Question
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
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 sub 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.
A solution of hydrochloric acid at equilibrium will have a greater concentration of solute than a solution of acetic acid at equilibrium.
Responses
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 sub 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.
A solution of hydrochloric acid at equilibrium will have a greater concentration of solute than a solution of acetic acid at equilibrium.
Answers
GPT-4o mini
The correct statement is:
**The pH of a solution of hydrochloric acid must be less than the pH of a solution of acetic acid.**
Here's why:
1. **If the initial concentration of each acid is the same, then acetic acid will produce more H₃O⁺ ions than hydrochloric acid.** - This is incorrect because hydrochloric acid (HCl) is a strong acid that completely dissociates in water, producing more H₃O⁺ ions than acetic acid (CH₃COOH), which only partially dissociates.
2. **The dissociation constant for hydrochloric acid is greater than the dissociation constant for acetic acid.** - This statement is misleading. While it's true that HCl has a higher degree of dissociation (as a strong acid, it dissociates completely), it is not typically expressed in terms of a dissociation constant like Ka. Instead, it can be assumed that HCl does not have a Ka value in the same context since it fully dissociates, while acetic acid does have a Ka value.
3. **The pH of a solution of hydrochloric acid must be less than the pH of a solution of acetic acid.** - This statement is correct because hydrochloric acid, being a strong acid, will produce more H₃O⁺ ions and therefore have a lower pH compared to acetic acid at the same initial concentration.
4. **A solution of hydrochloric acid at equilibrium will have a greater concentration of solute than a solution of acetic acid at equilibrium.** - This statement can be misleading as well. Equal initial concentrations do not directly imply equilibrium concentrations since HCl dissociates completely while acetic acid does not.
Therefore, the most unequivocal correct response is the one regarding the pH of the solutions.
**The pH of a solution of hydrochloric acid must be less than the pH of a solution of acetic acid.**
Here's why:
1. **If the initial concentration of each acid is the same, then acetic acid will produce more H₃O⁺ ions than hydrochloric acid.** - This is incorrect because hydrochloric acid (HCl) is a strong acid that completely dissociates in water, producing more H₃O⁺ ions than acetic acid (CH₃COOH), which only partially dissociates.
2. **The dissociation constant for hydrochloric acid is greater than the dissociation constant for acetic acid.** - This statement is misleading. While it's true that HCl has a higher degree of dissociation (as a strong acid, it dissociates completely), it is not typically expressed in terms of a dissociation constant like Ka. Instead, it can be assumed that HCl does not have a Ka value in the same context since it fully dissociates, while acetic acid does have a Ka value.
3. **The pH of a solution of hydrochloric acid must be less than the pH of a solution of acetic acid.** - This statement is correct because hydrochloric acid, being a strong acid, will produce more H₃O⁺ ions and therefore have a lower pH compared to acetic acid at the same initial concentration.
4. **A solution of hydrochloric acid at equilibrium will have a greater concentration of solute than a solution of acetic acid at equilibrium.** - This statement can be misleading as well. Equal initial concentrations do not directly imply equilibrium concentrations since HCl dissociates completely while acetic acid does not.
Therefore, the most unequivocal correct response is the one regarding the pH of the solutions.