH3 is a weaker base than HSO4-
E) NH3 is a weaker acid than HSO4-
25. Which one of the following salts gives an acidic aqueous solution?
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