Chapter 16
Calculate the hydroxide ion concentration in an aqueous solution that contains 3.50 × 10-2 M in hydronium ion. A) 2.86 × 10-5 M B) 2.86 × 10-10 M C) 2.86 × 10-13 M D) 3.50 × 10-13 M
C) 2.86 × 10-13 M
How many of the following are weak acids? HNO2 HClO HNO3 H2PO4⁻ A) 0 B) 1 C) 3 D) 4 E) 2
C) 3
Find the percent ionization of a 0.337 M HF solution. The Ka for HF is 3.5 × 10-4. A) 1.1 % B) 1.2 × 10-2 % C) 3.2 % D) 3.5 × 10-2 % E) 4.7 %
C) 3.2 %
Calculate the hydronium ion concentration in an aqueous solution that contains 2.50 × 10-4 M in hydroxide ion. A) 4.00 × 10-9 M B) 4.00 × 10-10 M C) 4.00 × 10-11 M D) 5.00 × 10-11 M
C) 4.00 × 10-11 M
Calculate the hydronium ion concentration in an aqueous solution with a pH of 4.33 at 25°C. A) 2.1 × 10-10 M B) 9.7 × 10-10 M C) 4.7 × 10-5 M D) 3.8 × 10-5 M E) 6.3 × 10-6 M
C) 4.7 × 10-5 M
Determine the pOH of a 0.227 M C5H5N solution at 25°C. The Kb of C5H5N is 1.7 × 10-9. A) 4.59 B) 9.41 C) 4.71 D) 10.14 E) 9.29
C) 4.71
Determine the concentration of CO32- ions in a 0.18 M H2CO3 solution. Carbonic acid is a diprotic acid whose Ka1 = 4.3 × 10-7 and Ka2 = 5.6 × 10-11. A) 2.8 × 10-4 M B) 3.2 × 10-6 M C) 5.6 × 10-11 M D) 4.3 × 10-7 M E) 6.9 × 10-8 M
C) 5.6 × 10-11 M
Calculate the pOH in an aqueous solution with a pH of 7.85 at 25°C. A) 4.15 B) 5.15 C) 6.15 D) 7.15 E) 8.15
C) 6.15
Calculate the pH of a solution that contains 2.4 × 10-8 M H3O⁺ at 25°C. A) 2.40 B) 6.38 C) 7.62 D) 5.38 E) 8.62
C) 7.62
Determine the pH of a 0.22 M NaF solution at 25°C. The Ka of HF is 3.5 × 10-5. A) 10.20 B) 5.10 C) 8.90 D) 11.44 E) 2.56
C) 8.90
Which of the following is TRUE? A) A neutral solution contains [H2O] = [H3O⁺] B) A neutral solution does not contain any H3O+ or OH- C) An acidic solution has [H3O⁺] > [OH⁻] D) A basic solution does not contain H3O+ E) None of the above are true.
C) An acidic solution has [H3O⁺] > [OH⁻]
Which of the following bases is the weakest? The base is followed by its Kb value. A) HOCH2CH2NH2, 3.2 × 10-5 B) NH3, 1.76 × 10-5 C) C5H5N, 1.7 × 10-9 D) (CH3CH2)3N, 5.2 × 10-4 E) Since these are all weak bases, they have the same strength.
C) C5H5N, 1.7 × 10-9
Which Brønsted-Lowry acid is not considered to be a strong acid in water? A) HI B) HBr C) H2S O3 D) H NO3
C) H2S O3
Identify the weak diprotic acid. A) HNO3 B) H3PO4 C) H2SO3 D) HClO4 E) H2SO4
C) H2SO3
Which of these is an example of a polyprotic oxyacid? A) HClO3 B) CH3COOH C) H2SO3 D) H2S E) None of the above
C) H2SO3
Which of the following is a strong acid? A) C6H5CO2H B) HF C) HI D) NH4+ E) H2O
C) HI
Which of the following is a Brønsted-Lowry base? A) CH4 B) HCN C) NH3 D) I2 E) None of the above are Brønsted-Lowry bases.
C) NH3
Identify the base that is in baking soda. A) RbOH B) NaOH C) NaHCO3 D) K2CO3 E) NH3
C) NaHCO3
The stronger the acid, then which of the following is TRUE? A) The stronger the conjugate acid. B) The stronger the conjugate base. C) The weaker the conjugate base. D) The weaker the conjugate acid. E) None of the above
C) The weaker the conjugate base.
Identify the food that is not acidic. A) soft drink B) apple C) egg white D) soda E) wine
C) egg white
Calculate the hydronium ion concentration in an aqueous solution with a pH of 9.85 at 25°C. A) 7.1 × 10-5 M B) 4.2 × 10-10 M C) 8.7 × 10-10 M D) 6.5 × 10-5 M E) 1.4 × 10-10 M
E) 1.4 × 10-10 M
Calculate the hydroxide ion concentration in an aqueous solution with a pOH of 9.85 at 25°C. A) 7.1 × 10-5 M B) 4.2 × 10-10 M C) 8.7 × 10-10 M D) 6.5 × 10-5 M E) 1.4 × 10-10 M
E) 1.4 × 10-10 M
Determine the Ka for CH3NH3⁺ at 25°C. The Kb for CH3NH2 is 4.4 × 10-4. A) 3.1 × 10-10 B) 6.8 × 10-11 C) 5.6 × 10-10 D) 2.3 × 10-3 E) 2.3 × 10-11
E) 2.3 × 10-11
Determine the pH of a 0.18 M H2CO3 solution. Carbonic acid is a diprotic acid whose Ka1 = 4.3 × 10-7 and Ka2 = 5.6 × 10-11. A) 11.00 B) 10.44 C) 5.50 D) 4.31 E) 3.56
E) 3.56
Determine the [H3O⁺] in a 0.265 M HClO solution. The Ka of HClO is 2.9 × 10-8. A) 1.1 × 10-10 M B) 7.7 × 10-9 M C) 1.3 × 10-6 M D) 4.9 × 10-4 M E) 8.8 × 10-5 M
E) 8.8 × 10-5 M
Determine the pH of a 0.227 M C5H5N solution at 25°C. The Kb of C5H5N is 1.7 × 10-9. A) 4.59 B) 9.41 C) 4.71 D) 10.14 E) 9.29
E) 9.29
Which one of the following will form a basic solution in water? A) NaC2H3O2 B) LiCN C) KClO2 D) LiBrO E) All of the above will form basic solutions.
E) All of the above will form basic solutions.
All of the following anions are considered basic EXCEPT A) F-. B) CN-. C) PO43-. D) HPO42-. E) Cl-.
E) Cl-.
Identify the weak diprotic acid. A) CH3COOH B) HCOOH C) H3PO4 D) H2SO4 E) H2CO3
E) H2CO3
What is the conjugate acid of HCO3⁻ ? A) H3O+ B) H2O C) CO32- D) OH⁻ E) H2CO3
E) H2CO3
Which of the following solutions would have the lowest pH? Assume that they are all 0.10 M in acid at 25∘C. The acid is followed by its Ka value. A) HF, 3.5 × 10-4 B) HCN, 4.9 × 10-10 C) HNO2, 4.6 × 10-4 D) HCHO2, 1.8 × 10-4 E) HClO2, 1.1 × 10-2
E) HClO2, 1.1 × 10-2
Give the characteristics of a strong acid. A) ionizes completely in aqueous solutions B) has equilibrium far to the right C) has a polar bond D) has a weaker bond to hydrogen E) all of the above
E) all of the above
Calculate the hydronium ion concentration in an aqueous solution with a pOH of 9.85 at 25°C. A) 7.1 × 10-5 M B) 4.2 × 10-10 M C) 8.7 × 10-10 M D) 6.5 × 10-5 M E) 1.4 × 10-10 M
A) 7.1 × 10-5 M
Calculate the hydroxide ion concentration in an aqueous solution with a pH of 9.85 at 25°C. A) 7.1 × 10-5 M B) 4.2 × 10-10 M C) 8.7 × 10-10 M D) 6.5 × 10-5 M E) 1.4 × 10-10 M
A) 7.1 × 10-5 M
Determine the pH of a 0.580 M KCH3CO2 solution at 25°C. The Ka of CH3CO2H is 1.80 × 10-5. A) 9.25 B) 4.75 C) 7.00 D) 12.5 E) 1.47
A) 9.25
________ is the active component in vinegar. A) CH3COOH B) H2CO3 C) HCOOH D) H3C6H5O7 E) CH3CH2COOH
A) CH3COOH
When dissolved in water, which compound is generally considered to be an Arrhenius acid? A) H NO2 B) KOH C) Li F D) CH3OH
A) H NO2
Identify the acid that is in car batteries. A) H2SO4 B) HNO3 C) H2CO3 D) CH3COOH E) HCl
A) H2SO4
Which of the following is an Arrhenius acid? A) H2SO4 B) NaOH C) NH2CH3 D) CH3CH3 E) More than one of these is an Arrhenius acid.
A) H2SO4
Identify the weakest acid. A) HF B) HCl C) HBr D) HI E) Not enough information is available.
A) HF
Identify the strongest acid. A) HIO4 B) HIO3 C) HIO2 D) HIO E) Not enough information is given.
A) HIO4
Which of the following species is amphoteric? A) HPO4- B) H3O+ C) PO43- D) Cl- E) None of the above are amphoteric.
A) HPO4-
What is the conjugate base of H2PO4⁻ ? A) HPO42- B) PO43- C) H3PO4 D) H3O+ E) OH⁻
A) HPO42-
In a triprotic acid, which Ka has the highest value? A) Ka1 B) Ka2 C) Ka3 D) Kb1 E) Kb2
A) Ka1
Which of the following is a Brønsted-Lowry acid? A) NH4+ B) CI4 C) NH2- D) BF3 E) I2
A) NH4+
A Lewis base A) donates electrons. B) accepts electrons. C) donates a proton. D) accepts a proton. E) donates more than one proton.
A) donates electrons.
Place the following in order of increasing acid strength. HBrO2 HBrO3 HBrO HBrO4 A) HBrO2 < HBrO4 < HBrO < HBrO3 B) HBrO < HBrO2 < HBrO3 < HBrO4 C) HBrO2 < HBrO3 < HBrO4 < HBrO D) HBrO4 < HBrO2 < HBrO3 < HBrO E) HBrO < HBrO4 < HBrO3 < HBrO2
B) HBrO < HBrO2 < HBrO3 < HBrO4
Which of the following solutions would have the highest pH? Assume that they are all 0.10 M in acid at 25∘C. The acid is followed by its Ka value. A) HF, 3.5 × 10-4 B) HCN, 4.9 × 10-10 C) HNO2, 4.6 × 10-4 D) HCHO2, 1.8 × 10-4 E) HClO2, 1.1 × 10-2
B) HCN, 4.9 × 10-10
Which of the following is an Arrhenius base? A) CH3CO2H B) KOH C) CH3OH D) Na F E) More than one of these compounds is an Arrhenius base.
B) KOH
Determine the pH in a 0.235 M NaOH solution. A) 13.76 B) 0.24 C) 13.37 D) 0.63 E) 12
C) 13.37
Calculate the pH for an aqueous solution of acetic acid that contains hydronium ion. A) 4.65 × 10-12 M B) 2.15 × 10-3 M C) 2.67 D) 11.33
C) 2.67
A container of orange juice at 25°C has a hydronium concentration of 1.78 × 10-3M. What is the pH of the juice? A) 1.84 B) 3.31 C) 2.75 D) 11.25 E) 7.00
C) 2.75
Calculate the pOH of a solution that contains 3.9 × 10-4 M H3O⁺ at 25°C. A) 4.41 B) 3.41 C) 10.59 D) 9.59 E) 0.59
C) 10.59
Identify the diprotic acid. A) HNO3 B) HBr C) CH3COOH D) H2SO4 E) HClO4
D) H2SO4
Identify the strongest acid. A) H2O B) H2S C) H2Se D) H2Te E) Not enough information is available.
D) H2Te
Which of the following acids will have the strongest conjugate base? A) HCl B) HClO4 C) HNO3 D) HCN E) HI
D) HCN
Which of the following is a weak acid? A) HClO4 B) H2SO4 C) HBr D) HCN E) HNO3
D) HCN
The stomach excretes ________ to kill microorganisms and to activate enzymes that break down food. A) CH3COOH B) HBr C) LiHCO3 D) HCl E) HNO3
D) HCl
Which of the following species is amphoteric? A) CO32- B) HF C) NH4⁺ D) HPO42- E) None of the above are amphoteric.
D) HPO42-
Which of the following statements is TRUE? A) A strong acid is composed of a proton and an anion that have a very strong attraction for one another. B) A weak base is composed of a cation and an anion with a very weak attraction between them. C) A strong acid has a strong conjugate base. D) The conjugate base of a very weak acid is stronger than the conjugate base of a strong acid. E) None of the above statements are true.
D) The conjugate base of a very weak acid is stronger than the
A solution with a hydroxide ion concentration of 4.15 × 10-6 M is ________ and has a hydrogen ion concentration of ________. A) acidic, 2.41 × 10-8 M B) acidic, 2.41 × 10-9 M C) basic, 2.41 × 10-8 M D) basic, 2.41 × 10-9 M
D) basic, 2.41 × 10-9 M
Which of the following weak acids has the strongest conjugate base? A) acetic acid, Ka = 1.8 × 10-5 B) nitrous acid, Ka = 4.5 × 10-4 C) dihydrogen phosphate ion, Ka = 6.2 × 10-8 D) hydrocyanic acid, Ka = 4.0 × 10-10 E) benzoic acid, Ka = 6.3 × 10-5
D) hydrocyanic acid, Ka = 4.0 × 10-10
Determine the Ka of an acid that has a pH of 4.67 and a concentration of 0.448 M. A) 5.8 × 10-8 B) 3.3 × 10-11 C) 9.9 × 10-5 D) 4.6 × 10-7 E) 1.0 × 10-9
E) 1.0 × 10-9
What is the concentration of hydroxide ions in pure water at 30.0∘C, if Kw at this temperature is 1.47 × 10-14? A) 1.00 × 10-7 M B) 1.30 × 10-7 M C) 1.47 × 10-7 M D) 8.93 × 10-8 M E) 1.21 × 10-7 M
E) 1.21 × 10-7 M
Which of the following bases is the strongest? The base is followed by its Kb. A) (CH3CH2)2NH, 8.6 × 10-4 B) CH3NH2, 4.4 × 10-4 C) C6H5NH2, 4.0 × 10-10 D) NH3, 1.76 × 10-5 E) C5H5N, 1.7 × 10-9
A) (CH3CH2)2NH, 8.6 × 10-4
Determine the [OH⁻] concentration in a 0.169 M Ca(OH)2 solution. A) 0.338 M B) 0.169 M C) 5.92 × 10-14 M D) 2.96 × 10-14 M E) 0.298 M
A) 0.338 M
Calculate the concentration of H3O⁺ in a solution that contains 5.5 × 10-5 M OH⁻ at 25°C. Identify the solution as acidic, basic, or neutral. A) 1.8 × 10-10 M, basic B) 1.8 × 10-10 M, acidic C) 5.5 × 10-10 M, neutral D) 9.2 × 10-1 M, acidic E) 9.2 × 10-1 M, basic
A) 1.8 × 10-10 M, basic
Determine the pOH of a 0.00598 M HClO4 solution. A) 11.777 B) 6.434 C) 7.566 D) 2.223 E) 3.558
A) 11.777
Calculate the hydronium ion concentration in an aqueous solution with a pOH of 4.33 at 25°C. A) 2.1 × 10-10 M B) 9.7 × 10-10 M C) 4.7 × 10-5 M D) 3.8 × 10-5 M E) 6.3 × 10-6 M
A) 2.1 × 10-10 M
Calculate the hydroxide ion concentration in an aqueous solution with a pH of 4.33 at 25°C. A) 2.1 × 10-10 M B) 9.7 × 10-10 M C) 4.7 × 10-5 M D) 3.8 × 10-5 M E) 6.3 × 10-6 M
A) 2.1 × 10-10 M
Determine the pH of a 0.461 M C6H5CO2H M solution if the Ka of C6H5CO2H is 6.5 × 10-5. A) 2.26 B) 4.52 C) 11.74 D) 9.48 E) 5.48
A) 2.26
Calculate the concentration of OH⁻ in a solution that contains 3.9 × 10-4 M H3O⁺ at 25°C. Identify the solution as acidic, basic, or neutral. A) 2.6 × 10-11 M, acidic B) 2.6 × 10-11 M, basic C) 3.9 × 10-4 M, neutral D) 2.7 × 10-2 M, basic E) 2.7 × 10-2 M, acidic
A) 2.6 × 10-11 M, acidic
What is the pH of pure water at 40.0°C if the Kw at this temperature is 2.92 × 10-14? A) 6.767 B) 0.465 C) 7.000 D) 7.233 E) 8.446
A) 6.767
Calculate the concentration of H3O⁺ in a solution that contains 6.25 × 10-9 M OH⁻ at 25°C. Identify the solution as acidic, basic, or neutral. A) 6.38 × 10-9 M, basic B) 1.60 × 10-6 M, acidic C) 7.94 × 10-11 M, acidic D) 7.38 × 10-3 M, basic E) 4.92× 10-5 M, acidic
B) 1.60 × 10-6 M, acidic
Calculate the hydronium ion concentration in an aqueous solution with a pH of 11.7 at 25°C. A) 5.7 × 10-11 M B) 1.9× 10-12 M C) 5.4 × 10-2 M D) 6.4 × 10-7 M E) 9.5× 10-3 M
B) 1.9× 10-12 M
Determine the pOH in a 2.58 × 10-3 M KOH solution. A) 11.4 B) 2.59 C) 9.33 D) 4.67 E) 7.00
B) 2.59
Determine the pOH of a 0.188 M NH3 solution at 25°C. The Kb of NH3 is 1.76 × 10-5. A) 5.480 B) 2.740 C) 8.520 D) 11.260 E) 12.656
B) 2.740
Calculate the pH of a solution that contains 3.9 × 10-5 M H3O⁺ at 25°C. A) 5.41 B) 4.41 C) 9.59 D) 8.59 E) 0.59
B) 4.41
Calculate the pOH of a solution that contains 7.8 × 10-6 M OH⁻ at 25°C. A) 1.28 B) 5.11 C) 12.72 D) 8.89 E) 9.64
B) 5.11
What is the Kw of pure water at 50.0°C, if the pH is 6.630? A) 2.34 × 10-7 B) 5.50 × 10-14 C) 2.13 × 10-14 D) 1.00 × 10-14 E) There is not enough information to calculate the Kw.
B) 5.50 × 10-14
Calculate the pOH of a solution that contains 2.4 × 10-8 M H3O⁺ at 25°C. A) 2.40 B) 6.38 C) 7.62 D) 5.38 E) 8.62
B) 6.38
Determine the Ka of an acid whose 0.294 M solution has a pH of 2.80. A) 1.2 × 10-5 B) 8.5 × 10-6 C) 2.7 D) 4.9 × 10-7 E) 5.4 × 10-3
B) 8.5 × 10-6
________ is found in carbonated beverages due to the reaction of carbon dioxide with water. A) CH3COOH B) H2CO3 C) HCOOH D) H3C6H5O7 E) CH3CH2COOH
B) H2CO3
Which of the following is not a conjugate acid-base pair? A) NH4+/NH3 B) H3O⁺/OH⁻ C) H2SO3/HSO3⁻ D) C2H3O2⁻/HC2H3O2 E) All of the above are conjugate acid-base pairs.
B) H3O⁺/OH⁻
Identify the triprotic acid. A) HNO3 B) H3PO4 C) H2CO3 D) HClO4 E) H2SO4
B) H3PO4
An aqueous solution of ammonia is found to be basic. This observation can be explained by the net ionic equation A) NO3-(aq) + H2O(l) → HNO3(aq) + OH-(aq). B) NH3(aq) + H2O(l) → NH4+(aq) + OH-(aq). C) HNO3(aq) + H2O(l) → NO3-(aq) + H3O+(aq). D) NH4+(aq) + H2O(l) → NH3(aq) + H3O+(aq).
B) NH3(aq) + H2O(l) → NH4+(aq) + OH-(aq).
All of the following cations are considered acidic EXCEPT A) Fe2+ B) Na+ C) Al3+ D) NH4+ E) V2+
B) Na+
Identify the base that is in Drano. A) LiOH B) NaOH C) NaHCO3 D) Li2CO3 E) NH3
B) NaOH
A Lewis acid A) donates electrons. B) accepts electrons. C) donates a proton. D) accepts a proton. E) donates more than one proton.
B) accepts electrons
A solution with a hydrogen ion concentration of 3.25 × 10-5 M is ________ and has a hydroxide ion concentration of ________. A) acidic, 3.08 × 10-9 M B) acidic, 3.08 × 10-10 M C) basic, 3.08 × 10-9 M D) basic, 3.08 × 10-10 M
B) acidic, 3.08 × 10-10 M
Determine the [OH-] concentration of a 0.741 M KOH solution at 25°C. A) 1.34 × 10-13 M B) 1.34 × 10-14 M C) 0.741 M D) 7.41 M E) none of the above
C) 0.741 M
Determine the pH of a 0.023 M HNO3 solution. A) 12.36 B) 3.68 C) 1.64 D) 2.30 E) 2.49
C) 1.64
Determine the pOH in a 0.235 M NaOH solution. A) 13.76 B) 0.24 C) 13.37 D) 0.63 E) 12
D) 0.63
Determine the pH of a solution that is 0.15 M HClO2 (Ka = 1.1 × 10-2) and 0.15 M HClO (Ka = 2.9 × 10-8). A) 4.18 B) 9.82 C) 12.55 D) 1.39 E) 3.55
D) 1.39
Determine the pH of a 0.188 M NH3 solution at 25°C. The Kb of NH3 is 1.76 × 10-5. A) 5.480 B) 2.740 C) 8.520 D) 11.260 E) 12.656
D) 11.260
Determine the Kb for CN⁻ at 25°C. The Ka for HCN is 4.9 × 10-10. A) 4.9 × 10-14 B) 2.3 × 10-9 C) 1.4 × 10-5 D) 2.0 × 10-5 E) 3.7 × 10-7
D) 2.0 × 10-5
Determine the pH of a 0.00598 M HClO4 solution. A) 11.777 B) 6.434 C) 7.566 D) 2.223 E) 3.558
D) 2.223
Determine the pH of a 0.62 M NH4NO3 solution at 25°C. The Kb for NH3 is 1.76 × 10-5. A) 2.48 B) 9.27 C) 11.52 D) 4.73 E) 9.45
D) 4.73
Calculate the pH of a solution that contains 7.8 × 10-6 M OH⁻ at 25°C. A) 1.28 B) 5.11 C) 12.72 D) 8.89 E) 9.64
D) 8.89
Identify the acid that is in vinegar. A) H2SO4 B) HNO3 C) Li2CO3 D) CH3COOH E) HF
D) CH3COOH