Problem: 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 A. 8.09B. 9.42C. 4.56D. 9.08E. 4.92

FREE Expert Solution

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.

pH=pKa+log (conjugate baseweak acid)


Given solution:

The solution is composed of 0.18 M NH3 and 0.27 M NH4Cl.

 NH4Cl breaks up into its ions in the solution:

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Problem Details

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 

A. 8.09
B. 9.42
C. 4.56
D. 9.08
E. 4.92

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