Question 1

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

Accepted Answer

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

Question 2

Which of the following is not a conjugate acid-base pair?

Accepted Answer

A) NH4+/NH3 
B) H3O⁺/OH⁻ 
C) H2SO3/HSO3⁻ 
D) C2H3O2⁻/HC2H3O2 
E) All of the above are conjugate acid-base pairs. 
A) NH4+/NH3 
B) H3O⁺/OH⁻ 
C) H2SO3/HSO3⁻ 
D) C2H3O2⁻/HC2H3O2 
E) All of the above are conjugate acid-base pairs.

Question 3

Give the pH of 0.330 M phosphoric acid.For phosphoric acid,Ka1 = 7.5 × 10-3,Ka2 = 6.2 × 10-8,and Ka3 = 4.2 × 10-13.

Accepted Answer

A) 1.30 
B) 3.84 
C) 6.43 
D) 2.61 
E) 5.68 
A) 1.30 
B) 3.84 
C) 6.43 
D) 2.61 
E) 5.68

Question 4

Determine the pOH of a 0.227 M C5H5N solution at 25°C.The Kb of C5H5N is 1.7 × 10-9.

Accepted Answer

A) 4.59 
B) 9.41 
C) 4.71 
D) 10.14 
E) 9.29 
A) 4.59 
B) 9.41 
C) 4.71 
D) 10.14 
E) 9.29

Question 5

Match the following.
-Br∅nsted-Lowry base

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 6

Determine the [H3O⁺] in a 0.265 M HClO solution.The Ka of HClO is 2.9 × 10-8.

Accepted Answer

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 
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

Question 7

Which of the following is an Arrhenius acid?

Accepted Answer

A) H2SO4 
B) LiOH 
C) NH2CH3 
D) CH3CH3 
E) More than one of these is an Arrhenius acid. 
A) H2SO4 
B) LiOH 
C) NH2CH3 
D) CH3CH3 
E) More than one of these is an Arrhenius acid.

Question 8

What is the pH of a 0.500 M NH3 solution that has Kb = 1.8 × 10-5? The equation for the dissociation of NH3 is:
NH3(aq)+ H2O(l)⇌ NH4+(aq)+ OH-(aq)

Accepted Answer

A) 2.22 
B) 2.52 
C) 11.47 
D) 11.48 
A) 2.22 
B) 2.52 
C) 11.47 
D) 11.48

Question 9

What species are present in a 6 M aqueous solution of HCl (a strong acid)?

Accepted Answer

A) H+ and Cl-  
B) H+,Cl-,HCl 
C) H+,Cl-,HCl,H2O 
D) H+,Cl-,HCl,H2O,OH- 
A) H+ and Cl-  
B) H+,Cl-,HCl 
C) H+,Cl-,HCl,H2O 
D) H+,Cl-,HCl,H2O,OH-

Question 10

Identify the triprotic acid.

Accepted Answer

A) HNO3 
B) H3PO4 
C) H2SO3 
D) HClO4 
E) H2SO4 
A) HNO3 
B) H3PO4 
C) H2SO3 
D) HClO4 
E) H2SO4

Question 11

What is the Kw of pure water at 50.0°C,if the pH is 6.630?

Accepted Answer

A) 2.34 × 10-7 
B) 5.50 × 10-14 
C) 2.13 × 10-14 
D) 1.00 × 10-14 
E) There is not enough information to calculate the Kw. 
A) 2.34 × 10-7 
B) 5.50 × 10-14 
C) 2.13 × 10-14 
D) 1.00 × 10-14 
E) There is not enough information to calculate the Kw.

Question 12

The acid-dissociation constant of hydrocyanic acid (HCN)at 25.0°C is 4.9 × 10-10.What is the pH of an aqueous solution of 0.080 M sodium cyanide (NaCN)?

Accepted Answer

A) 11.11 
B) 2.89 
C) 1.3 × 10-3 
D) 7.8 × 10-12 
E) 3.9 × 10-11 
A) 11.11 
B) 2.89 
C) 1.3 × 10-3 
D) 7.8 × 10-12 
E) 3.9 × 10-11

Question 13

An aqueous solution at 25.0°C contains [H+] = 0.080 M.What is the pH of the solution?

Accepted Answer

A) 1.10 
B) -1.10 
C) 13.0 
D) 0.0800 
E) 1.30 × 10-13 
A) 1.10 
B) -1.10 
C) 13.0 
D) 0.0800 
E) 1.30 × 10-13

Question 14

Calculate the pH for an aqueous solution of pyridine that contains 2.15 × 10-4 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

Question 15

Determine the pH of a 0.741 M KOH solution at 25°C.

Accepted Answer

A) 0.13 
B) 13.87 
C) 0.17 
D) 12.65 
E) 11.88 
A) 0.13 
B) 13.87 
C) 0.17 
D) 12.65 
E) 11.88

Question 16

Calculate the hydroxide ion concentration in an aqueous solution with a pH of 4.33 at 25°C.

Accepted Answer

A) 2.1 × 10-10 M 
B) 9.7 × 10-10 M 
C) 4.7 × 10-5 M 
D) 3.8 × 10-5 M 
E) 6.3 × 10-6 M 
A) 2.1 × 10-10 M 
B) 9.7 × 10-10 M 
C) 4.7 × 10-5 M 
D) 3.8 × 10-5 M 
E) 6.3 × 10-6 M

Question 17

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

Accepted Answer

A) HOCH2CH2NH2,3.2 × 10-5 
B) NH3,1.76 × 10-5 
C) C5H5N,1.7 × 10-9 
D) (CH3CH2)3N,5.2 × 10-4 
E) Since these are all weak bases,they have the same strength. 
A) HOCH2CH2NH2,3.2 × 10-5 
B) NH3,1.76 × 10-5 
C) C5H5N,1.7 × 10-9 
D) (CH3CH2)3N,5.2 × 10-4 
E) Since these are all weak bases,they have the same strength.

Question 18

Which is the definition of Arrhenius acid?

Accepted Answer

A) a substance that produces H+ ions in aqueous solution 
B) a substance that produces OH- ions in aqueous solution 
C) a substance that is a proton donor 
D) a substance that is a proton acceptor 
A) a substance that produces H+ ions in aqueous solution 
B) a substance that produces OH- ions in aqueous solution 
C) a substance that is a proton donor 
D) a substance that is a proton acceptor

Question 19

Determine the pH of a 0.00598 M HClO4 solution.

Accepted Answer

A) 1.777 
B) 6.434 
C) 7.566 
D) 2.223 
E) 3.558 
A) 1.777 
B) 6.434 
C) 7.566 
D) 2.223 
E) 3.558

Question 20

What is the hydroxide ion concentration of a lye solution that has a pH of 9.20?

Accepted Answer

A) 6.31 × 10-10 M 
B) 1.58 × 10-5 M 
C) 4.80 M 
D) 9.20 M 
A) 6.31 × 10-10 M 
B) 1.58 × 10-5 M 
C) 4.80 M 
D) 9.20 M

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

Which of the following is not a conjugate acid-base pair?

Give the pH of 0.330 M phosphoric acid.For phosphoric acid,K_a1 = 7.5 × 10^-3,K_a2 = 6.2 × 10^-8,and K_a3 = 4.2 × 10^-13.

Determine the pOH of a 0.227 M C₅H₅N solution at 25°C.The K_b of C₅H₅N is 1.7 × 10^-9.

Match the following. -Br∅nsted-Lowry base

Determine the [H₃O^⁺] in a 0.265 M HClO solution.The K_a of HClO is 2.9 × 10^-8.

Which of the following is an Arrhenius acid?

What is the pH of a 0.500 M NH₃ solution that has K_b = 1.8 × 10^-5? The equation for the dissociation of NH₃ is: NH₃(aq)+ H₂O(l)⇌ NH₄⁺(aq)+ OH^-(aq)

What species are present in a 6 M aqueous solution of HCl (a strong acid)?

Identify the triprotic acid.

What is the K_w of pure water at 50.0°C,if the pH is 6.630?

The acid-dissociation constant of hydrocyanic acid (HCN)at 25.0°C is 4.9 × 10^-¹⁰.What is the pH of an aqueous solution of 0.080 M sodium cyanide (NaCN)?

An aqueous solution at 25.0°C contains [H⁺] = 0.080 M.What is the pH of the solution?

Calculate the pH for an aqueous solution of pyridine that contains 2.15 × 10^-⁴ hydroxide ion.

Determine the pH of a 0.741 M KOH solution at 25°C.

Calculate the hydroxide ion concentration in an aqueous solution with a pH of 4.33 at 25°C.

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

Which is the definition of Arrhenius acid?

Determine the pH of a 0.00598 M HClO₄ solution.

What is the hydroxide ion concentration of a lye solution that has a pH of 9.20?

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Chemical Quantities and Aqueous Reactions

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Chemical Bonding I: Lewis Theory

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Filters

Exam 15: Acids and Bases

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

Which of the following is not a conjugate acid-base pair?

Give the pH of 0.330 M phosphoric acid.For phosphoric acid,Ka1 = 7.5 × 10-3,Ka2 = 6.2 × 10-8,and Ka3 = 4.2 × 10-13.

Determine the pOH of a 0.227 M C5H5N solution at 25°C.The Kb of C5H5N is 1.7 × 10-9.

Match the following. -Br∅nsted-Lowry base

Determine the [H3O⁺] in a 0.265 M HClO solution.The Ka of HClO is 2.9 × 10-8.

Which of the following is an Arrhenius acid?

What is the pH of a 0.500 M NH3 solution that has Kb = 1.8 × 10-5? The equation for the dissociation of NH3 is: NH3(aq)+ H2O(l)⇌ NH4+(aq)+ OH-(aq)

What species are present in a 6 M aqueous solution of HCl (a strong acid)?

Identify the triprotic acid.

What is the Kw of pure water at 50.0°C,if the pH is 6.630?

The acid-dissociation constant of hydrocyanic acid (HCN)at 25.0°C is 4.9 × 10-10.What is the pH of an aqueous solution of 0.080 M sodium cyanide (NaCN)?

An aqueous solution at 25.0°C contains [H+] = 0.080 M.What is the pH of the solution?

Calculate the pH for an aqueous solution of pyridine that contains 2.15 × 10-4 hydroxide ion.

Determine the pH of a 0.741 M KOH solution at 25°C.

Calculate the hydroxide ion concentration in an aqueous solution with a pH of 4.33 at 25°C.

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

Which is the definition of Arrhenius acid?

Determine the pH of a 0.00598 M HClO4 solution.

What is the hydroxide ion concentration of a lye solution that has a pH of 9.20?

Matter, Measurement, and Problem Solving

Atoms and Elements

Molecules, Compounds and Chemical Equations

Chemical Quantities and Aqueous Reactions

Gases

Thermochemistry

The Quantum-Mechanical Model of the Atom

Periodic Properties of the Elements

Chemical Bonding I: Lewis Theory

Chemical Bonding II: Molecular Shapes, Valence Bond Theory, and

Liquids, Solids, and Intermolecular Forces

Solutions

Chemical Kinetics

Chemical Equilibrium

Aqueous Ionic Equilibrium

Free Energy and Thermodynamics

Electrochemistry

Radioactivity and Nuclear Chemistry

Filters

Give the pH of 0.330 M phosphoric acid.For phosphoric acid,K_a1 = 7.5 × 10^-3,K_a2 = 6.2 × 10^-8,and K_a3 = 4.2 × 10^-13.

Determine the pOH of a 0.227 M C₅H₅N solution at 25°C.The K_b of C₅H₅N is 1.7 × 10^-9.

Determine the [H₃O^⁺] in a 0.265 M HClO solution.The K_a of HClO is 2.9 × 10^-8.

What is the pH of a 0.500 M NH₃ solution that has K_b = 1.8 × 10^-5? The equation for the dissociation of NH₃ is: NH₃(aq)+ H₂O(l)⇌ NH₄⁺(aq)+ OH^-(aq)

What is the K_w of pure water at 50.0°C,if the pH is 6.630?

The acid-dissociation constant of hydrocyanic acid (HCN)at 25.0°C is 4.9 × 10^-¹⁰.What is the pH of an aqueous solution of 0.080 M sodium cyanide (NaCN)?

An aqueous solution at 25.0°C contains [H⁺] = 0.080 M.What is the pH of the solution?

Calculate the pH for an aqueous solution of pyridine that contains 2.15 × 10^-⁴ hydroxide ion.

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

Determine the pH of a 0.00598 M HClO₄ solution.