Q&A Hero

Q: What is the pH of a 0. 40 M H2Se solution that has the stepwise dissociation constants Ka1= 1.3 10-4andKa2= 1.0 10-11? A) 2. 14 B) 3.89 C) 4. 28 D) 5. 57

Q: Calculate the pH of a 0. 60 M H2SO3, solution that has the stepwise dissociation constants Ka1= 1.5 10-2and Ka2= 6.3 10-8. A) 1.02 B) 1.06 C) 1.82 D) 2.04

Q: Calculate the pH of a 0. 080 M carbonic acid solution, H2CO3(aq), that has the stepwise dissociation constants Ka1= 4.3 10-7and Ka2= 5.6 10-11. A) 1.10 B) 3.73 C) 6.37 D) 10.25

Q: Potassium hydrogen phthalate (molar mass = 204.2 g/mol)is one of the most commonly used acids for standardizing solutions containing bases. KHP is a monoprotic weak acid with Ka= 3.91 10-6. Calculate the pH of the solution that results when 0. 50 g of KHP is dissolved in enough water to produce 25.0 mL of solution. A) 2.05 B) 3. 21 C) 4. 40 D) 5.41

Q: What is the hydronium ion concentration of a 0. 150 M hypochlorous acid solution withKa= 3.5 10-8? The equation for the dissociation of hypochlorous acid is:HOCl(aq) + H2O(l) H3O+(aq) + OCl-(aq).A) 1.9 10-4 MB) 7.2 10-4 MC) 2.8 10-5 MD) 7.2 10-5 M

Q: What is the hydronium ion concentration of a 0. 500 M acetic acid solution with Ka= 1.8 10-5? The equation for the dissociation of acetic acid is:CH3CO2H(aq) + H2O(l) H3O+(aq) + CH3CO2-(aq).A) 3.0 10-2MB) 4.2 10-2MC) 3.0 10-3MD) 4.2 10-3M

Q: What is the pH of a solution prepared by mixing 100.00 mL of 0.020 M Ca(OH)2with 50.00 mL of 0. 300 M NaOH? Assume that the volumes are additive. A) 13.05 B) 13.10 C) 13.28 D) 13.58

Q: What is the pH of a solution prepared by mixing 100.00 mL of 0.20 M HCl with 150.00 mL of 0. 10 M HCl? Assume that the volumes are additive. A) 0. 17 B) 0. 52 C) 0. 85 D) 1.70

Q: What is the pH of a solution prepared by diluting 100.00 mL of 0.020 M Ba(OH)2with enough water to produce a total volume of 250.00 mL? A) 1.80 B) 2. 10 C) 11.90 D) 12.20

Q: What is the pH of a solution prepared by diluting 20.00 mL of 0.10 M HCl with enough water to produce a total volume of 100.00 mL? A) 1.00 B) 1. 70 C) 2.00 D) 3.40

Q: What is the pH of a solution prepared by dissolving 0. 45 grams of solid CaO (lime) in enough water to make 2.00 L of aqueous Ca(OH)2(limewater)?CaO(s) + H2O(l) -> Ca2+(aq) + 2 OH-(aq)A) 2.10B) 2.40C) 11.60D) 11.90

Q: What is the pH of a 0.0 40 M Ba(OH)2solution? A) 1.10 B) 1.40 C) 12.60 D) 12.90

Q: What is the hydroxide ion concentration of a lye solution that has a pH of 9.20? A) 6.31 10- 10M B) 1.58 10- 5M C) 4.80 M D) 9.20 M

Q: What is the hydronium ion concentration of an acid rain sample that has a pH of 3. 45? A) 2.82 10-11M B) 3.55 10-4M C) 3. 45 M D) 10. 55 M

Q: What is the hydronium ion concentration and the pH for an aqueous solution of NH3that has a hydroxide ion concentration of 2.25 10-2M? A) 4.44 10- 12M and 2.65 B) 4.44 10- 12M and 11.35 C) 4.44 10- 13M and 1.65 D) 4.44 10- 13M and 12.35

Q: What is the hydroxide ion concentration and the pH for a hydrochloric acid solution that has a hydronium ion concentration of 1.50 10-2M? A) 6.67 10- 12M, 2.82 B) 6.67 10- 12M, 11.18 C) 6.67 10- 13M, 1.82 D) 6.67 10- 13M, 12.17

Q: Calculate the pH for an aqueous solution of acetic acid that contains 2.15 10-3M hydronium ion. A) 4.65 10-12 M B) 2.15 10-3 M C) 2. 67 D) 11. 33

Q: A solution with a hydroxide ion concentration of 4.15 10- 6M is ________ and has a hydrogen ion concentration of ________. A) acidic, 2.41 10- 8M B) acidic, 2.41 10- 9M C) basic, 2.41 10- 8M D) basic, 2.41 10- 9M

Q: A solution with a hydrogen ion concentration of 3.25 10- 6M is ________ and has a hydroxide ion concentration of ________. A) acidic, 3.08 10- 8M B) acidic, 3.08 10- 9M C) basic, 3.08 10- 8M D) basic, 3.08 10- 9M

Q: Calculate the hydroxide ion concentration in an aqueous solution that contains 3.50 10- 4M in hydronium ion. A) 2.86 10- 3M B) 2.86 10- 10M C) 2.86 10- 11M D) 3.50 10- 11M

Q: Calculate the hydronium ion concentration in an aqueous solution that contains 2.50 10- 6M in hydroxide ion. A) 4.00 10- 7M B) 4.00 10- 8M C) 4.00 10- 9M D) 5.00 10- 9M

Q: Which Bronsted-Lowry acid is not considered to be a strong acid in water?A) H IB) H BrC) H2S O3D) HNO3

Q: When dissolved in water, which compound is generally considered to be an Arrhenius acid? A) HNO2 B) KOH C) LiF D) CH3OH

Q: BF3and NH3undergo a Lewis acid-base reaction forming an adduct. Which picture below correctly represents the curved arrow notation for the initial Lewis acid-Lewis base interaction in this reaction; what is the Lewis acid and the Lewis base?A) Picture (1) is correct; NH3is the Lewis acid and BF3is the Lewis base.B) Picture (2) is correct; BF3is the Lewis acid and NH3is the Lewis base.C) Picture (3) is correct; NH3 is the Lewis acid and BF3is the Lewis base.D) Picture (4) is correct; BF3is the Lewis acid and NH3is the Lewis base.

Q: CO2reacts with H2O to form HCO3-and H+. Which picture below correctly represents the curved arrow notation for the initial Lewis acid-Lewis base interaction in this reaction; what is the Lewis acid and the Lewis base? (1) (2) A) Picture (1) is correct; H2O is the Lewis acid and CO2is the Lewis base. B) Picture (1) is correct; CO2is the Lewis acid and H2O is the Lewis base. C) Picture (2) is correct; H2O is the Lewis acid and CO2is the Lewis base. D) Picture (2) is correct; CO2is the Lewis acid and H2O is the Lewis base.

Q: SO3reacts with H2O to form H2SO4. Which picture below correctly represents the curved arrow notation for the initial Lewis acid-Lewis base interaction in this reaction; what is the Lewis acid and the Lewis base? A) Picture (1) is correct; H2O is the Lewis acid and SO3is the Lewis base. B) Picture (1) is correct; SO3is the Lewis acid and H2O is the Lewis base. C) Picture (2) is correct; H2O is the Lewis acid and SO3is the Lewis base. D) Picture (2) is correct; SO3is the Lewis acid and H2O is the Lewis base.

Q: Of the elements indicated on the periodic table shown above, which forms the weakest oxoacid acid with the formula H2XO3or HXO3, where X = A, B, C, or D? A) A B) B C) C D) D

Q: Of the elements indicated on the periodic table shown above, which forms the strongest oxoacid acid with the formula H2XO3or HXO3, where X = A, B, C, or D? A) A B) B C) C D) D

Q: Of the elements indicated on the periodic table shown above, which forms the weakest binary acid, H2X or HX, where X = A, B, C, or D? A) A B) B C) C D) D

Q: Of the elements indicated on the periodic table shown above, which forms the strongest binary acid, H2X or HX, where X = A, B, C, or D? A) A B) B C) C D) D

Q: Which picture represents a basic salt? A) (1) B) (2) C) (3) D) None of these

Q: Which picture represents a neutral salt? A) (1) B) (2) C) (3) D) None of these

Q: Which picture represents an acidic salt? A) (1) B) (2) C) (3) D) None of these

Q: The following pictures represent solutions of three salts NaA (A-= X-, Y-, or Z-); water molecules and Na+ions have been omitted for clarity. Arrange the three A-ions in order of decreasing base strength. A) X-> Y-> Z- B) X-> Z-> Y- C) Y-> Z-> X- D) Z-> Y-> XZ-

Q: Arrange the conjugate bases (A-= X-, Y-, or Z-) in order of increasing value of Kb. A) Kb(Z-) < Kb(Y-) < Kb(X-) B) Kb(Y-) < Kb(Z-) < Kb(X-) C) Kb(Z-) < Kb(X-) < Kb(Y-) D) Kb(X-) < Kb(Z-) < Kb(Y-)

Q: Arrange the conjugate bases (A-= X-, Y-, or Z-) in order of increasing base strength. A) Z-< Y-< X- B) Y-< Z-< X- C) Z-< X-< Y- D) X-< Z-< Y-

Q: Arrange the acids in order of increasing pH. A) HZ < HY < HX B) HY < HZ < HX C) HZ < HX < HY D) HX < HZ < HY

Q: Arrange the acids in order of increasing value of percent dissociation. A) HZ < HY < HX B) HY < HZ < HX C) HZ < HX < HY D) HX < HZ < HY

Q: Arrange the acids in order of increasing value of Ka. A) Ka(HZ) < Ka(HY) < Ka(HX) B) Ka(HY) < Ka(HZ) < Ka(HX) C) Ka(HZ) < Ka(HX) < Ka(HY) D) Ka(HX) < Ka(HZ) < Ka(HY)

Q: Arrange the acids in order of increasing acid strength. A) HZ < HY < HX B) HY < HZ < HX C) HZ < HX < HY D) HX < HZ < HY

Q: Which of the above pictures represents a solution of a diprotic acid H2A for which Ka1= ï‚¥and Ka2is exceptionally small. (Water molecules have been omitted for clarity.) A) picture (a) B) picture (b) C) picture (c) D) picture (d)

Q: Which of the above pictures represents a solution of a weak diprotic acid H2A for which Ka1>> Ka2? (Water molecules have been omitted for clarity.) A) picture (a) B) picture (b) C) picture (c) D) picture (d)

Q: Which acid solution has the lowestpH? A) HX B) HY C) HZ D) All have the same pH.

Q: Which acid has the lowestpercent dissociation? A) HX B) HY C) HZ D) All have the same percent dissociation.

Q: Which acid has the smallestvalue of Ka? A) HX B) HY C) HZ D) All have the same Kavalue.

Q: Which acid, if any, is a strong acid? A) All are strong acids. B) HX and HZ C) HY D) None are strong acids.

Q: Arrange the three acids in order of increasing acid strength. A) HZ < HY < HX B) HY < HZ < HX C) HZ < HX < HY D) HX < HZ < HY

Q: Identify the Br∅nsted-Lowry acid/base conjugate pairs. A) (1)/(2) and (3)/(4) B) (1)/(3) and (2)/(4) C) (1)/(4) and (2)/(3)

Q: Identify the Bronsted-Lowry acid/base conjugate pairs.A) (1)/(2) and (3)/(4)B) (1)/(3) and (2)/(4)C) (1)/(4) and (2)/(3)

Q: Identify the Bronsted-Lowry bases.A) (1) and (3)B) (1) and (4)C) (2) and (3)D) (2) and (4)

Q: Identify the Br∅nsted-Lowry acids. A) (1) and (3) B) (1) and (4) C) (2) and (3) D) (2) and (4)

Q: Identify the Bronsted-Lowry bases.A) (1) and (3)B) (1) and (4)C) (2) and (3)D) (2) and (4)

Q: Identify the Bronsted-Lowry acids.A) (1) and (3)B) (1) and (4)C) (2) and (3)D) (2) and (4)

Q: Which one of the following is expected to be the strongest Lewis acid? A) Fe B) Fe+ C) Fe2+ D) Fe3+

Q: Identify the set of Lewis acids. A) BH3, BF3, Cu2+, CO2 B) Cl-, OH-, NH3, H2O C) H3PO4, H2PO4-, HPO42-, PO43- D) CH3-, NH2-, OH-, F-

Q: The compound BF3can be described as a(n) ________.A) Arrhenius acidB) Bronsted-Lowry acidC) Lewis acidD) Lewis base

Q: Which one of the following is leastable to behave as a Lewis base? A) CH3NH2 B) (CH3)2NH C) (CH3)3N D) (CH3)3NH+

Q: Which one of the following is notconsidered to be a Lewis base? A) H2O B) NH3 C) NH4+ D) Cl-

Q: For Cu2+and CO2, which will behave as a Lewis acid toward OH-in water? A) only Cu2+ B) only CO2 C) Cu2+and CO2 D) neither Cu2+nor CO2

Q: Identify the Lewis acid that acts as a reactant in the following reaction.Co(H2O)63+(aq) + 6 NH3(aq) -> Co(NH3)63+(aq) + 6 H2O(l)A) Co(H2O)63+B) Co3+C) NH3D) H2O

Q: Identify the Lewis acid that acts as a reactant in the following reaction.Fe(H2O)63+(aq) + 6 CN-(aq) -> Fe(CN)63-(aq) + 6 H2O(l)A) Fe3+B) H2OC) CN-D) Fe(H2O)63+

Q: What is the strongest acid among the following? A) CH3CO2H B) ClCH2CO2H C) Cl2CHCO2H D) Cl3CCO2H

Q: What is the strongest acid among the following? A) HIO B) HIO2 C) HIO3 D) HIO4

Q: What is the strongest acid of the following? A) HOI B) HOBr C) HOCl D) All are equivalent.

Q: What is the strongest acid among the following? A) H2SO3 B) H2SO4 C) H2SeO3 D) H2SeO4

Q: What is the strongest base among the following? A) ClO- B) ClO2- C) ClO3- D) ClO4-

Q: Which acid of the following set has the strongest conjugate base? A) CH4 B) NH3 C) H2O D) HF

Q: What is the weakest acid among the following? A) SiH4 B) PH3 C) H2S D) HCl

Q: What is the strongest acid among the following? A) HF B) HCl C) H2O D) H2S

Q: What is the strongest acid among the following? A) H2O B) H2S C) H2Se D) H2Te

Q: What is the strongest acid among the following? A) HF B) HCl C) HBr D) HI

Q: What is the identity of M in the hydrate M(H2O)6n+that has the 0.10 M solution with the highest pH? A) Li+ B) Na+ C) Mg2+ D) Al3+

Q: What is the identity of M in the hydrate M(H2O)6n+that has the 0.10 M solution with the lowestpH? A) Li+ B) Na+ C) Mg2+ D) Al3+

Q: Which one of the following salts, when dissolved in water, produces the solution with the lowestpH? A) NaCl B) NH4Cl C) MgCl2 D) AlCl3

Q: Equal volumes of 0.10 M NH3(Kb= 1.8 10-5) and 0.10 M HCN (Ka= 4.9 10-10) are mixed together. Will the resulting solution be acidic, basic, or neutral? A) acidic B) basic C) neutral D) insufficient information to solve

Q: Calculate the pH of a 0.100 M CH3NH3Cl solution. Kbfor methylamine, CH3NH2, is 3.7 10-4. A) 2.22 B) 5.78 C) 8.22 D) 11.78

Q: Calculate the pH of a of 0.100 M KBrO solution. Kafor hypobromous acid, HBrO, is 2.0 10-9. A) 3.15 B) 4.85 C) 9.15 D) 10.85

Q: Calculate the pH of a 0.100 M NaCH3CO2solution. Kafor acetic acid, CH3CO2H, is 1.8 10-5. A) 2.87 B) 5.13 C) 8.87 D) 11.13

Q: Which one of the following salts, when dissolved in water, produces the solution with a pH closestto 7.00? A) NH4Cl B) BaO C) NaHSO4 D) RbI

Q: Which one of the following salts, when dissolved in water, produces the solution with the highestpH? A) KI B) KBr C) KCl D) KF