Acids Practice Test 2
1. What colour would 1.0 M HCl be in an indicator mixture consisting of phenol red and thymolphthalein?
2. During a titration, what volume of 0.500 M KOH is necessary to completely neutralize 10.0 mL of 2.00 M CH3COOH?
A 10.0 mL
B 20.0 mL
C 25.0 mL
D 40.0 mL
3. Which indicator has a Ka = 1.0 x 10-6?
A neutral red
B thymol blue
D chlorophenol red
4. Acid is added to a buffer solution. When equilibrium is reestablished the buffering effect has resulted in [H3O+]
A increasing slightly
B decreasing slightly
C increasing considerably
D decreasing considerably
5. A buffer solution will form when 0.10 M NaF is mixed with an equal volume of
A 0.10 M HF
B 0.10 M HCl
C 0.10 M NaCl
D 0.10 M NaOH
6. Which of the following statements applies to 1.0 M NH3(aq) but not to 1.0 M NaOH(aq)?
A partially ionizes
B neutralizes an acid
C has a pH greater than 7
D turns bromocresol green from yellow to blue
7. In which of the following are the reactants favoured?
A HNO2 + CN- ⇄ NO2- + HCN
B H2S + HCO3- ⇄ HS- + H2CO3
C H3PO4 + NH3 ⇄ H2PO4- + NH4+
D CH3COOH + PO43- ⇄ CH3COO- + HPO42-
8. What is the pOH of a solution prepared by adding 0.50 moles of NaOH to prepare 0.50 L of solution?
9. What is the [H3O+] in a solution with a pH = 5.20?
A 1.4 x 10-14
B 1.6 x 10-9
C 6.3 x 10-6
D 7.1 x 10-1
10. Consider the following equilibrium: 2H2O(l) + energy ⇄ H3O+(aq) + OH-(aq)
What will cause the pH to increase and the Kw to decrease?
A adding a strong acid
B adding a strong base
C increasing the temperature
D decreasing the temperature
11. The complete neutralization of 15.0 mL of KOH requires 0.0250 moles H2SO4. The [KOH] was
A 1.50 M
B 1.67 M
C 3.33 M
D 6.67 M
12. What is the [H3O+] at the equivalence point for the titration between HBr and KOH?
A 1.0 x 10-9 M
B 1.0 x 10-7 M
C 1.0 x 10-5 M
D 0.0 M
13. Which of the following would form a buffer solution when equal moles are mixed together?
A HCl and NaCl
B HCN and NaCN
C KNO3 and KOH
D Na2SO4 and NaOH
14. Which of the following acids has the weakest conjugate base?
15. When 10.0 ml of 0.10 M HCl is added to 10.0 mL of water, the concentration of H3O+ in the final solution is
A 0.010 M
B 0.050 M
C 0.10 M
D 0.20 M
16. The conjugate base of an acid is produced by
A adding a proton to the acid
B adding an electron to the acid
C removing a proton from the acid
D removing an electron from the acid
17. Which of the following represents the predominant reaction between HCO3- and water?
A 2HCO3- ⇄ H2O + 2CO2
B HCO3- + H2O ⇄ H2CO3 + OH-
C HCO3- + H2O ⇄ H3O+ + CO32-
D 2HCO3- + H2O ⇄ H3O+ + CO32- + OH- + CO2
18. Water acts as an acid when it reacts with
A I and IV only
B II and III only
C I, II, and IV
D II, III, and IV
19. In a solution of 0.10 M H2SO4, the ions present in order of decreasing concentration are
A [H3O+] > [HSO4-] > [SO42-] > [OH-]
B [H3O+] > [SO42-] > [HSO4-] > [OH-]
C [OH-] > [SO42-] > [HSO4-] > [H3O+]
D [SO42-] > [HSO4-] > [OH-] > [H3O+]
20. Which of the following will dissolve in water to produce an acidic solution?
21. Which of the following solutions will have a pH = 1.00?
I 0.10 M HCl
II 0.10 M HNO2
III 0.10 M NaOH
A I only
B II only
C I and II only
D I, II, and III
22. Ka for the acid H2AsO4- is 5.6 x 10-8. What is the value of the Kb for HAsO42-?
A 5.6 x 10-22
B 3.2 x 10-14
C 1.8 x 10-7
B 2.4 x 10-4
23. In a titration, which of the following has a pH = 7.00 at the equivalence point?
A NH3 and HNO3
B KOH and HCl
C NaF and HCl
D Ca(OH)2 and CH3COOH
24. Which of the following salts dissolves to produce a basic solution?
25. Calculate the pH in a 0.200 M solution of Sr(OH)2.
26. Which of the following solutions has a pH less than 7.00?
27. Which of the following will form a basic aqueous solution?
28. What is the approximate Ka value for the indicator chlorophenol red?
A 1 x 10-14
B 1 x 10-8
C 1 x 10-6
D 1 x 10-3
29. What is the approximate pH of the solution formed when 0.040 mol NaOH is added to 2.00 L of 0.020 M HCl?
30. In which one of the following equations are the Bronsted acids and bases all correctly identified?
Acid + Base ⇄ Base + Acid
A H2O2 + SO32- ⇄ HO2- + HSO3-
B H2O2 + SO32- ⇄ HSO3- + HO2-
C SO32- + H2O2 ⇄ HO2- + HSO3-
D SO32- + H2O2 ⇄ HSO3- + HO2-
31. Which of the following titrations will always have an equivalence point at a pH > 7.00?
A weak acid with a weak base
B strong acid with a weak base
C weak acid with a strong base
D strong acid with a strong base
32. A buffer solution may contain equal moles of
A weak acid and strong base
B strong acid and strong base
C weak acid and its conjugate base
D strong acid and its conjugate base
33. A gas which is produced by burning coal and also contributes to the formation of acid rain is
34. Which of the following 1.0 M salt solutions is acidic?
35. Which of the following statements applies to 1.0 M NH3(aq) but not to 1.0 M NaOH(aq)?
A partially ionizes
B neutralizes and acid
C has a pH greater than 7
D turns bromcresol green from yellow to blue
36. When the indicator thymol blue is added to 0.10 M solution of an unknown acid, the solution is red. The acid could be
1. Calculate the pH of the solution prepared by mixing 15.0 mL of 0.50 M HCl with 35.0 mL 0.50 M NaOH.
HCl + NaOH → NaCl + HOH
0.0150 L x 0.50 moles 0.0350 L x 0.50 moles
I 0.0075 moles 0.0175 moles
C 0.0075 moles 0.0075 moles
E 0 0.0010 moles
[OH-] = 0.0010 moles = 0.20M
pOH = 0.70
pH = 13.30
2. Calculate the [OH-] in 0.50 M NH3(aq).
NH3 + H2O ⇄ NH4+ + OH-
I 0.50 0 0
C x x x Kb(NH3) = 1.0 x 10-14
E 0.50 - x x x
0 small Ka approximation Kb = 1.0 x 10-14 = 1.786 x 10-5
5.6 x 10-10
x2 = 1.786 x 10-5
x = [OH-] = 3.0 x 10-3 M
3. A titration was performed by adding 0.175 M H2C2O4 to a 25.00 mL sample of NaOH. The following data was collected.
Trial 1 Trial 2 Trial 3
Final volume of H2C2O4 from burette (mL) 23.00 39.05 20.95
Initial volume of H2C2O4 from burette (mL) 4.85 23.00 5.00
18.15 16.05 15.95 average to 16.00 mL
Calculate the [NaOH] reject
H2C2O4 + 2NaOH → Na2C2O4 + 2H20
0.0160 L 0.0250 L
0.175 M ? M
[NaOH] = 0.0160 L H2C2O4 x 0.175 mole x 2 mole NaOH
L 1 mole H2C2O4
= 0.224 M
4. A 250.0 mL sample of HCl with a pH of 2.000 is completely neutralized with 0.200 M NaOH. What volume of NaOH is required to reach the stoichiometric point.
pH = 2.000 [H+] = 0.010 M
HCl + NaOH → NaCl + H2O
0.2500 L x 0.0100 mole x 1moleNaOH x L = 0.0125 L
L 1 mole HCl 0.200 mole
5. If the HCl were titrated with 0.200 M NH3(aq) instead of 0.200 M NaOH, how would the volume of base required to reach the equivalence point compare with the volume calculated in the last question? Explain your answer.
It would be the same
HCl forces the reaction to completion so a weak base is as good as a strong base for neutralizing a strong acid.
6. Consider the following salt ammonium acetate, NH4CH3COO.
a) Write the equation for the dissociation of
NH4CH3COO → NH4+ + CH3COO-
b) Write the equations for the hydrolysis reactions that occur.
CH3COO- + H2O ⇄ CH3COOH + OH-
NH4+ + H2O ⇄ NH3 + H3O+
c) Explain why a solution of NH4CH3COO has a pH =7.00. Support your answer with a calculation.
Ka(NH4+) = 5.6 x 10-10
Kb(CH3COO-) = Kw = 5.6 x 10-10
1.8 x 10-5
7. Consider the following equilibrium: energy + 2H2O ⇄ H3O+ + OH-
a) Explain how pure water can have a pH = 7.30.
At a lower temperature the equilibrium shifts left, the [H3O+] decreases and the pH increases.
b) Calculate the value of the Kw for the sample of water with a pH = 7.30.
pH = 7.30 [H+] = 10-7.3 = 5.02 x 10-8 M
remember the [H+] = [OH-] = 5.02 x 10-8 M
Kw = [H+][OH-] = (5.02 x 10-8 M)2 = 2.5 x 10-15