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Acid Base Worksheet with Solved 66 Extra Practice Problems, Exercises of Chemistry

Bethel University TennesseeChemistry

66 MCQs with solution key on acid, base and salt by Dr. Craig P. Jasperse Minnesota State University Moorhead.

Typology: Exercises

2020/2021

Uploaded on 03/30/2021

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General Chemistry II Jasperse
Acid-Base Chemistry. Extra Practice Problems
General Types/Groups of problems:
Conceptual Questions. Acids, Bases, and
Conjugates, Miscellaneous
p1
Kb and pKb, Base Strength, and using Kb or
pKb to Calculate [OH-], pOH, pH, and/or [H+]
p7-10
Recognizing Strong versus Weak Acids;
Recognizing Basic versus Nonbasic
p3
Recognizing Acid/Base Properties when
Ionics are Dissolved in Water
p11
pH Calculations; Relationships between pH and pOH
p4
Answers
p12
Ka: Sense + Calculations. Using Ka or pKa to Calculate
[H+] and/or pH; using pH to calculate Ka or pKa
p5
Conceptual Questions. Acids, Bases, and Conjugates, Miscellaneous
1. In the Brønsted–Lowry definition of acids and bases, an acid __________
a.
d.
breaks stable hydrogen bonds.
b.
e.
corrodes metals.
c.
2. In the Brønsted–Lowry definition of acids and bases, a base __________
a.
d.
breaks stable hydrogen bonds.
b.
e.
corrodes metals.
c.
3. In the following reaction in aqueous solution, the acid reactant is __________ and its conjugate base product is
__________.
CH3COOH + NH3 CH3COO– + NH4
+
a.
d.
NH3; NH4
+
b.
e.
CH3COOH; H3O+
c.
4. In the following reaction in aqueous solution, the acid reactant is __________, and its conjugate base product is
__________.
CH3NH2 + HSO4
– CH3NH3
+ + SO4
2–
a.
d.
HSO4
–; SO4
2–
b.
e.
HSO4
–; H3O+
c.
5. Which of the following is the conjugate acid of the hydrogen phosphate ion, HPO4
2–?
a.
d.
PO4
3–
b.
e.
H3O+
c.
pf3
pf4
pf5
pf8
pf9
pfa

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Download Acid Base Worksheet with Solved 66 Extra Practice Problems and more Exercises Chemistry in PDF only on Docsity!

General Chemistry II Jasperse

Acid-Base Chemistry. Extra Practice Problems

General Types/Groups of problems:

Conceptual Questions. Acids, Bases, and

Conjugates, Miscellaneous

p1 Kb and pKb, Base Strength, and using Kb or

pKb to Calculate [OH-], pOH, pH, and/or [H+]

p7- 10

Recognizing Strong versus Weak Acids;

Recognizing Basic versus Nonbasic

p3 Recognizing Acid/Base Properties when

Ionics are Dissolved in Water

p

pH Calculations; Relationships between pH and pOH p4 Answers p

Ka: Sense + Calculations. Using Ka or pKa to Calculate [H+] and/or pH; using pH to calculate Ka or pKa

p

Conceptual Questions. Acids, Bases, and Conjugates, Miscellaneous

  1. In the Brønsted–Lowry definition of acids and bases, an acid __________ a. is a proton donor. d. breaks stable hydrogen bonds. b. is a proton acceptor. e. corrodes metals. c. forms stable hydrogen bonds.
  2. In the Brønsted–Lowry definition of acids and bases, a base __________ a. is a proton donor. d. breaks stable hydrogen bonds. b. is a proton acceptor. e. corrodes metals. c. forms stable hydrogen bonds.
  3. In the following reaction in aqueous solution, the acid reactant is __________ and its conjugate base product is __________. CH 3 COOH + NH 3 CH 3 COO–^ + NH 4 + a. CH 3 COOH; CH 3 COO–^ d. NH 3 ; NH 4 + b. CH 3 COOH; NH 4 +^ e. CH 3 COOH; H 3 O+ c. NH 3 ; CH 3 COO–
  4. In the following reaction in aqueous solution, the acid reactant is __________, and its conjugate base product is __________. CH 3 NH 2 + HSO 4 –^ CH 3 NH 3 +^ + SO 42 – a. CH 3 NH 2 ; CH 3 NH 3 +^ d. HSO 4 – ; SO 42 – b. CH 3 NH 2 ; SO 42 –^ e. HSO 4 – ; H 3 O+ c. HSO 4 – ; CH 3 NH 3 +
  5. Which of the following is the conjugate acid of the hydrogen phosphate ion, HPO 42 –? a. H 3 PO 4 d. PO 43 – b. H 2 PO 4 –^ e. H 3 O+ c. HPO 42 –
  1. Which one of the following is not a conjugate acid–base pair? a. NH 3 and NH 4 +^ d. HS–^ and H 2 S b. H 3 O+^ and OH–^ e. NH 3 and NH 2 – c. H 2 PO 4 –^ and HPO 42 –
  2. Which one of the following is a conjugate acid–base pair? a. NH 3 and NH 4 +^ d. H 2 O and O^2 – b. H 3 O+^ and OH–^ e. NaF and F– c. NH 2 -^ and NH 4 +
  3. Which one of the following is a conjugate acid–base pair? a. NaF and F–^ d. NH 4 +^ and NH 2 – b. HNO 3 and HNO 2 e. H 2 O and H 2 O 2 c. HI and I–
  4. Which one of the following is not a conjugate acid–base pair? a. NH 3 and NH 2 –^ d. H 2 PO 4 –^ and HPO 42 – b. HNO 3 and HNO 2 e. H 2 O and OH– c. HI and I–
  5. The stronger the acid, __________ a. the stronger its conjugate base. d. the less concentrated the conjugate base. b. the weaker its conjugate base. e. the more concentrated the conjugate base. c. the more concentrated the acid.
  6. Ammonia (NH 3 ) acts as a weak base in aqueous solution. What is the acid that reacts with this base when ammonia is dissolved in water? a. none, there are no acids in pure water b. H 2 O c. NH 4 + d. trick question, because no acids are present, ammonia cannot act as a base e. oxygen that always is dissolved in water
  7. The base ionization constant K b describes which of the following reactions for a weak base, B, in aqueous solution? (Note: often the base will be anionic rather than neutral, but “B” here is meant to represent anionic or neutral bases, which will gain one H and become one charge unit more positive whether starting neutral or anionic.) a. B + H+^ BH+^ d. B + OH–^ BH–^ + O^2 – b. B + H 3 O+^ BH+^ + H 2 O e. BH+^ + OH–^ B + H 2 O c. B + H 2 O BH+^ + OH–

pH Calculations; Relationships between pH and pOH

  1. If the pH of a solution increases by 2 units (e.g., from 1 to 3), then the ratio of the new to the original hydronium ion concentration is __________ a. 2/1 d. 1/100. b. 100/1 e. 1/1, unchanged c. 1/
  2. When [H+] = 1.0 × 10 –^7 M in water at 25°C, then __________ a. pH = 1. d. (^) [OH–] = 1.0 × 107 M. b. pH = 10–^7. e. [OH–] = 0 M. c. (^) [OH–] = 1.0 × 10 –^7 M.
  3. When [H+] = 4.0 × 10 –^9 M in water at 25°C, then __________ a. pH = 9.40. d. pH = 8.40. b. pH = 7.00. e. pH = – 9. c. pH = – 8.40.
  4. A solution with pH of 9.50 has a pOH of __________ a. 9.50. d. 23.5. b. 0.50. e. 19.0. c. 4.50.
  5. A solution with an [OH–] concentration of 1.20 × 10 –^7 M has a pOH and pH of __________ a. 6.92 and 7.08 d. 7.08 and 6. b. 1.00 and 13.00 e. 5.94 and 8. c. 5.35 and 8.
  6. A solution with a pOH of 4.3 has a [H+] of __________ a. (^) 6.8 × 10 –^9 M. d. (^) 2.0 × 10 –^10 M. b. (^) 3.2 × 10 –^4 M. e. 4.3 M. c. (^) 4.8 × 10 –^5 M.
  7. Which statement, A–D, is not correct? If all are correct, respond E. Pure water at 25°C has __________ a. (^) K w = 1.0 × 10 –^14. d. pH = 7. b. pOH = 7. e. A–D are all correct. c. [H 3 O+] = [OH–].

Ka: Sense + Calculations. Using Ka or pKa to Calculate [H+] and/or pH; using pH to calculate Ka or pKa

  1. Solutions of each of the hypothetical acids in the following table are prepared with an initial concentration of 0.100 M. Which of the four solutions will have the lowest pH and be most acidic? Acid p K a HA 4. HB 7. HC 10. HD 11. a. HA d. HD b. HB e. All will have the same pH because the concentrations are the same. c. HC
  2. What is the hydronium ion concentration of a 0.010 M solution of acetic acid? Ka for acetic acid is 1.8 x 10–^5 a. (^) 1.8 × 10 –^3 d. (^) 1.8 × 10 –^7 b. (^) 1.8 × 10 –^5 e. (^) 4.2 × 10 –^4 c. (^) 1.0 × 10 –^2
  3. What is the pH of a 0.010 M solution of acetic acid? K a for acetic acid is 1.8 × 10 –^5 a. 2.74 d. 3. b. 4.74 e. 6. c. 2.
  4. When values of K a are small (e.g., 1 × 10 –^5 ) and concentrations of weak acids [HA] are relatively large (e.g., 0.10 M ), and assuming there is no other source of anion A–, the hydronium ion concentration of the solution can be calculated using which expression? a. [H+] = K a d. [H+] = K a K b[HA] b. [H+] = K a[HA] e. [H+] = K a[HA]^2 /[A–] c. [H+] = ( K a[HA])1/
  5. The first disinfectant used by Joseph Lister was called carbolic acid. This substance now is known as phenol, C 6 H 5 OH (p K a = 10.0). What is the pH of a 0.10 M solution of phenol? a. 3.5 d. 5. b. 10.0 e. 4. c. 6.
  6. The pH of a popular soft drink is 3.4; what is its hydronium ion concentration? a. (^) 5.0 × 10 –^4 M d. (^) 1.0 × 10 –^7 M b. (^) 4.0 × 10 –^4 M e. (^) 5.0 × 10 –^5 M c. (^) 2.5 × 103 M

Kb and pKb, Base Strength, and using Kb or pKb to Calculate [OH-], pOH, pH, and/or [H+]

a. (^) 3.6 × 10 –^6 M d. (^1) .9 × 10 –^3 M b. (^) 1.8 × 10 –^5 M e. (^) 4.2 × 10 –^4 M

  • a. 1.0 × 10 –^4 d. 39. A cup of coffee has a hydroxide ion concentration of 1.0 × 10 –^10 M What is the pH of this coffee?
  • b. 4 e. –
  • c.
    1. What is the concentration of [OH–] in a 0.20 M solution of ammonia? The K b value for ammonia is 1.8 × 10 –
    1. What is the pOH of a 0.20 M solution of ammonia? The K b value for ammonia is 1.8 × 10 – c. 0.20 M
    • a. 4.44 d. 2.
    • b. 4.74 e. 3.
    • c. 0.
    1. What is the pH of a 0.20 M solution of ammonia? The K b value for ammonia is 1.8 × 10 –
    • a. 9.56 d. 11.
    • b. 9.26 e. 2.
    • c. 4.
    1. What is the hydronium ion concentration of a 0.20 M solution of ammonia? The K b value for ammonia is 1.8 × 10 –
    • a. 2.8 × 10 –^10 d. 5.2 × 10 –
    • b. 5.5 × 10 –^10 e. 1.9 × 10 –
    • c. 1.8 × 10 –
    • a. 2.22 d. 4. 44. What is the pH of a 0.500 M solution of trimethylamine (p K b = 4.13)?
    • b. 11.8 e. 5.
    • c. 0.

Miscellaneous problems involving Weak Bases and perhaps their Conjugates.

  1. Phosphoric acid is a triprotic acid, ionizing in the following sequential steps: H 3 PO 4 + H 2 O H 2 PO 4 –^ + H 3 O+^ K a H 2 PO 4 –^ + H 2 O HPO 42 –^ + H 3 O+^ K a HPO 42 –^ + H 2 O PO 43 –^ + H 3 O+^ K a Write the Kb expression for the base, sodium phosphate (Na 3 PO 4 )?
  2. Phosphoric acid is a triprotic acid, ionizing in the following sequential steps: H 3 PO 4 + H 2 O H 2 PO 4 –^ + H 3 O+ H 2 PO 4 –^ + H 2 O HPO 42 –^ + H 3 O+ HPO 42 –^ + H 2 O PO 43 –^ + H 3 O+ Write the Kb expression for the base, sodium dihydrogen phosphate (NaH 2 PO 4 )?
  3. Use the following acid ionization constants to identify the correct decreasing order of base strengths. HF (^) K a = 7.2 × 10 –^4 HNO 2 K a = 4.5 × 10 –^4 HCN (^) K a = 6.2 × 10 –^10 a. CN–^ > NO 2 –^ > F–^ d. F–^ > NO 2 –^ > CN– b. NO 2 –^ > F–^ > CN–^ e. NO 2 –^ > CN–^ > F– c. F–^ > CN–^ > NO 2 –
  4. Three acids found in foods are lactic acid (in milk products), oxalic acid (in rhubarb), and malic acid (in apples). The p K a values are LA = 3.88, OA = 1.23, and MA = 3.40. Which list has the conjugate bases of these acids in order of decreasing strength? a. lactate > oxalate > malate d. oxalate > lactate > malate b. oxalate > malate > lactate e. malate > lactate > oxalate c. lactate > malate > oxalate
  5. What is the pH of a 0. 20 M solution of cubaramine? The K b value for jaspersamine is 2.5 × 10 –^6.
  6. What is the pH of a 0.10 M solution of trimethylamine (p K b = 4.13)?

Getting Information about an Acid or Base Based on Ka or pKa or Kb or pKb of the conjugate.

56. What is the pH of a 0.20 M solution of sodium acetate? The Ka for acetic acid is 1.8 x 10–^5?

57. What is the pH of a 0. 40 M solution of sodium nitrite, NaNO 2? The pKa for nitrous acid (HNO 2 ) is 3.35.

  1. What is the pH of a 0. 20 M solution of weak acid jaspersammonium bromide? The K b value for jaspersamine is 4.0 × 10 –^5.
  2. What is the pH of a 0.10 M solution of weak acid trimethylammonium chloride? The p K b = 4.13 for it’s conjugate base triethylamine

Recognizing Acid/Base Properties when Ionics are Dissolved in Water

  1. Aqueous solutions of __________ are basic. a. NaF d. NaI b. NaCl e. KI c. NaBr
  2. Which one of the following salts forms aqueous solutions with pH = 7? a. Na 2 S d. NaNO 2 b. NaBr e. Na 2 CO 3 c. NaClO 2
  3. Which one of the following salts forms aqueous solutions with pH = 7? a. NaCN d. NaH 2 PO 4 b. NH 4 Br e. Na 2 CO 3 c. NaNO 3
  4. Which one of the following salts does not produce a basic solution when dissolved in water? a. NaOCH 3 d. NaNO b. NaHSO 4 e. NaHCO 3 c. NaBrO 2
  5. The pH of an aqueous sodium fluoride (NaF) solution is __________ because __________ a. 7; sodium fluoride is a simple salt. b. above 7; fluoride is a weak base. c. below 7; fluoride reacts with water to make hydrofluoric acid. d. about 7; fluoride is a weak base, but produces hydrofluoric acid, and these two neutralize one another. e. 0; sodium fluoride is a salt not an acid or a base.
  6. Which one of the following, A–D, is correct? If all are correct, respond E. a. K 2 SO 3 is a stronger base than KHSO 3. d. Na 2 HPO 4 is a weaker base than NaH 2 PO 4. b. K 2 CO 3 is a weaker base than KHCO 3. e. All of these statements are correct. c. NaHSO 3 is a stronger acid than NaHSO 4.
  7. Which of the following groups, A–D, consist of salts that all form basic solutions in water? (Ac = acetate) If none or all satisfy this criterion, respond E. a. NaNO 3 , NH 4 CN, NaAc, NH 4 Cl d. NaHCO 3 , NaF, NH 4 Cl, Na 2 SO 3 b. Na 2 CO 3 , KCl, NaOOCH 3 , NH 4 Cl e. None or all of the above. c. Na 2 CO 3 , NaF, NaOOCH 3 , NaCN