Chemical Forums
Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: duma on October 22, 2014, 02:06:37 AM
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What is the predominant form of ammonia in a solution at pH 7.0? Approximately
what fraction is in this form?
SOLUTION In Appendix B, we find pKa 9.24 for the ammonium ion (NH 4,
the conjugate acid of ammonia, NH3). At pH 9.24, [NH4 ] [NH3]. Below pH 9.24, NH4 will be the predominant form. Because pH 7.0 is about 2 pH units below pKa, the quotient [NH3]/[NH4 ] will be about 1:100. Approximately 99% is in the form NH4 .
so the book said that the pka is 9.24 for the ammonium ion NH4. Then it said ph = 9.24.
Are they saying pka = ph because they are assuming the ion is at 1/2 equivalence point? I'm confused. How did they get pka=ph? Is it a typo? We're not even talking about titrations in this example.
Also I don't understand how they got 1:100 due ph of 7 being 2 units lower then the ph of 9.24. How does that work?
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Are they saying pka = ph because they are assuming the ion is at 1/2 equivalence point? I'm confused. How did they get pka=ph? Is it a typo? We're not even talking about titrations in this example.
They didn't say pH is 9.24. They said "at pH 9.24 [NH3]=[NH4+]". That's not about pH 7.0 solution, but it is a good starting point to find the concentrations asked about.
Also I don't understand how they got 1:100 due ph of 7 being 2 units lower then the ph of 9.24. How does that work?
Please see http://www.titrations.info/acid-base-titration-indicators
While it is about indicators, equation (2) holds for any weak acid, and nicely shows how the ratio of the protonated/free form changes with pH (and why it changes tenfold with pH changing by one unit).