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Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: a7m3l5a on October 06, 2008, 07:41:06 PM

Title: Ka of this acid
Post by: a7m3l5a on October 06, 2008, 07:41:06 PM

26.20 ml of 0.102M Naoh is needed to neutralize 25.00 ml of an unknown acid HA. The pH at the equivalence point was measured to be 8.77. What is the Ka of this acid?

Title: Re: Ka of this acid
Post by: AWK on October 07, 2008, 01:05:53 AM

Calculate stoichiometry of neutralization and use Henderson-Haselbach equation.

Title: Re: Ka of this acid
Post by: Borek on October 07, 2008, 02:53:12 AM

Quote from: AWK on October 07, 2008, 01:05:53 AM

Calculate stoichiometry of neutralization and use Henderson-Haselbach equation.

You don't use Henderson-Hasselbalch equation to calculate pH at the equivalence point.

Idential question was asked here:

http://www.chemicalforums.com/index.php?topic=28764