Question 1

Which of the following is an Arrhenius acid?

Accepted Answer

A) H2SO4 
B) LiOH 
C) NH2CH3 
D) CH3CH3 
E) NH3 
A) H2SO4 
B) LiOH 
C) NH2CH3 
D) CH3CH3 
E) NH3

Question 2

Which Bronsted-Lowry acid is not considered to be a strong acid in water?

Accepted Answer

A) HBr 
B) HCl  
C) H NO2 
D) H ClO4 
A) HBr 
B) HCl  
C) H NO2 
D) H ClO4

Question 3

Calculate the pH of a 1.60 mol L-1 CH3NH3Cl solution.Kb for methylamine,CH3NH2,is $3.7 \times 10 ^- 4$

Accepted Answer

A) 1.61 
B) 5.18 
C) 8.82 
D) 12.39 
A) 1.61 
B) 5.18 
C) 8.82 
D) 12.39

Question 4

Calculate the molarity of hydroxide ion in an aqueous solution that has a pOH of 3.00.

Accepted Answer

A) 11.00 mol L-1 
B) 1.00 × 10-11 mol L-1 
C) 1.00 × 10-3 mol L-1 
D) 3.00 × 10-14 mol L-1 
E) 1.1 × 10-13 mol L-1 
A) 11.00 mol L-1 
B) 1.00 × 10-11 mol L-1 
C) 1.00 × 10-3 mol L-1 
D) 3.00 × 10-14 mol L-1 
E) 1.1 × 10-13 mol L-1

Question 5

What is the concentration of hydroxide ions in pure water at 30.0 °C if Kw at this temperature is 1.47 × 10-14?

Accepted Answer

A) 1.00 × 10-7 mol L-1 
B) 1.30 × 10-7 mol L-1 
C) 1.47 × 10-7 mol L-1 
D) 8.93 × 10-8 mol L-1 
E) 1.21 × 10-7 mol L-1 
A) 1.00 × 10-7 mol L-1 
B) 1.30 × 10-7 mol L-1 
C) 1.47 × 10-7 mol L-1 
D) 8.93 × 10-8 mol L-1 
E) 1.21 × 10-7 mol L-1

Question 6

Which of the following is TRUE?

Accepted Answer

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) An acidic solution does not contain OH- 
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) An acidic solution does not contain OH-

Question 7

Calculate the pH of a 1.60 mol L-1 KBrO solution.Ka for hypobromous acid,HBrO,is $2.0 \times 10 ^- 9$

Accepted Answer

A) 2.55 
B) 4.25 
C) 9.75 
D) 11.45 
A) 2.55 
B) 4.25 
C) 9.75 
D) 11.45

Question 8

Describe a molecule that can be a Lewis acid.

Accepted Answer

A molecule with an i

Question 9

Determine the pH of a 0.18 mol L-1 H2CO3 solution.Carbonic acid is a diprotic acid whose Ka1 = 4.3 × 10-7 and Ka2 = 5.6 × 10-11.

Accepted Answer

A) 11.00 
B) 10.44 
C) 5.50 
D) 4.31 
E) 3.56 
A) 11.00 
B) 10.44 
C) 5.50 
D) 4.31 
E) 3.56

Question 10

Which of the following is an Arrhenius base?

Accepted Answer

A) CH3CO2H 
B) NaOH 
C) CH3OH 
D) LiCl 
E) H2CO3 
A) CH3CO2H 
B) NaOH 
C) CH3OH 
D) LiCl 
E) H2CO3

Question 11

What is the pH of a 0.40 mol L-1 H2Se solution that has the stepwise dissociation constants Ka1 = 1.3 × 10-4 and $K _ { \mathrm { a } 2 } = 1.0 \times 10 ^{- 11} ?$

Accepted Answer

A) 2.14 
B) 3.89 
C) 4.28 
D) 5.57 
A) 2.14 
B) 3.89 
C) 4.28 
D) 5.57

Question 12

Which of the following is a Lewis base?

Accepted Answer

A) AlF3 
B) H2O 
C) SiF4 
D) C5H12 
E) BH3 
A) AlF3 
B) H2O 
C) SiF4 
D) C5H12 
E) BH3

Question 13

Calculate the hydronium ion concentration in an aqueous solution that contains 2.50 × 10-6 mol L-1 in hydroxide ion.

Accepted Answer

A) 4.00 × 10-7 mol L-1 
B) 4.00 × 10-8 mol L-1 
C) 4.00 × 10-9 mol L-1 
D) 5.00 × 10-9 mol L-1 
A) 4.00 × 10-7 mol L-1 
B) 4.00 × 10-8 mol L-1 
C) 4.00 × 10-9 mol L-1 
D) 5.00 × 10-9 mol L-1

Question 14

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 15

Describe the relationship between molecular structure and acid strength.

Accepted Answer

1)The stronger the bond betwee

Question 16

Which of the following statements is TRUE?

Accepted Answer

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) The dissociation reaction of a weak acid is completely shifted to the right. 
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) The dissociation reaction of a weak acid is completely shifted to the right.

Question 17

The pH of an aqueous solution at 25.0 °C is 10.55.What is the molarity of  $ \mathrm{H}^{+} $ ?

Accepted Answer

A) 2.8 × 10-11 mol L-1 
B) 3.5 × 1010 mol L-1 
C) 3.5 × 10-4 mol L-1 
D) 3.5 mol L-1 
E) 2.36 mol L-1 
A) 2.8 × 10-11 mol L-1 
B) 3.5 × 1010 mol L-1 
C) 3.5 × 10-4 mol L-1 
D) 3.5 mol L-1 
E) 2.36 mol L-1

Question 18

Which one of the following will form a basic solution in water?

Accepted Answer

A) NaBr 
B) LiCN 
C) NaCl 
D) KClO4 
E) NH4Cl 
A) NaBr 
B) LiCN 
C) NaCl 
D) KClO4 
E) NH4Cl

Question 19

Determine the pH of a 0.461 mol L-1 C6H5CO2H solution if the Ka of C6H5CO2H is 6.5 × 10-5.

Accepted Answer

A) 2.26 
B) 4.52 
C) 11.74 
D) 9.48 
E) 5.48 
A) 2.26 
B) 4.52 
C) 11.74 
D) 9.48 
E) 5.48

Question 20

Calculate the pH for an aqueous solution of pyridine that contains $2.15 \times 10 ^{- 4 }\mathrm {~mol} \mathrm {~L} ^ { - 1 }$ hydroxide ion.

Accepted Answer

A) 4.65 × 10-11 
B) 2.15 × 10-4  
C) 3.67 
D) 10.33 
A) 4.65 × 10-11 
B) 2.15 × 10-4  
C) 3.67 
D) 10.33

Exam 15: Acids and Bases

Which of the following is an Arrhenius acid?

Which Bronsted-Lowry acid is not considered to be a strong acid in water?

Calculate the pH of a 1.60 mol L-1 CH3NH3Cl solution.Kb for methylamine,CH3NH2,is 3.7×10−43.7 \times 10 ^- 43.7×10−4

Calculate the molarity of hydroxide ion in an aqueous solution that has a pOH of 3.00.

What is the concentration of hydroxide ions in pure water at 30.0 °C if Kw at this temperature is 1.47 × 10-14?

Which of the following is TRUE?

Calculate the pH of a 1.60 mol L-1 KBrO solution.Ka for hypobromous acid,HBrO,is 2.0×10−92.0 \times 10 ^- 92.0×10−9

Describe a molecule that can be a Lewis acid.

Determine the pH of a 0.18 mol L-1 H2CO3 solution.Carbonic acid is a diprotic acid whose Ka1 = 4.3 × 10-7 and Ka2 = 5.6 × 10-11.

Which of the following is an Arrhenius base?

What is the pH of a 0.40 mol L-1 H2Se solution that has the stepwise dissociation constants Ka1 = 1.3 × 10-4 and Ka2=1.0×10−11?K _ { \mathrm { a } 2 } = 1.0 \times 10 ^{- 11} ?Ka2​=1.0×10−11?

Which of the following is a Lewis base?

Calculate the hydronium ion concentration in an aqueous solution that contains 2.50 × 10-6 mol L-1 in hydroxide ion.

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

Describe the relationship between molecular structure and acid strength.

Which of the following statements is TRUE?

The pH of an aqueous solution at 25.0 °C is 10.55.What is the molarity of H+ \mathrm{H}^{+} H+ ?

Which one of the following will form a basic solution in water?

Determine the pH of a 0.461 mol L-1 C6H5CO2H solution if the Ka of C6H5CO2H is 6.5 × 10-5.

Calculate the pH for an aqueous solution of pyridine that contains 2.15×10−4 mol L−12.15 \times 10 ^{- 4 }\mathrm {~mol} \mathrm {~L} ^ { - 1 }2.15×10−4 mol L−1 hydroxide ion.

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Filters

Calculate the pH of a 1.60 mol L^-1 CH₃NH₃Cl solution.K_b for methylamine,CH₃NH₂,is $3.7 \times 10 ^- 4$

What is the concentration of hydroxide ions in pure water at 30.0 °C if K_w at this temperature is 1.47 × 10^-14?

Calculate the pH of a 1.60 mol L^-1 KBrO solution.K_a for hypobromous acid,HBrO,is $2.0 \times 10 ^- 9$

Determine the pH of a 0.18 mol L^-1 H₂CO₃ solution.Carbonic acid is a diprotic acid whose K_a1 = 4.3 × 10^-7 and K_a2 = 5.6 × 10^-11.

What is the pH of a 0.40 mol L^-1 H₂Se solution that has the stepwise dissociation constants K_a1 = 1.3 × 10^-4 and $K _ { \mathrm { a } 2 } = 1.0 \times 10 ^{- 11} ?$

Calculate the hydronium ion concentration in an aqueous solution that contains 2.50 × 10^-⁶ mol L^-1in hydroxide ion.

The pH of an aqueous solution at 25.0 °C is 10.55.What is the molarity of $\mathrm{H}^{+}$ ?

Determine the pH of a 0.461 mol L^-1 C₆H₅CO₂H solution if the K_a of C₆H₅CO₂H is 6.5 × 10^-5.

Calculate the pH for an aqueous solution of pyridine that contains $2.15 \times 10 ^{- 4 }\mathrm {~mol} \mathrm {~L} ^ { - 1 }$ hydroxide ion.