Chemical Forums
Chemistry Forums for Students => Inorganic Chemistry Forum => Topic started by: mol on February 01, 2011, 04:12:49 PM
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If a buffer with a pH of 10.00 is needed, which of the following can we use?
ethanoic acid with Ka= 1.8* 10^-5 or
ammonia with Kb = 1.8* 10^-5.
I know that pH and pOH must equal 14. so if 10 is to be added then we r left out with 4 .
The negative log of 1.8* 10^-5 is 4.7(still a closer value to 4). we need either a weak acid ( ethanoic acid) or a weak base (as ammonia) . So I am not sure how to choose one out of the above 2...
pls help.
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Do you know Henderson-Hasselbalch equation (http://www.chembuddy.com/?left=pH-calculation&right=pH-buffers-henderson-hasselbalch)?
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For buffers you need two reagents: NH3 and eg. NH4Cl, or CH3COOH and eg. CH3COONa
http://en.wikipedia.org/wiki/Buffer_solution
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Yes I know Henderson Hasselbach eqtn. But to use that eqtn I must have the concentrations of the base and acid in hand..Here I dont know the conc of them. Is it still possible I can use the eqtn to solve this.. can u pls show me how to do that?
Thanks
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Buffer works when the concentration of both acid and conjugate base are comparable. Best buffer is the one containing both in identical concentrations. Try to plug this information into HH equation.
eqtn eqtn conc eqtn u pls
Please read forum rules (http://www.chemicalforums.com/index.php?topic=33740.0).
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I'll try that. Thank you Borek and AWK.