Chem 102 Final Acids and Bases

Calculate the pOH in an aqueous solution with a pH of 9.85 at 25°C. A) 2.15 B) 3.15 C) 4.15 D) 5.15 E) 4.00

C) 4.15

Which of the following is TRUE? A) A neutral solution contains [H2O] = [H3O⁺] B) An 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⁻]

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

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

What is the conjugate acid of HCO3⁻ ? A) H3O+ B) H2O C) CO32- D) OH⁻ E) H2CO3

E) H2CO3

Which of the following acids is the STRONGEST? 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 a very electronegative atom attached to the oxygen C) has a polar bond D) has a weaker bond to hydrogen E) all of the above

E) all of the above

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

Which of the following is a Lewis acid? A) BCl3 B) CH4 C) NH3 D) CHCl3 E) None of the above are Lewis acids.

A) BCl3

Identify the weakest acid. A) HF B) HCl C) HBr D) HI E) not enough information is available

A) HF

Which of the following is a Bronsted-Lowry acid? A) NH4+ B) CH4 C) NH2- D) NH3 E) Br2

A) NH4+

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

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

Identify the strongest acid. A) H2O B) H2S C) H2Se D) H2Te E) not enough information is available

D) H2Te

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 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

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 pH of a 0.461 M C6H5CO2H M solution if the Ka of C6H5CO2H is 6.5 x 10-5. A) 2.26 B) 4.52 C) 11.74 D) 9.48 E) 5.48

A) 2.26

Calculate the pOH of a solution that contains 3.9 x 10-4 M H3O⁺ at 25°C. A) 4.59 B) 3.31 C) 10.59 D) 9.14 E) 0.59

C) 10.59

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