Question 1

Which one of the following salts, when dissolved in water, produces the solution with the highest pH?

Accepted Answer

A)  RbI 
B)  RbBr 
C)  RbCl 
D)  RbF 
A)  RbI 
B)  RbBr 
C)  RbCl 
D)  RbF

Question 2

If an equal number of moles of the weak acid HCN  and the strong base KOH are added to water, is the resulting solution acidic, basic, or neutral?

Accepted Answer

A)  acidic 
B)  basic 
C)  neutral 
D)  Depends on the solution volume 
A)  acidic 
B)  basic 
C)  neutral 
D)  Depends on the solution volume

Question 3

Match the following.
-Arrhenius acid

Accepted Answer

A) electron pair donor 
B) produces protons in aqueous solution 
C) electron pair acceptor 
D) proton acceptor 
E) produces hydroxide ions in aqueous solution
F)proton donor 
A) electron pair donor 
B) produces protons in aqueous solution 
C) electron pair acceptor 
D) proton acceptor 
E) produces hydroxide ions in aqueous solution
F)proton donor

Question 4

The base-dissociation constant of ethylamine 
(C2H5NH2) is 6.4 × 10-4at 25.0 °C. The [   ] in a 1.7 × 10-2 
mol L-1 solution of ethylamine is ________ mol L-1.

Accepted Answer

A)  1.1 × 10-5 
B)  11.48 
C)  3.3 × 10-3 
D)  3.0 × 10-3 
E)  3.3 × 10-12 
A)  1.1 × 10-5 
B)  11.48 
C)  3.3 × 10-3 
D)  3.0 × 10-3 
E)  3.3 × 10-12

Question 5

The stronger the acid, ________.

Accepted Answer

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)  the stronger the conjugate acid-base pair 
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)  the stronger the conjugate acid-base pair

Question 6

Which of the following bases is the strongest? The base is followed by its Kb.

Accepted Answer

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 
B)  CH3NH2, 4.4 × 10-4 
C)  C6H5NH2, 4.0 × 10-10 
D)  NH3, 1.76 × 10-5 
E)  C5H5N, 1.7 × 10-9

Question 7

Which one of the following salts, when dissolved in water, produces the solution with a pH closest to 7.00?

Accepted Answer

A)  NH4ClO4 
B)  NaO 
C)  Na CO3 
D)  K I 
A)  NH4ClO4 
B)  NaO 
C)  Na CO3 
D)  K I

Question 8

Which of the following is the correct definition of Lewis acids and bases?

Accepted Answer

A)  A Lewis acid is an electron acceptor while a Lewis base is an electron donor. 
B)  A Lewis acid is an electron pair donor while a Lewis base is an electron pair acceptor. 
C)  A Lewis acid is an electron donor while a Lewis base is an electron acceptor. 
D)  A Lewis acid is an electron pair acceptor while a Lewis base is a proton donor. 
E)  A Lewis acid is an electron pair acceptor while a Lewis base is an electron pair donor. 
A)  A Lewis acid is an electron acceptor while a Lewis base is an electron donor. 
B)  A Lewis acid is an electron pair donor while a Lewis base is an electron pair acceptor. 
C)  A Lewis acid is an electron donor while a Lewis base is an electron acceptor. 
D)  A Lewis acid is an electron pair acceptor while a Lewis base is a proton donor. 
E)  A Lewis acid is an electron pair acceptor while a Lewis base is an electron pair donor.

Question 9

Which of the following is the correct Arrhenius definition of acids?

Accepted Answer

A)  An acid is a substance that produces H+ ions in aqueous solutions. 
B)  An acid is a substance that reacts with H+ ions in aqueous solutions. 
C)  An acid is a substance that produces OH- ions in aqueous solutions. 
D)  An acid is a substance that decreases the amount of H+ ions in aqueous solutions. 
E)  An acid is a substance that does not alter the amount of H+ ions in aqueous solutions. 
A)  An acid is a substance that produces H+ ions in aqueous solutions. 
B)  An acid is a substance that reacts with H+ ions in aqueous solutions. 
C)  An acid is a substance that produces OH- ions in aqueous solutions. 
D)  An acid is a substance that decreases the amount of H+ ions in aqueous solutions. 
E)  An acid is a substance that does not alter the amount of H+ ions in aqueous solutions.

Question 10

Determine the ammonia concentration of an aqueous solution that has a pH of 11. 00. The equation for the dissociation of NH3 (Kb = 1.8 × 10-5) is below:

Accepted Answer

A)  3.0 mol L-1 
B)  0. 056 mol L-1 
C)  1.8 × 10-2 mol L-1 
D)  1.0 × 10-3 mol L-1 
A)  3.0 mol L-1 
B)  0. 056 mol L-1 
C)  1.8 × 10-2 mol L-1 
D)  1.0 × 10-3 mol L-1

Question 11

What is the conjugate acid of HCO3⁻ ?

Accepted Answer

A)  H3O+ 
B)  H2O 
C)  CO32- 
D)  OH⁻ 
E)  H2CO3 
A)  H3O+ 
B)  H2O 
C)  CO32- 
D)  OH⁻ 
E)  H2CO3

Question 12

Which one of the following salts, when dissolved in water, produces the solution with the highest pH?

Accepted Answer

A)  NaH CO3 
B)  KClO4 
C)  Na2CO3 
D)  CH3NH3Cl  
A)  NaH CO3 
B)  KClO4 
C)  Na2CO3 
D)  CH3NH3Cl

Question 13

Which of the following is a weak base?

Accepted Answer

A)  NH(CH3)2 
B)  N2 
C)  NaOH 
D)  CH2CH2 
E)  Ca(OH)2 
A)  NH(CH3)2 
B)  N2 
C)  NaOH 
D)  CH2CH2 
E)  Ca(OH)2

Question 14

Which of the following increases the strength of an oxo acid, HYOn?

Accepted Answer

A)  increasing the electron affinity of Y and increasing the number of oxygen atoms, n 
B)  decreasing the electron affinity of Y and increasing the number of oxygen atoms, n 
C)  increasing the electron affinity of Y and decreasing the number of oxygen atoms, n 
D)  decreasing the electron affinity of Y and decreasing the number of oxygen atoms, n 
E)  none of the above 
A)  increasing the electron affinity of Y and increasing the number of oxygen atoms, n 
B)  decreasing the electron affinity of Y and increasing the number of oxygen atoms, n 
C)  increasing the electron affinity of Y and decreasing the number of oxygen atoms, n 
D)  decreasing the electron affinity of Y and decreasing the number of oxygen atoms, n 
E)  none of the above

Question 15

Identify the strongest acid.

Accepted Answer

A)  H2O 
B)  H2S 
C)  H2Se 
D)  H2Te 
E)  CaH2 
A)  H2O 
B)  H2S 
C)  H2Se 
D)  H2Te 
E)  CaH2

Question 16

Calculate the hydroxide ion concentration in an aqueous solution with a pH of 9.85 at 25 °C.

Accepted Answer

A)  7.1 × 10-5 mol L-1 
B)  4.2 × 10-10 mol L-1 
C)  8.7 × 10-10 mol L-1 
D)  6.5 × 10-5 mol L-1 
E)  1.4 × 10-10 mol L-1 
A)  7.1 × 10-5 mol L-1 
B)  4.2 × 10-10 mol L-1 
C)  8.7 × 10-10 mol L-1 
D)  6.5 × 10-5 mol L-1 
E)  1.4 × 10-10 mol L-1

Question 17

Calculate the concentration of H3O⁺ in a solution that contains 5.5 × 10-5 mol L-1 OH⁻ at 25 °C. Also identify the solution as acidic, basic, or neutral.

Accepted Answer

A)  1.8 × 10-10 mol L-1, basic 
B)  1.8 × 10-10 mol L-1, acidic 
C)  5.5 × 10-10 mol L-1, neutral 
D)  9.2 × 10-1 mol L-1, acidic 
E)  9.2 × 10-1 mol L-1, basic 
A)  1.8 × 10-10 mol L-1, basic 
B)  1.8 × 10-10 mol L-1, acidic 
C)  5.5 × 10-10 mol L-1, neutral 
D)  9.2 × 10-1 mol L-1, acidic 
E)  9.2 × 10-1 mol L-1, basic

Question 18

Which of the following acids will have the strongest conjugate base?

Accepted Answer

A)  HCl 
B)  HClO4 
C)  HNO3 
D)  HCN 
E)  HI 
A)  HCl 
B)  HClO4 
C)  HNO3 
D)  HCN 
E)  HI

Question 19

Identify the Lewis acid, Lewis base, and Lewis acid-base adduct in the following equation: (C2H5)2O + BF3 ⇌ (C2H5)2O:BF3

Accepted Answer

A)  (C2H5)2O is a Lewis base, BF3 is a Lewis acid, and (C2H5)2O:BF3 is a Lewis acid-base adduct. 
B)  (C2H5)2O is a Lewis acid, BF3 is a Lewis base, and (C2H5)2O:BF3 is a Lewis acid-base adduct. 
C)  (C2H5)2O is a Lewis acid-base adduct, BF3 is a Lewis acid, and (C2H5)2O:BF3 is a Lewis base. 
D)  (C2H5)2O is a Lewis base, BF3 is a Lewis acid-base adduct, and (C2H5)2O:BF3 is a Lewis acid adduct. 
E)  (C2H5)2O and BF3 are both Lewis acid-base adducts and (C2H5)2O:BF3 is a Lewis acid. 
A)  (C2H5)2O is a Lewis base, BF3 is a Lewis acid, and (C2H5)2O:BF3 is a Lewis acid-base adduct. 
B)  (C2H5)2O is a Lewis acid, BF3 is a Lewis base, and (C2H5)2O:BF3 is a Lewis acid-base adduct. 
C)  (C2H5)2O is a Lewis acid-base adduct, BF3 is a Lewis acid, and (C2H5)2O:BF3 is a Lewis base. 
D)  (C2H5)2O is a Lewis base, BF3 is a Lewis acid-base adduct, and (C2H5)2O:BF3 is a Lewis acid adduct. 
E)  (C2H5)2O and BF3 are both Lewis acid-base adducts and (C2H5)2O:BF3 is a Lewis acid.

Question 20

Determine the [OH⁻] concentration in a 0.235 mol L-1 NaOH solution.

Accepted Answer

A)  4.25 × 10-14 mol L-1 
B)  0.470 mol L-1 
C)  2.13 × 10-14 mol L-1 
D)  0.198 mol L-1 
E)  0.235 mol L-1 
A)  4.25 × 10-14 mol L-1 
B)  0.470 mol L-1 
C)  2.13 × 10-14 mol L-1 
D)  0.198 mol L-1 
E)  0.235 mol L-1

Exam 15: Acids and Bases

Which one of the following salts, when dissolved in water, produces the solution with the highest pH?

If an equal number of moles of the weak acid HCN and the strong base KOH are added to water, is the resulting solution acidic, basic, or neutral?

Match the following. -Arrhenius acid

The base-dissociation constant of ethylamine (C2H5NH2) is 6.4 × 10-4at 25.0 °C. The [ ] in a 1.7 × 10-2 mol L-1 solution of ethylamine is ________ mol L-1.

The stronger the acid, ________.

Which of the following bases is the strongest? The base is followed by its Kb.

Which one of the following salts, when dissolved in water, produces the solution with a pH closest to 7.00?

Which of the following is the correct definition of Lewis acids and bases?

Which of the following is the correct Arrhenius definition of acids?

Determine the ammonia concentration of an aqueous solution that has a pH of 11. 00. The equation for the dissociation of NH3 (Kb = 1.8 × 10-5) is below:

What is the conjugate acid of HCO3⁻ ?

Which one of the following salts, when dissolved in water, produces the solution with the highest pH?

Which of the following is a weak base?

Which of the following increases the strength of an oxo acid, HYOn?

Identify the strongest acid.

Calculate the hydroxide ion concentration in an aqueous solution with a pH of 9.85 at 25 °C.

Calculate the concentration of H3O⁺ in a solution that contains 5.5 × 10-5 mol L-1 OH⁻ at 25 °C. Also identify the solution as acidic, basic, or neutral.

Which of the following acids will have the strongest conjugate base?

Identify the Lewis acid, Lewis base, and Lewis acid-base adduct in the following equation: (C2H5)2O + BF3 ⇌ (C2H5)2O:BF3

Determine the [OH⁻] concentration in a 0.235 mol L-1 NaOH solution.

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Filters

The base-dissociation constant of ethylamine (C₂H₅NH₂) is 6.4 × 10^-4at 25.0 °C. The [ ] in a 1.7 × 10^-2 mol L^-1solution of ethylamine is ________ mol L^-1.

Which of the following bases is the strongest? The base is followed by its K_b.

Determine the ammonia concentration of an aqueous solution that has a pH of 11. 00. The equation for the dissociation of NH₃ (K_b= 1.8 × 10^-5) is below:

What is the conjugate acid of HCO₃⁻ ?

Which of the following increases the strength of an oxo acid, HYO_n?

Calculate the concentration of H₃O⁺ in a solution that contains 5.5 × 10^-5 mol L^-1 OH⁻ at 25 °C. Also identify the solution as acidic, basic, or neutral.

Identify the Lewis acid, Lewis base, and Lewis acid-base adduct in the following equation: (C₂H₅)₂O + BF₃ ⇌ (C₂H₅)₂O:BF₃

Determine the [OH⁻] concentration in a 0.235 mol L^-1 NaOH solution.