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Buffer NH3 and NH4Cl

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I am really having problems with this problem:

Calculate the pH of the 0.20 M NH3 and 0.15 NH4Cl buffer. What is the pH of the buffer after the addition of 10.0 mL of 0.10 M HCl to 57.5 mL of the buffer.

The first part was fair enough, I got 9.35 pH, which is correct. The set up of the second part is tripping me up, I can't figure out how HCl would effect NH4 + OH->NH3. I calculated that the HCl wouldn't effect the pH, because it doesn't have significant OH-.

Please help, with step by step calculations.

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Solution Summary

The solutions uses the Henderson Hasselbalch equation to answer questions about acids and bases. Step by step calculations are provided in the solution.

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Problem: Calculate the pH of the 0.20 M NH3 and 0.15 NH4Cl buffer. What is the pH of the buffer after the addition of 10.0 mL of 0.10 M HCl to 57.5 mL of the buffer.

Solution:

Please refer to the attached file. Cheers.

NH4+ + H2O --> NH3 + H3O+

To find the pH of a buffer, you need to use the Henderson Hasselbalch equation:

(see attached file ...

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