Name: _________________________
Graded HW: Acid, Base and Salts
Date: ________
1. Which of the following would be a strong electrolyte?
A) A weak Arrhenius acid
C) A weak Lewis acid
E) A salt with a Ksp of 1.0 × 10 –9
B) A strong Arrhenius acid
D) A strong Lewis base
2. Which properties are common to both strong acids and bases?
I
II
III
Taste bitter.
Conduct an electric current.
Cause neutral litmus to change color.
A) II only
C) I and III only
E) I, II and III
B) I and II only
D) II and III only
3. Which 0.10 M solutions will have the greatest electrical conductivity?
A) HF
B) NH 3
C) NaOH
D) C6H5COOH E) PbCl 2
C) KOH
D) NaCl
4. Which is the weakest electrolyte?
A) CH 3COOH
B) HCl
5. An Arrhenius acid
A) accepts a proton
C) produces H + in solution
E) donates a pair of electrons
B) donates a proton
D) produces OH– in solution
6. An Arrhenius base is a substance which
A) donates protons
C) produces H + in solution
E) produces basic salts in solution
B) donates electrons
D) produces OH– in solution
7. Which two act as Brönsted–Lowry acids?
H2BO 3–(aq) + HCO 3–(aq) «
H2CO 3(aq)+ HBO32–(aq)
A) HCO3– and H2CO 3
C) HCO3– and HBO32–
E) H2BO 3– and HCO3–
B) H2BO 3– and H2CO 3
D) H2BO 3– and HBO32–
E) CaO
8. When hydrogen carbonate ion, HCO 3–, is added to water, the resulting solution is
A)
B)
C)
D)
E)
basic because the solute Kb is greater than K a
basic because the solute Ka is greater than K b
acidic because the solute K a is greater than K b
acidic because the solute K b is greater than K a
dependent on the temperature
9. In which equilibrium system does HCO 3– act as a Brönsted–Lowry base?
A) HCO3– « H+ + CO 32–
C) HCO3– + H2S « H2CO 3 + HS –
E) HCO3– + H2O « H3O + CO3–
B) HCO3– + HS – « H2S + CO 32–
D) HCO3– + H2O « H3O+ + CO 32–
10. Which of the following species is considered an acid according to the Lewis theory but
not according to the Arrhenius or Bronsted-Lowry theories?
A) A proton donor
C) HCl
E) An electron pair acceptor
B) A proton acceptor
D) An electron pair donor
11. Which of the following is hydroiodic acid
A) HI
C) HIO 3
E) none of the above
B) HIO 2
D) HIO 4
12. Which of the following is phosphoric acid?
A) H3P
C) H3PO 3
E) none of the above
B) H3PO 2
D) H3PO 4
13. What is the name of the acid formed by HNO2?
A) nitric acid
C) nitrous acid
E) none of the above
B) nitronic acid
D) hydronitrous acid
14. The acid formed by H 2SO 3 is called
A) sulfuric acid
C) hydrosulfuric acid
E) none of the above
B) sulfurous acid
D) hydrosulfurous acid
15. Which of the following is a weak acid?
A) H2S
B) HBr
C) HI
D) HNO3
E) H2SO 4
16. Base your answer to the following question on the data from the chart below.
Which is amphiprotic?
A) SO 32–
B) NH 4+
C) PO 43–
D) HSO 3–
17. Which indicator will be yellow at pH 7 and blue at pH 10?
A) thymol blue
C) bromothymol blue
E) none of the above
B) methyl violet
D) bromocresol green
E) H2SO 4
18. An indicator is added to solutions of different pH.
The indicator is
A) methyl red
C) methyl orange
E) either thymol blue or methyl orange
B) thymol blue
D) bromothymol blue
19. Which equation correctly calculates the
?
A)
B)
C)
E)
D)
20. Which is true?
A) [H3O+ ] [OH–] = 14.00
C) [H3O+ ] – [OH–] = 14.00
E) [H3O+ ] [OH–] = 1.0 × 10 –14
B) [H3O+ ] + [OH–] = 14.00
D) [H3O+ ] + [OH–] = 1.0 × 10 –14
21. Which is the correct equilibrium law equation for the ion product constant of water?
A)
B)
C)
D)
E)
22. What is the pH of 0.00040 M KOH?
A) 3.40
B) 4.60
C) 9.40
D) 10.60
E) 12.80
23. Which 0.1 M aqueous solutions has the highest pH?
A) NH 3
B) NaOH
C) HClO 4
D) CH 3COOH
E) CH 3COONa
24. In a solution the concentration of the OH – ion is 100 times greater than the concentration
of the H + ion. What is the pH of this solution?
A) 2
B) 6
C) 8
D) 12
25. Which solution has the highest electrical conductivity?
A) 1.0 M HCN
C) 1.0 M H2SO 3
E) 1.0 M CH 3CH 2OH
B) 1.0 M H2SO 4
D) 1.0 M CH 3COOH
E) 14