Podcast
Questions and Answers
What is the term used to describe the self-ionization of water?
What is the term used to describe the self-ionization of water?
- Neutralization
- Dissociation
- Hydration
- Autoionization (correct)
In the autoionization of water, what ions are formed in a 1:1 molar ratio?
In the autoionization of water, what ions are formed in a 1:1 molar ratio?
- Sodium and chloride ions
- Proton and electron
- Carbonate and bicarbonate ions
- Hydronium and hydroxide ions (correct)
What happens to the concentrations of hydronium and hydroxide ions in pure water?
What happens to the concentrations of hydronium and hydroxide ions in pure water?
- Hydronium concentration is higher
- Hydroxide concentration is higher
- They are not present
- They are equal (correct)
How is a molecule acting as an acid defined in relation to proton donation?
How is a molecule acting as an acid defined in relation to proton donation?
What is the molar ratio of hydronium and hydroxide ions when water undergoes autoionization?
What is the molar ratio of hydronium and hydroxide ions when water undergoes autoionization?
What does the autoionization constant help determine in aqueous solutions?
What does the autoionization constant help determine in aqueous solutions?
In what form do hydronium and hydroxide ions exist in pure water compared to non-ionized water?
In what form do hydronium and hydroxide ions exist in pure water compared to non-ionized water?
What is the common name used to refer to the dissociation constant, as mentioned in the text?
What is the common name used to refer to the dissociation constant, as mentioned in the text?
At 25 degrees C, the concentration of hydronium ions in pure water is approximately:
At 25 degrees C, the concentration of hydronium ions in pure water is approximately:
What is the negative logarithm of the Kw constant?
What is the negative logarithm of the Kw constant?
In the pH scale, what does a high pH value indicate?
In the pH scale, what does a high pH value indicate?
When a solution becomes more acidic, what happens to the concentration of hydronium ions?
When a solution becomes more acidic, what happens to the concentration of hydronium ions?
Which principle describes the shift in equilibrium when an acid is added to pure water?
Which principle describes the shift in equilibrium when an acid is added to pure water?
What happens to the product of hydronium and hydroxide ions concentrations in acidic solutions compared to pure water?
What happens to the product of hydronium and hydroxide ions concentrations in acidic solutions compared to pure water?
"p" represents the negative logarithm of:
"p" represents the negative logarithm of:
