Question
Which acid-base chemical reaction is irreversible?
Strong acid added to water
Hydrochloric acid is a strong acid. Acetic acid is a weak acid. Which statement about hydrochloric acid and acetic acid is correct?
The dissociation constant for hydrochloric acid is greater than the dissociation constant for acetic acid.
Which list shows the acidic solutions in order from least conductive of electricity to most conductive?
HA, HC, HB
Which change would decrease the pH of a base in a solution at equilibrium?
decreasing the concentration of OH– ions
Strong acid added to water
Hydrochloric acid is a strong acid. Acetic acid is a weak acid. Which statement about hydrochloric acid and acetic acid is correct?
The dissociation constant for hydrochloric acid is greater than the dissociation constant for acetic acid.
Which list shows the acidic solutions in order from least conductive of electricity to most conductive?
HA, HC, HB
Which change would decrease the pH of a base in a solution at equilibrium?
decreasing the concentration of OH– ions
Answers
Answered by
GPT-4o mini
Let's address each part of your query:
1. **Irreversible Acid-Base Reaction**: The reaction of a strong acid with water is considered essentially irreversible. When a strong acid, like hydrochloric acid (HCl), dissociates in water, it completely ionizes, resulting in a significant increase in the concentration of hydrogen ions (H⁺). This reaction effectively goes to completion.
2. **Dissociation Constants**: Your statement is correct. Hydrochloric acid (HCl) is a strong acid and dissociates completely in solution, meaning its dissociation constant (K_a) is very large, effectively approaching infinity. Acetic acid (CH₃COOH), being a weak acid, has a much smaller dissociation constant, indicating that it does not dissociate completely. Thus, \( K_a \) for HCl is indeed greater than \( K_a \) for acetic acid.
3. **Conductivity Order of Acidic Solutions**: Conductivity in solutions is primarily determined by the concentration of ions present. Strong acids (like HCl) dissociate completely, producing a higher concentration of ions compared to weak acids (like acetic acid). Therefore, in the list provided:
- **HA** (presumably a weak acid, like acetic acid)
- **HB** (possibly another weak acid or even a strong acid, depending on its nature)
- **HC** (likely a strong acid)
The order from least to most conductive would likely be: HA < HB < HC, assuming HA is a weak acid, HB is another weak or a lesser strong acid, and HC is a strong acid.
4. **Effect on pH**: Decreasing the concentration of OH⁻ ions in a solution will lead to an increase in the concentration of H⁺ ions, as the system shifts to maintain equilibrium. According to the relationship pH = -log[H⁺], if [H⁺] increases, the pH will decrease. Therefore, decreasing the concentration of OH⁻ ions in a basic solution would indeed lead to a decrease in pH.
If you have any more questions or need further clarification, feel free to ask!
1. **Irreversible Acid-Base Reaction**: The reaction of a strong acid with water is considered essentially irreversible. When a strong acid, like hydrochloric acid (HCl), dissociates in water, it completely ionizes, resulting in a significant increase in the concentration of hydrogen ions (H⁺). This reaction effectively goes to completion.
2. **Dissociation Constants**: Your statement is correct. Hydrochloric acid (HCl) is a strong acid and dissociates completely in solution, meaning its dissociation constant (K_a) is very large, effectively approaching infinity. Acetic acid (CH₃COOH), being a weak acid, has a much smaller dissociation constant, indicating that it does not dissociate completely. Thus, \( K_a \) for HCl is indeed greater than \( K_a \) for acetic acid.
3. **Conductivity Order of Acidic Solutions**: Conductivity in solutions is primarily determined by the concentration of ions present. Strong acids (like HCl) dissociate completely, producing a higher concentration of ions compared to weak acids (like acetic acid). Therefore, in the list provided:
- **HA** (presumably a weak acid, like acetic acid)
- **HB** (possibly another weak acid or even a strong acid, depending on its nature)
- **HC** (likely a strong acid)
The order from least to most conductive would likely be: HA < HB < HC, assuming HA is a weak acid, HB is another weak or a lesser strong acid, and HC is a strong acid.
4. **Effect on pH**: Decreasing the concentration of OH⁻ ions in a solution will lead to an increase in the concentration of H⁺ ions, as the system shifts to maintain equilibrium. According to the relationship pH = -log[H⁺], if [H⁺] increases, the pH will decrease. Therefore, decreasing the concentration of OH⁻ ions in a basic solution would indeed lead to a decrease in pH.
If you have any more questions or need further clarification, feel free to ask!
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