Question 1

Which of the following solutions would have the most basic pH? Assume that they are all 0.10 M in acid at 25∘C.The acid is followed by its Ka value.

Accepted Answer

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 
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

Question 2

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)

Accepted Answer

A) 3.0 × 10-2 M 
B) 4.2 × 10-2 M 
C) 3.0 × 10-3 M 
D) 4.2 × 10-3 M 
A) 3.0 × 10-2 M 
B) 4.2 × 10-2 M 
C) 3.0 × 10-3 M 
D) 4.2 × 10-3 M

Question 3

What is the pH of a 0.30 M pyridine solution that has Kb = 1.9 × 10-9? The equation for the dissociation of pyridine is:
C5H5N(aq)+ H2O(l)⇌ C5H5NH+(aq)+ OH-(aq)

Accepted Answer

A) 4.62 
B) 8.72 
C) 9.38 
D) 10.38 
A) 4.62 
B) 8.72 
C) 9.38 
D) 10.38

Question 4

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) None of the above statements are 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.

Question 5

What is the autoionization of water?

Accepted Answer

Autoionization of water is the equilibri

Question 6

Match the following.
-Arrhenius acid

Accepted Answer

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

Question 7

A solution with a hydroxide ion concentration of 4.15 × 10-6 M is ________ and has a hydrogen ion concentration of ________.

Accepted Answer

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 
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

Question 8

Determine the pH of a 0.188 M NH3 solution at 25°C.The Kb of NH3 is 1.76 × 10-5.

Accepted Answer

A) 5.480 
B) 2.740 
C) 8.520 
D) 11.260 
E) 12.656 
A) 5.480 
B) 2.740 
C) 8.520 
D) 11.260 
E) 12.656

Question 9

What is the conjugate base of H2PO4⁻?

Accepted Answer

A) HPO42- 
B) PO43- 
C) H3PO4 
D) H3O+ 
E) OH⁻ 
A) HPO42- 
B) PO43- 
C) H3PO4 
D) H3O+ 
E) OH⁻

Question 10

Calculate the pH of a solution that contains 3.9 × 10-4 M H3O⁺ at 25°C.

Accepted Answer

A) 4.59 
B) 3.41 
C) 10.59 
D) 9.41 
E) 0.59 
A) 4.59 
B) 3.41 
C) 10.59 
D) 9.41 
E) 0.59

Question 11

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

Accepted Answer

A) NaCl 
B) KCl 
C) MgCl2 
D) AlCl3 
A) NaCl 
B) KCl 
C) MgCl2 
D) AlCl3

Question 12

Determine the pH of a 0.116 M Ba(OH)2 solution at 25°C.

Accepted Answer

A) 8.62 
B) 13.06 
C) 13.37 
D) 0.63 
E) 12.56 
A) 8.62 
B) 13.06 
C) 13.37 
D) 0.63 
E) 12.56

Question 13

Give the characteristics of a strong acid.

Accepted Answer

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. 
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.

Question 14

Calculate the hydroxide ion concentration in an aqueous solution that contains 3.50 × 10-4 M in hydronium ion.

Accepted Answer

A) 2.86 × 10-3 M 
B) 2.86 × 10-10 M 
C) 2.86 × 10-11 M 
D) 3.50 × 10-11 M 
A) 2.86 × 10-3 M 
B) 2.86 × 10-10 M 
C) 2.86 × 10-11 M 
D) 3.50 × 10-11 M

Question 15

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:
NH3(aq)+ H2O(l)⇌ NH4+(aq)+ OH-(aq)

Accepted Answer

A) 3.0 M 
B) 0.056 M 
C) 1.8 × 10-2 M 
D) 1.0 × 10-3 M 
A) 3.0 M 
B) 0.056 M 
C) 1.8 × 10-2 M 
D) 1.0 × 10-3 M

Question 16

Calculate the pH of a 1.60 M CH3NH3Cl solution.Kb for methylamine,CH3NH2,is 3.7× 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 17

A 7.0 × 10-3 M aqueous solution of Ca(OH)2 at 25.0°C has a pH of ________.

Accepted Answer

A) 12.15 
B) 1.85 
C) 1.4 × 10-2 
D) 7.1 × 10-13 
E) 11.85 
A) 12.15 
B) 1.85 
C) 1.4 × 10-2 
D) 7.1 × 10-13 
E) 11.85

Question 18

Identify the strongest acid.

Accepted Answer

A) HF 
B) HBr 
C) HI 
D) HCl 
E) Not enough information is given. 
A) HF 
B) HBr 
C) HI 
D) HCl 
E) Not enough information is given.

Question 19

The acid-dissociation constant at 25.0°C for hypochlorous acid (HClO)is 3.0 × 10-8.At equilibrium,the molarity of H3O+ in a 0.010 M solution of HClO is ________.

Accepted Answer

A) 1.7 × 10-5 
B) 0.010 
C) 5.8 × 10-10 
D) 4.76 
E) 2.00 
A) 1.7 × 10-5 
B) 0.010 
C) 5.8 × 10-10 
D) 4.76 
E) 2.00

Question 20

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

Which of the following solutions would have the most basic pH? Assume that they are all 0.10 M in acid at 25^∘C.The acid is followed by its K_a value.

What is the hydronium ion concentration of a 0.500 M acetic acid solution with K_a = 1.8 × 10^-5? The equation for the dissociation of acetic acid is: CH₃CO₂H(aq)+ H₂O(l)⇌ H₃O⁺(aq)+ CH₃CO₂^-(aq)

What is the pH of a 0.30 M pyridine solution that has K_b = 1.9 × 10^-9? The equation for the dissociation of pyridine is: C₅H₅N(aq)+ H₂O(l)⇌ C₅H₅NH⁺(aq)+ OH^-(aq)

Which of the following statements is true?

What is the autoionization of water?

Match the following. -Arrhenius acid

A solution with a hydroxide ion concentration of 4.15 × 10^-6 M is and has a hydrogen ion concentration of .

Determine the pH of a 0.188 M NH₃ solution at 25°C.The K_bof NH₃ is 1.76 × 10^-5.

What is the conjugate base of H₂PO₄^⁻?

Calculate the pH of a solution that contains 3.9 × 10^-4 M H₃O^⁺ at 25°C.

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

Determine the pH of a 0.116 M Ba(OH)₂ solution at 25°C.

Give the characteristics of a strong acid.

Calculate the hydroxide ion concentration in an aqueous solution that contains 3.50 × 10^-4 M in hydronium ion.

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: NH₃(aq)+ H₂O(l)⇌ NH₄⁺(aq)+ OH^-(aq)

Calculate the pH of a 1.60 M CH₃NH₃Cl solution.K_b for methylamine,CH₃NH₂,is 3.7× 10^-4.

A 7.0 × 10^-3 M aqueous solution of Ca(OH)₂ at 25.0°C has a pH of ________.

Identify the strongest acid.

The acid-dissociation constant at 25.0°C for hypochlorous acid (HClO)is 3.0 × 10^-⁸.At equilibrium,the molarity of H₃O⁺ in a 0.010 M solution of HClO is ________.

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

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Exam 15: Acids and Bases

Which of the following solutions would have the most basic pH? Assume that they are all 0.10 M in acid at 25∘C.The acid is followed by its Ka value.

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)

What is the pH of a 0.30 M pyridine solution that has Kb = 1.9 × 10-9? The equation for the dissociation of pyridine is: C5H5N(aq)+ H2O(l)⇌ C5H5NH+(aq)+ OH-(aq)

Which of the following statements is true?

What is the autoionization of water?

Match the following. -Arrhenius acid

A solution with a hydroxide ion concentration of 4.15 × 10-6 M is ________ and has a hydrogen ion concentration of ________.

Determine the pH of a 0.188 M NH3 solution at 25°C.The Kb of NH3 is 1.76 × 10-5.

What is the conjugate base of H2PO4⁻?

Calculate the pH of a solution that contains 3.9 × 10-4 M H3O⁺ at 25°C.

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

Determine the pH of a 0.116 M Ba(OH)2 solution at 25°C.

Give the characteristics of a strong acid.

Calculate the hydroxide ion concentration in an aqueous solution that contains 3.50 × 10-4 M in hydronium ion.

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: NH3(aq)+ H2O(l)⇌ NH4+(aq)+ OH-(aq)

Calculate the pH of a 1.60 M CH3NH3Cl solution.Kb for methylamine,CH3NH2,is 3.7× 10-4.

A 7.0 × 10-3 M aqueous solution of Ca(OH)2 at 25.0°C has a pH of ________.

Identify the strongest acid.

The acid-dissociation constant at 25.0°C for hypochlorous acid (HClO)is 3.0 × 10-8.At equilibrium,the molarity of H3O+ in a 0.010 M solution of HClO is ________.

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

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Thermochemistry

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Which of the following solutions would have the most basic pH? Assume that they are all 0.10 M in acid at 25^∘C.The acid is followed by its K_a value.

What is the hydronium ion concentration of a 0.500 M acetic acid solution with K_a = 1.8 × 10^-5? The equation for the dissociation of acetic acid is: CH₃CO₂H(aq)+ H₂O(l)⇌ H₃O⁺(aq)+ CH₃CO₂^-(aq)

What is the pH of a 0.30 M pyridine solution that has K_b = 1.9 × 10^-9? The equation for the dissociation of pyridine is: C₅H₅N(aq)+ H₂O(l)⇌ C₅H₅NH⁺(aq)+ OH^-(aq)

A solution with a hydroxide ion concentration of 4.15 × 10^-6 M is and has a hydrogen ion concentration of .

Determine the pH of a 0.188 M NH₃ solution at 25°C.The K_bof NH₃ is 1.76 × 10^-5.

What is the conjugate base of H₂PO₄^⁻?

Calculate the pH of a solution that contains 3.9 × 10^-4 M H₃O^⁺ at 25°C.

Determine the pH of a 0.116 M Ba(OH)₂ solution at 25°C.

Calculate the hydroxide ion concentration in an aqueous solution that contains 3.50 × 10^-4 M in hydronium ion.

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: NH₃(aq)+ H₂O(l)⇌ NH₄⁺(aq)+ OH^-(aq)

Calculate the pH of a 1.60 M CH₃NH₃Cl solution.K_b for methylamine,CH₃NH₂,is 3.7× 10^-4.

A 7.0 × 10^-3 M aqueous solution of Ca(OH)₂ at 25.0°C has a pH of ________.

The acid-dissociation constant at 25.0°C for hypochlorous acid (HClO)is 3.0 × 10^-⁸.At equilibrium,the molarity of H₃O⁺ in a 0.010 M solution of HClO is ________.