We’re being asked to calculate the pH of a buffer solution prepared that is 0.18 M NH3 and 0.27 M NH4Cl.
A solution that contains a weak acid and its conjugate base is a buffer solution. The pH of a buffer solution can be determined using the Henderson-Hasselbalch equation.
The solution is composed of 0.18 M NH3 and 0.27 M NH4Cl.
• NH4Cl breaks up into its ions in the solution:
A buffer solution is prepared that is 0.18 M NH3 and 0.27 M NH4Cl. What is the pH of this buffer? Kb for NH3 is 1.8 x 10 -5
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