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The pH of a buffer solution containing a weak acid and its conjugate base depends only on the magnitude of Ka.
The pH of a buffer solution containing a weak acid and its conjugate base depends only on the magnitude of Ka.
False
The Henderson-Hasselbalch equation is used to calculate the pKa of buffer solutions.
The Henderson-Hasselbalch equation is used to calculate the pKa of buffer solutions.
False
A solution that is 0.200 M in NH3 and 0.300 M in NH4Cl will have a lower pH than a solution that is 0.400 M in formic acid and 1.00 M in sodium formate.
A solution that is 0.200 M in NH3 and 0.300 M in NH4Cl will have a lower pH than a solution that is 0.400 M in formic acid and 1.00 M in sodium formate.
True
Increasing the concentration of the weak acid in a buffer solution will always result in a lower pH.
Increasing the concentration of the weak acid in a buffer solution will always result in a lower pH.
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Both hydronium and hydroxide ion concentrations affect the pH of buffer solutions.
Both hydronium and hydroxide ion concentrations affect the pH of buffer solutions.
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Hydronium and hydroxide ion concentrations of pure water at 25°C are equal.
Hydronium and hydroxide ion concentrations of pure water at 25°C are equal.
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The pH and pOH of a 0.200 M aqueous NaOH solution are both less than 7.
The pH and pOH of a 0.200 M aqueous NaOH solution are both less than 7.
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Ba(OH)2 solution has a higher concentration of OH- ions compared to Ba+2 ions.
Ba(OH)2 solution has a higher concentration of OH- ions compared to Ba+2 ions.
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The pH of a 0.12 M aqueous HCl solution is greater than 7.
The pH of a 0.12 M aqueous HCl solution is greater than 7.
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Ammonium ion has a higher dissociation constant than ammonia.
Ammonium ion has a higher dissociation constant than ammonia.
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Buffer solutions are generally prepared from an acid / base pair.
Buffer solutions are generally prepared from an acid / base pair.
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