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Topic: preparing a buffer  (Read 4148 times)

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mikey14

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preparing a buffer
« on: November 13, 2005, 03:17:34 AM »
Question:
How much .0036 M HCl should be added to .1 L of a .042 M ammonia solution to make a pH 8.8 buffer? State all assumptions.

I thought about using the Henderson-Hasselbach equation, but I don't think that would work. I also started with the equation: NH3 + H20 < = > NH4+  + OH-, knowing that NH4 is NH3's conjugate acid.

Any help is much appreciated!
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Offline Borek

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Re:preparing a buffer
« Reply #1 on: November 13, 2005, 04:15:25 AM »
You are on the right track, continue!
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mikey14

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Re:preparing a buffer
« Reply #2 on: November 13, 2005, 12:31:58 PM »
I'm just not sure how the strong acid would affect it. I could use pOH=pKb+log(conj. acid/base), to get a ratio of the conj. acid /base. Then I'm stuck.
Thanks
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Offline AWK

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Re:preparing a buffer
« Reply #3 on: November 14, 2005, 01:50:56 AM »
Strong acid reacts with base to form a salt. An axcessing ammonia and salt form a buffer soluta ion
« Last Edit: November 14, 2005, 01:51:41 AM by AWK »
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