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Topic: Buffer solutions volume ratio  (Read 8463 times)

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Offline helpme89

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Buffer solutions volume ratio
« on: March 14, 2008, 11:37:26 PM »
so i have a question that is puzzling me so much i can not figure it out mabey you guys can guide me through it !
In what volume ratio should you mix 1.0 solutions of  NH4Cl and NH3 to produce a buffer solution having a pH = 9.70?

thank you
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Offline Borek

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Re: Buffer solutions volume ratio
« Reply #1 on: March 15, 2008, 05:00:15 AM »
Google Henderson-Hasselbalch equation.
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Offline helpme89

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Re: Buffer solutions volume ratio
« Reply #2 on: March 15, 2008, 07:29:01 PM »
I ahve tried googling and calling other chemistry students buh no luck .. if someone could help me that would be very much appreciated!
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Offline Borek

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Re: Buffer solutions volume ratio
« Reply #3 on: March 15, 2008, 07:32:33 PM »
Google and write Henderson-Hasselbalch equation.
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Offline Arkcon

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Re: Buffer solutions volume ratio
« Reply #4 on: March 15, 2008, 07:44:48 PM »
There is no way to solve this problem without using the Henderson-Hasselbalch equation.  I'm sure that very name is in the index of your text book, we need it to even start to figure out how to use the info you've been given.
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Offline helpme89

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Re: Buffer solutions volume ratio
« Reply #5 on: March 16, 2008, 10:34:35 PM »
sorry i misunderstood what you guys were trying to sya yes you need Henderson equation but i just do not know how to apply it to this question here it is :

 
pH = PKa + log (Base/ Acid)

much appreciation again!
 


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Offline enahs

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Re: Buffer solutions volume ratio
« Reply #6 on: March 16, 2008, 10:42:03 PM »
So. You know the pH you want. You know your acids and bases. Look up the pKa. Solve for the ratio in the log term. Walk away.

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Offline Arkcon

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Re: Buffer solutions volume ratio
« Reply #7 on: March 17, 2008, 06:54:24 AM »
Good, now, which of your reagents is the acid, and which is the base?
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