Question 1 A)Which acid-base chemical reaction is irreversible?(1 point) Responses weak base added to water weak base added to water strong acid added to water strong acid added to water weak acid added to water weak acid added to water water on its own water on its own Question 2 A)Hydrochloric acid is a strong acid. Acetic acid is a weak acid. Which statement about hydrochloric acid and acetic acid is correct?(1 point) Responses A solution of hydrochloric acid at equilibrium will have a greater concentration of solute than a solution of acetic acid at equilibrium. A solution of hydrochloric acid at equilibrium will have a greater concentration of solute than a solution of acetic acid at equilibrium. If the initial concentration of each acid is the same, then acetic acid will produce more H3O+ ions than hydrochloric acid. If the initial concentration of each acid is the same, then acetic acid will produce more H 3 O + ions than hydrochloric acid. The dissociation constant for hydrochloric acid is greater than the dissociation constant for acetic acid. The dissociation constant for hydrochloric acid is greater than the dissociation constant for acetic acid. The pH of a solution of hydrochloric acid must be less than the pH of a solution of acetic acid. The pH of a solution of hydrochloric acid must be less than the pH of a solution of acetic acid. Question 3 A) Use the information in the table to answer the question. Acid pH of Solution HA 5.6 HB 3.9 HC 4.7 Which list shows the acidic solutions in order from least conductive of electricity to most conductive? (1 point) Responses HC, HB, HA HC, HB, HA HA, HB, HC HA, HB, HC HB, HC, HA HB, HC, HA HA, HC, HB HA, HC, HB Question 4 A)Which change would decrease the pH of a base in a solution at equilibrium?(1 point) Responses decreasing the amount of water added to the solute decreasing the amount of water added to the solute decreasing the concentration of OH– ions decreasing the concentration of OH – ions increasing the initial concentration of solute increasing the initial concentration of solute increasing the strength of the base

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Question 1:
The irreversible acid-base chemical reaction among the options provided is:

Strong acid added to water

Question 2:
The correct statement about hydrochloric acid and acetic acid is:

The dissociation constant for hydrochloric acid is greater than the dissociation constant for acetic acid.

Question 3:
To determine the order of acidic solutions from least conductive to most conductive based on their pH values:

HA, HC, HB
(HA has the highest pH, thus is the weakest acid and least conductive, while HB has the lowest pH and is the strongest acid, thus most conductive.)

Question 4:
The change that would decrease the pH of a base in a solution at equilibrium is:

Decreasing the concentration of OH– ions

This is because decreasing the concentration of hydroxide ions (OH–) would shift the equilibrium towards producing more hydrogen ions (H3O+), thereby lowering the pH.

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Question 1 A)Which acid-base chemical reaction is irreversible?(1 point) Responses weak base added to water weak base added to water strong acid added to water strong acid added to water weak acid added to water weak acid added to water water on its own water on its own Question 2 A)Hydrochloric acid is a strong acid. Acetic acid is a weak acid. Which statement about hydrochloric acid and acetic acid is correct?(1 point) Responses A solution of hydrochloric acid at equilibrium will have a greater concentration of solute than a solution of acetic acid at equilibrium. A solution of hydrochloric acid at equilibrium will have a greater concentration of solute than a solution of acetic acid at equilibrium. If the initial concentration of each acid is the same, then acetic acid will produce more H3O+ ions than hydrochloric acid. If the initial concentration of each acid is the same, then acetic acid will produce more H 3 O + ions than hydrochloric acid. The dissociation constant for hydrochloric acid is greater than the dissociation constant for acetic acid. The dissociation constant for hydrochloric acid is greater than the dissociation constant for acetic acid. The pH of a solution of hydrochloric acid must be less than the pH of a solution of acetic acid. The pH of a solution of hydrochloric acid must be less than the pH of a solution of acetic acid. Question 3 A) Use the information in the table to answer the question. Acid pH of Solution HA 5.6 HB 3.9 HC 4.7 Which list shows the acidic solutions in order from least conductive of electricity to most conductive? (1 point) Responses HC, HB, HA HC, HB, HA HA, HB, HC HA, HB, HC HB, HC, HA HB, HC, HA HA, HC, HB HA, HC, HB Question 4 A)Which change would decrease the pH of a base in a solution at equilibrium?(1 point) Responses decreasing the amount of water added to the solute decreasing the amount of water added to the solute decreasing the concentration of OH– ions decreasing the concentration of OH – ions increasing the initial concentration of solute increasing the initial concentration of solute increasing the strength of the base

1 answer

Question 1:
The irreversible acid-base chemical reaction among the options provided is:

Strong acid added to water

Question 2:
The correct statement about hydrochloric acid and acetic acid is:

The dissociation constant for hydrochloric acid is greater than the dissociation constant for acetic acid.

Question 3:
To determine the order of acidic solutions from least conductive to most conductive based on their pH values:

HA, HC, HB
(HA has the highest pH, thus is the weakest acid and least conductive, while HB has the lowest pH and is the strongest acid, thus most conductive.)

Question 4:
The change that would decrease the pH of a base in a solution at equilibrium is:

Decreasing the concentration of OH– ions

This is because decreasing the concentration of hydroxide ions (OH–) would shift the equilibrium towards producing more hydrogen ions (H3O+), thereby lowering the pH.

Ask a New Question or answer this question.

GPT-4o mini · Answer

**Question 1:** The irreversible acid-base chemical reaction among the options provided is: - **Strong acid added to water** **Question 2:** The correct statement about hydrochloric acid and acetic acid is: - **The dissociation constant for hydrochloric acid is greater than the dissociation constant for acetic acid.** **Question 3:** To determine the order of acidic solutions from least conductive to most conductive based on their pH values: - **HA, HC, HB** (HA has the highest pH, thus is the weakest acid and least conductive, while HB has the lowest pH and is the strongest acid, thus most conductive.) **Question 4:** The change that would decrease the pH of a base in a solution at equilibrium is: - **Decreasing the concentration of OH– ions** This is because decreasing the concentration of hydroxide ions (OH–) would shift the equilibrium towards producing more hydrogen ions (H3O+), thereby lowering the pH.