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Questions and Answers
The pH of a buffer solution depends only on the concentration of the weak acid present.
The pH of a buffer solution depends only on the concentration of the weak acid present.
False (B)
The Henderson-Hasselbalch equation is used to calculate the concentration of hydronium ions in a solution.
The Henderson-Hasselbalch equation is used to calculate the concentration of hydronium ions in a solution.
False (B)
A buffer solution containing a weak acid and its conjugate base can never be neutral.
A buffer solution containing a weak acid and its conjugate base can never be neutral.
False (B)
The pH of a buffer solution may change significantly when a small amount of acid or base is added to it.
The pH of a buffer solution may change significantly when a small amount of acid or base is added to it.
The relative concentrations of hydronium and hydroxide ions in a buffer solution depend only on the magnitudes of Ka and Kb.
The relative concentrations of hydronium and hydroxide ions in a buffer solution depend only on the magnitudes of Ka and Kb.
The hydronium and hydroxide ion concentrations of pure water at 25°C and 100°C are equal.
The hydronium and hydroxide ion concentrations of pure water at 25°C and 100°C are equal.
The molar concentration for Ba+2 and OH- ions in 0.03 M of Ba(OH)2 solution is the same.
The molar concentration for Ba+2 and OH- ions in 0.03 M of Ba(OH)2 solution is the same.
When a weak acid or weak base is dissolved in water, complete dissociation always occurs.
When a weak acid or weak base is dissolved in water, complete dissociation always occurs.
Conjugate acid-base pairs have equal dissociation constants.
Conjugate acid-base pairs have equal dissociation constants.
Buffer solutions are prepared from non-related acid-base pairs.
Buffer solutions are prepared from non-related acid-base pairs.
Buffer solutions resist changes in pH when diluted or when acids or bases are added to them.
Buffer solutions resist changes in pH when diluted or when acids or bases are added to them.
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