Question 1

Which of the following statements describes a neutral solution? A)[H₃O⁺] > [OH^-] B)[H₃O⁺] < [OH^-] C)[H₃O⁺] × [OH^-] ≠ 1 × 10^-14 D)[H₃O⁺]/[OH^-] = 1 × 10^-14 E)[H₃O⁺]/[OH^-] = 1

Accepted Answer

A neutral solution has an equal concentration of hydrogen ions (H+) and hydroxide ions (OH-), resulting in a pH of 7. Therefore, the ratio of H+ to OH- is 1:1, and the ratio of [H₃O⁺] to [OH^-] must also be 1:1, making option E the correct choice. Option A and B describe solutions with an imbalance of H+ and OH-, while options C and D describe expressions that are not consistent with a neutral solution.

Question 2

Arrange the following images of an aqueous base solution in order of increasing base strength: 
A)A,B,C
B)B,C,A
C)C,B,A
D)A,C,B
E)All are equally strong.

Accepted Answer

The answer of Arrange the following images of an aqueous...

Question 3

What would the concentration of OH^- be if the concentration of H₃O⁺ was 1 × 10^-8M? [H₃O⁺] × [OH^-] = K_w= 1 × 10^-14 A)1 × 10^-14 B)1 × 10^-6 C)1 × 10⁸ D)1 × 10⁶ E)1 × 10^-8

Accepted Answer

Given the ion product of water (Kw) is 1 × 10^-14 M^2, and the concentration of H3O+ is 1 × 10^-8 M, the concentration of OH- can be found by dividing Kw by the concentration of H3O+. Therefore, [OH-] = 1 × 10^-14 M^2 / 1 × 10^-8 M = 1 × 10^-6 M.

Question 4

Qualitatively,what happens to the hydronium ion concentration if you increase the hydroxide ion concentration? A)The concentration of H₃O⁺ stays the same but the ratio changes. B)The concentration of H₃O⁺ increases but the ratio stays the same. C)The concentration of H₃O⁺ increases to neutralize the excess hydroxide. D)none of the above

Accepted Answer

Increasing the hydroxide ion concentration in a solution will decrease the hydronium ion concentration to maintain the product of their concentrations at a constant value (1.0 x 10^-14 at 25°C), not increase it. None of the provided options accurately describe this relationship.

Question 5

What do the brackets in the following equation represent? [H₃O⁺] × [OH^-] = K_w A)The brackets mean the molarity of the compound inside them. B)The molecule inside does not react with the other molecules in brackets. C)The molecule in brackets is undergoing hydrogen bonding with the other molecule in brackets. D)The first molecule in brackets is an acid and it reacts with the second molecule in brackets,which is a base. E)none of the above

Accepted Answer

The brackets in chemical equations typically denote the concentration or molarity of the species inside them.

Question 6

Which of the following statements describes an acidic solution? A)[H₃O⁺] > [OH^-] B)[H₃O⁺] < [OH^-] C)[H₃O⁺] × [OH^-] ≠ 1 × 10^-14 D)[H₃O⁺]/[OH^-] = 1 × 10^-14 E)[H₃O⁺]/[OH^-] = 1

Accepted Answer

An acidic solution is characterized by having a higher concentration of hydrogen ions ([H+]) than hydroxide ions ([OH-]).

Question 7

-Which of the above illustrations shows an acidic aqueous solution?
A)A
B)B
C)C
D)All of the above are neutral solutions.
E)none of the above

Accepted Answer

The answer of 
-Which of the above illustrations shows an...

Question 8

-Which of the above illustrations shows a neutral aqueous solution?
A)A
B)B
C)C
D)All of the above are neutral solutions.
E)none of the above

Accepted Answer

The answer of 
-Which of the above illustrations shows a...

Question 9

What would the concentration of H₃O⁺ be if the concentration of OH^- was 1 × 10^-11M? [H₃O⁺] × [OH^-] = K_w= 1 × 10^-14 A)1 × 10^-3 B)1 × 10³ C)1 × 10¹⁴ D)1 × 10¹² E)1 × 10^-6

Accepted Answer

Given the ion product of water (Kw) is 1 × 10^-14, and the concentration of OH^- is 1 × 10^-11 M, the concentration of H3O+ can be found using the relation Kw = [H3O+][OH^-]. Substituting the given values, 1 × 10^-14 = [H3O+](1 × 10^-11), solving for [H3O+] gives 1 × 10^-3 M.

Question 10

If the pH of a solution is 10,what is the hydronium ion concentration? A)1 × 10^-10M B)1 × 10¹⁰M C)10 M D)-10 M E)- 1 × 10¹⁰M

Accepted Answer

The hydronium ion concentration in a solution with a pH of 10 is 1 × 10^-10 M. This is because pH is calculated as -log[H3O+], so if pH = 10, then [H3O+] = 10^-10 M.

Question 11

What would the concentration of OH^- be if the concentration of H₃O⁺ was 1 × 10^-⁵M? [H₃O⁺] × [OH^-] = K_w= 1 × 10^-14 A)1 × 10^-14 B)1 × 10^-5 C)1 × 10⁹ D)1 × 10⁵ E)1 × 10^-9

Accepted Answer

The concentration of OH⁻ can be found using the formula [H₃O⁺] × [OH⁻] = Kw. Given [H₃O⁺] = 1 × 10⁻⁵ M and Kw = 1 × 10⁻¹⁴, [OH⁻] = Kw / [H₃O⁺] = 1 × 10⁻¹⁴ / 1 × 10⁻⁵ = 1 × 10⁻⁹ M.

Question 12

-Which of the above illustrations shows a basic aqueous solution?
A)A
B)B
C)C
D)All of the above are neutral solutions.
E)none of the above

Accepted Answer

A basic aqueous solution has a pH greater than 7. In the illustration, only A has a pH greater than 7, which is 8.

Question 13

Sodium hydroxide,NaOH,is a strong base,which means that it readily accepts hydrogen ions.What products are formed when sodium hydroxide accepts a hydrogen ion from a water molecule?
A)water and sodium hydroxide
B)sodium hydroxide and hydronium ions
C)sodium ions and hydronium ions
D)sodium ions and water

Accepted Answer

The answer of Sodium hydroxide,NaOH,is a strong base,which means that...

Question 14

Which of the following statements describes a basic solution? A)[H₃O⁺] > [OH^-] B)[H₃O⁺] < [OH^-] C)[H₃O⁺] × [OH^-] ≠ 1 × 10^-14 D)[H₃O⁺]/[OH^-] = 1 × 10^-14 E)[H₃O⁺]/[OH^-] = 1

Accepted Answer

A basic solution is characterized by a higher concentration of hydroxide ions ([OH-]) than hydrogen ions ([H+]), which means [OH-] > [H+].

Question 15

Which of the following solutions is the most acidic?
A)a solution with a pH = 14
B)a solution with a pH = 10
C)a solution with a pH = 7
D)a solution with a pH = 4
E)All of the solutions are basic.

Accepted Answer

The lower the pH value, the more acidic the solution. Among the given options, the solution with pH = 4 is the most acidic.

Question 16

What would the concentration of H₃O⁺ be if the concentration of OH^- was 1 × 10^-1M? [H₃O⁺] × [OH^-] = K_w= 1 × 10^-1⁴ A)1 × 10^-3 B)1 × 10^-2 C)1 × 10^-4 D)1 × 10¹³ E)none of the above

Accepted Answer

The answer of What would the concentration of H₃O⁺ be...

Question 17

A weak acid is added to a concentrated solution of hydrochloric acid.Does the solution become more or less acidic?
A)More acidic,since there are more hydronium ions being added to the solution.
B)Less acidic,since the solution becomes more dilute with a less concentrated solution of hydronium ions being added to the solution.
C)No change in acidity,since the concentration of the hydrochloric acid is too high to be changed by the weak solution.
D)Less acidic since the concentration of hydroxide ions will increase.

Accepted Answer

Adding a weak acid to a concentrated solution of hydrochloric acid will lead to dilution of the solution. The concentration of hydronium ions will decrease, making the solution less acidic.

Question 18

As the hydronium ion concentration increases,the pH A)goes down. B)gets larger. C)starts to affect the OH^- concentration. D)starts to alter the chemical properties of the water molecules. E)stays constant.

Accepted Answer

The pH scale measures the concentration of hydrogen ions in a solution. As the hydronium ion concentration increases, the pH decreases. This means that the solution becomes more acidic. Therefore, the best choice is A, as the pH goes down.

Question 19

Qualitatively,what happens to the hydroxide ion concentration if you decrease the hydronium ion concentration? A)The concentration of OH^- stays the same but the ratio OH^-/H₃O⁺ changes. B)The concentration of OH^- increases but the ratio stays the same. C)The concentration of OH^- increases. D)none of the above

Accepted Answer

By decreasing the hydronium ion concentration, the equilibrium shifts to the left in the following reaction: H3O+ + OH- ↔ 2H2O. This means that more hydroxide ions (OH-) will form, causing an increase in their concentration. This increase is not balanced by a decrease in the concentration of hydroxide ions, as suggested in option A. Option B is incorrect because the concentration of hydroxide ions cannot increase while the ratio stays the same, as it would mean that the concentration of hydronium ions also increases. Therefore, option C is the best choice as it accurately describes the situation.

Question 20

Which of the following reactions illustrates an amphoteric compound? A)2 HF ⇌ H₂F⁺ + F^- B)NaOH + HBr ⇌ NaBr + H₂O C)2 H₂ + O₂ ⇌ 2 H₂O D)All are amphoteric. E)none of the above

Accepted Answer

The answer of Which of the following reactions illustrates an...

Quiz 18: Two Classes of Chemical Reactions

Which of the following statements describes a neutral solution?

Arrange the following images of an aqueous base solution in order of increasing base strength:

What would the concentration of OH- be if the concentration of H3O+ was 1 × 10-8M? [H3O+] × [OH-] = Kw = 1 × 10-14

Qualitatively,what happens to the hydronium ion concentration if you increase the hydroxide ion concentration?

What do the brackets in the following equation represent? [H3O+] × [OH-] = Kw

Which of the following statements describes an acidic solution?

-Which of the above illustrations shows an acidic aqueous solution?

-Which of the above illustrations shows a neutral aqueous solution?

What would the concentration of H3O+ be if the concentration of OH- was 1 × 10-11M? [H3O+] × [OH-] = Kw = 1 × 10-14

If the pH of a solution is 10,what is the hydronium ion concentration?

What would the concentration of OH- be if the concentration of H3O+ was 1 × 10-5M? [H3O+] × [OH-] = Kw = 1 × 10-14

-Which of the above illustrations shows a basic aqueous solution?

Sodium hydroxide,NaOH,is a strong base,which means that it readily accepts hydrogen ions.What products are formed when sodium hydroxide accepts a hydrogen ion from a water molecule?

Which of the following statements describes a basic solution?

Which of the following solutions is the most acidic?

What would the concentration of H3O+ be if the concentration of OH- was 1 × 10-1M? [H3O+] × [OH-] = Kw = 1 × 10-14

A weak acid is added to a concentrated solution of hydrochloric acid.Does the solution become more or less acidic?

As the hydronium ion concentration increases,the pH

Qualitatively,what happens to the hydroxide ion concentration if you decrease the hydronium ion concentration?

Which of the following reactions illustrates an amphoteric compound?

What would the concentration of OH^- be if the concentration of H₃O⁺ was 1 × 10^-8M? [H₃O⁺] × [OH^-] = K_w= 1 × 10^-14

What do the brackets in the following equation represent? [H₃O⁺] × [OH^-] = K_w

What would the concentration of H₃O⁺ be if the concentration of OH^- was 1 × 10^-11M? [H₃O⁺] × [OH^-] = K_w= 1 × 10^-14

What would the concentration of OH^- be if the concentration of H₃O⁺ was 1 × 10^-⁵M? [H₃O⁺] × [OH^-] = K_w= 1 × 10^-14

What would the concentration of H₃O⁺ be if the concentration of OH^- was 1 × 10^-1M? [H₃O⁺] × [OH^-] = K_w= 1 × 10^-1⁴