Question 1

Calculate the [OH-] in an aqueous solution when the [H3O+] is 1.2 x 10-2M.

Accepted Answer

A)  3.8 x 10-10 M 
B)  8.3 x 10-11 M 
C)  2.0 x 10-10 M 
D)  1.0 x 10-14 M 
A)  3.8 x 10-10 M 
B)  8.3 x 10-11 M 
C)  2.0 x 10-10 M 
D)  1.0 x 10-14 M

Question 2

The ethylammonium ion, CH3CH2NH3+ has a pKa of 10.81. It reacts with water to form ethylamine, CH3CH2NH2 and H3O+ as shown below.
  Which of the following statements is true at pH 7?

Accepted Answer

A)  ethylammonium ion predominates 
B)  ethylamine predominates 
C)  the concentration of ethylamine equals that of ethylammonium ion 
D)  the pH is higher than pKa of the ethylammonium ion 
A)  ethylammonium ion predominates 
B)  ethylamine predominates 
C)  the concentration of ethylamine equals that of ethylammonium ion 
D)  the pH is higher than pKa of the ethylammonium ion

Question 3

Hydrogen sulfide ion, HS-, can react differently depending on the acidity of the solution in which it is present.
  These two solutions show that the

Accepted Answer

A)  hydrogen sulfide ion is an acid. 
B)  hydrogen sulfide ion is a base. 
C)  hydrogen sulfide ion is amphoteric. 
D)  hydrogen sulfide ion can only react with water. 
A)  hydrogen sulfide ion is an acid. 
B)  hydrogen sulfide ion is a base. 
C)  hydrogen sulfide ion is amphoteric. 
D)  hydrogen sulfide ion can only react with water.

Question 4

When we talk about pH we are referring to the concentration of hydronium ions present. If the concentration of hydronium in a solution is 1.0 x 10-8 M, what is the hydroxide ion concentration?

Accepted Answer

A)  1.0 x 10-6 M 
B)  9.0 x 10-8 M 
C)  1.0 x 10-14 M 
D)  The concentration cannot be predicted. 
A)  1.0 x 10-6 M 
B)  9.0 x 10-8 M 
C)  1.0 x 10-14 M 
D)  The concentration cannot be predicted.

Question 5

What is the [OH-] of a solution whose pH is 3.00?

Accepted Answer

A)  1.0 x 10-3 M 
B)  1.0 x 10-14 M 
C)  1.0 x 10-11 M 
D)  1.0 x 10-12 M 
A)  1.0 x 10-3 M 
B)  1.0 x 10-14 M 
C)  1.0 x 10-11 M 
D)  1.0 x 10-12 M

Question 6

In the reaction below:
  Increasing the concentration of Cl2 will ___ at equilibrium.

Accepted Answer

A)  increase the concentration of PCl5 
B)  increase the concentration of PCl3 
C)  decrease the concentration of PCl5 
D)  have no effect 
A)  increase the concentration of PCl5 
B)  increase the concentration of PCl3 
C)  decrease the concentration of PCl5 
D)  have no effect

Question 7

A base is a compound that produces an ion with the formula ___ in aqueous solution and an acid is a compound that produces the ___ ion in aqueous solution, which is also written as the hydronium ion (___).

Accepted Answer

The answer of A base is a compound that produces...

Question 8

Basic substances tend to have a ___ taste.

Accepted Answer

The answer of Basic substances tend to have a ___...

Question 9

The conjugate acid of the hydrogen sulfate ion (HSO4-) is ___.

Accepted Answer

Question 10

The greater the hydronium ion concentration, the higher the pH.

Accepted Answer

A) True 
 B)False

Question 11

Which of the following are the strong acids? List all.
HF, HNO3, HCN, CH3COOH, H2SO4

Accepted Answer

Question 12

A solution in which the concentration of H+ is greater than the concentration of OH- will

Accepted Answer

A)  have a pH greater than 7.0 and be basic. 
B)  have a pH less than 7.0 and be basic. 
C)  have a pH greater than 7.0 and be acidic. 
D)  have a pH less than 7.0 and be acidic. 
A)  have a pH greater than 7.0 and be basic. 
B)  have a pH less than 7.0 and be basic. 
C)  have a pH greater than 7.0 and be acidic. 
D)  have a pH less than 7.0 and be acidic.

Question 13

The equation:
  has the following equilibrium constant expression.

Accepted Answer

A)    
B)    
C)    
D)    
A)    
B)    
C)    
D)

Question 14

Calculate the pH of a 0.01 M NaOH solution. Assume complete dissociation.

Accepted Answer

The answer of Calculate the pH of a 0.01 M...

Question 15

The Ka for the reaction of acetic acid and water shown below is 1.8 x 10-5.
  Which of the following statements is true at pH 7?

Accepted Answer

A)  there is much more acetic acid than acetate ion 
B)  there is more acetate ion than acetic acid 
C)  the concentration of acetate ion is equal to that of acetic acid 
D)  the pH is lower than pKa of acetic acid 
A)  there is much more acetic acid than acetate ion 
B)  there is more acetate ion than acetic acid 
C)  the concentration of acetate ion is equal to that of acetic acid 
D)  the pH is lower than pKa of acetic acid

Question 16

Excessive use of antacids can lead to

Accepted Answer

A)  an increase in blood pH known as acidosis. 
B)  an increase in blood pH known as alkalosis. 
C)  a decrease in blood pH know as acidosis. 
D)  a decrease in blood pH known as alkylosis. 
A)  an increase in blood pH known as acidosis. 
B)  an increase in blood pH known as alkalosis. 
C)  a decrease in blood pH know as acidosis. 
D)  a decrease in blood pH known as alkylosis.

Question 17

One serious effect of cholera is to destroy the hydrogen carbonate ion in the buffer system in the blood. Would the body then suffer from acidosis or alkalosis? Explain.

Accepted Answer

Loss of the hydrogen

Question 18

What is the pH of a solution in which [H3O]+ is 2.2 x 10-12 M?

Accepted Answer

A)  2.34 
B)  4.54 x 10-3 
C)  11.66 
D)  8.42 
A)  2.34 
B)  4.54 x 10-3 
C)  11.66 
D)  8.42

Question 19

What is the molar concentration of hydronium ions in a sample of a soft drink that has a pH of 4?

Accepted Answer

A)  1/4 M 
B)  4 M 
C)  1 x 104 M 
D)  1 x 10-4 M 
A)  1/4 M 
B)  4 M 
C)  1 x 104 M 
D)  1 x 10-4 M

Question 20

A is red, B is colorless, and C is yellow. Initially the system is in equilibrium and has an orange color.
   What color will the system become if concentration of A is increased?

Accepted Answer

The answer of A is red, B is colorless, and...

Calculate the [OH^-] in an aqueous solution when the [H₃O⁺] is 1.2 x 10^-2M.

The ethylammonium ion, CH₃CH₂NH₃⁺ has a pK_a of 10.81. It reacts with water to form ethylamine, CH₃CH₂NH₂ and H₃O⁺ as shown below. Which of the following statements is true at pH 7?

Hydrogen sulfide ion, HS^-, can react differently depending on the acidity of the solution in which it is present. These two solutions show that the

When we talk about pH we are referring to the concentration of hydronium ions present. If the concentration of hydronium in a solution is 1.0 x 10^-8 M, what is the hydroxide ion concentration?

What is the [OH^-] of a solution whose pH is 3.00?

In the reaction below: Increasing the concentration of Cl₂ will ___ at equilibrium.

A base is a compound that produces an ion with the formula _ in aqueous solution and an acid is a compound that produces the _ ion in aqueous solution, which is also written as the hydronium ion (___).

Basic substances tend to have a ___ taste.

The conjugate acid of the hydrogen sulfate ion (HSO₄^-) is ___.

The greater the hydronium ion concentration, the higher the pH.

Which of the following are the strong acids? List all. HF, HNO₃, HCN, CH₃COOH, H₂SO₄

A solution in which the concentration of H⁺is greater than the concentration of OH^-will

The equation: has the following equilibrium constant expression.

Calculate the pH of a 0.01 M NaOH solution. Assume complete dissociation.

The K_a for the reaction of acetic acid and water shown below is 1.8 x 10^-5. Which of the following statements is true at pH 7?

Excessive use of antacids can lead to

One serious effect of cholera is to destroy the hydrogen carbonate ion in the buffer system in the blood. Would the body then suffer from acidosis or alkalosis? Explain.

What is the pH of a solution in which [H₃O]⁺ is 2.2 x 10^-12 M?

What is the molar concentration of hydronium ions in a sample of a soft drink that has a pH of 4?

A is red, B is colorless, and C is yellow. Initially the system is in equilibrium and has an orange color. What color will the system become if concentration of A is increased?

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Exam 7: Acids, Bases, and Equilibrium

Calculate the [OH-] in an aqueous solution when the [H3O+] is 1.2 x 10-2M.

The ethylammonium ion, CH3CH2NH3+ has a pKa of 10.81. It reacts with water to form ethylamine, CH3CH2NH2 and H3O+ as shown below. Which of the following statements is true at pH 7?

Hydrogen sulfide ion, HS-, can react differently depending on the acidity of the solution in which it is present. These two solutions show that the

When we talk about pH we are referring to the concentration of hydronium ions present. If the concentration of hydronium in a solution is 1.0 x 10-8 M, what is the hydroxide ion concentration?

What is the [OH-] of a solution whose pH is 3.00?

In the reaction below: Increasing the concentration of Cl2 will ___ at equilibrium.

A base is a compound that produces an ion with the formula ___ in aqueous solution and an acid is a compound that produces the ___ ion in aqueous solution, which is also written as the hydronium ion (___).

Basic substances tend to have a ___ taste.

The conjugate acid of the hydrogen sulfate ion (HSO4-) is ___.

The greater the hydronium ion concentration, the higher the pH.

Which of the following are the strong acids? List all. HF, HNO3, HCN, CH3COOH, H2SO4

A solution in which the concentration of H+ is greater than the concentration of OH- will

The equation: has the following equilibrium constant expression.

Calculate the pH of a 0.01 M NaOH solution. Assume complete dissociation.

The Ka for the reaction of acetic acid and water shown below is 1.8 x 10-5. Which of the following statements is true at pH 7?

Excessive use of antacids can lead to

One serious effect of cholera is to destroy the hydrogen carbonate ion in the buffer system in the blood. Would the body then suffer from acidosis or alkalosis? Explain.

What is the pH of a solution in which [H3O]+ is 2.2 x 10-12 M?

What is the molar concentration of hydronium ions in a sample of a soft drink that has a pH of 4?

A is red, B is colorless, and C is yellow. Initially the system is in equilibrium and has an orange color. What color will the system become if concentration of A is increased?

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An Introduction to Organic Compounds

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Organic Reactions Hydrocarbons, Carboxlic Acids, Amines, and Related Compounds

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Carbohydrates

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Nucleic Acids

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Calculate the [OH^-] in an aqueous solution when the [H₃O⁺] is 1.2 x 10^-2M.

The ethylammonium ion, CH₃CH₂NH₃⁺ has a pK_a of 10.81. It reacts with water to form ethylamine, CH₃CH₂NH₂ and H₃O⁺ as shown below. Which of the following statements is true at pH 7?

Hydrogen sulfide ion, HS^-, can react differently depending on the acidity of the solution in which it is present. These two solutions show that the

When we talk about pH we are referring to the concentration of hydronium ions present. If the concentration of hydronium in a solution is 1.0 x 10^-8 M, what is the hydroxide ion concentration?

What is the [OH^-] of a solution whose pH is 3.00?

In the reaction below: Increasing the concentration of Cl₂ will ___ at equilibrium.

A base is a compound that produces an ion with the formula _ in aqueous solution and an acid is a compound that produces the _ ion in aqueous solution, which is also written as the hydronium ion (___).

The conjugate acid of the hydrogen sulfate ion (HSO₄^-) is ___.

Which of the following are the strong acids? List all. HF, HNO₃, HCN, CH₃COOH, H₂SO₄

A solution in which the concentration of H⁺is greater than the concentration of OH^-will

The K_a for the reaction of acetic acid and water shown below is 1.8 x 10^-5. Which of the following statements is true at pH 7?

What is the pH of a solution in which [H₃O]⁺ is 2.2 x 10^-12 M?