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