11 Questions
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.
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.
True
Increasing the concentration of the weak acid in a buffer solution will always result in a lower pH.
False
Both hydronium and hydroxide ion concentrations affect the pH of buffer solutions.
True
Hydronium and hydroxide ion concentrations of pure water at 25°C are equal.
True
The pH and pOH of a 0.200 M aqueous NaOH solution are both less than 7.
False
Ba(OH)2 solution has a higher concentration of OH- ions compared to Ba+2 ions.
True
The pH of a 0.12 M aqueous HCl solution is greater than 7.
False
Ammonium ion has a higher dissociation constant than ammonia.
False
Buffer solutions are generally prepared from an acid / base pair.
True
Test your understanding of pH calculations with various examples involving the calculation of hydronium and hydroxide ion concentrations, pH, and pOH in different aqueous solutions. Practice calculating molar concentrations of ions in solutions like Ba(OH)2.
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