Chemical Forums
Chemistry Forums for Students => High School Chemistry Forum => Topic started by: SemonSays on May 08, 2007, 06:48:17 PM
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I can't figure out why urea is basic and not acidic. I can't find any information on the internet and i have to use the molecular structure or Lewis structure of urea to prove it. I also need to find out how urea is chemically changed to nitrate ions.
Can anyone help me out?
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If you draw resonance structures for urea, that would be a good start.
Think about conjugate acids and bases.
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there are 4 i think. http://academic.evergreen.edu/curricular/MANDM2000/Spring/homework/hw6/Image950.gif
That is the Lewis structure of urea (hope the link works). But how does that help? Im so confused. :(
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I thought it had something to do with the amino groups or amidogens (NH2), but im not so sure.
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The lone pairs of electrons in the molecule are available despite resonance because in all of the resonance structures, at least one of the nitrogen atoms has a lone pair on it.
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Don't forget what Brønsted-Lowry said about a base, the whole part about a base being simply a proton acceptor.
The nitrogen has that nice lone pair. Looks like a good place to accept a proton to me.
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Hi guys - sorry for being dumb, but, why is it then that urea dissolved in water is quite acidic - pH being about 1 when I put it in water at about 20%.
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Hi guys - sorry for being dumb, but, why is it then that urea dissolved in water is quite acidic - pH being about 1 when I put it in water at about 20%.
This is a good point, the pKa for urea is low, why have you assumed that it is basic Semonsays?
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Yea - my first assumption (which was wrong) was that the solution would be basic - I guess it was the 2 NH2's that threw me - it just 'looks' as though it should be basic to me. It is, however, quite acidic in solution - I might be missing something simple here, but, at the moment I'm not sure why it is acidic.
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Yea - my first assumption (which was wrong) was that the solution would be basic - I guess it was the 2 NH2's that threw me - it just 'looks' as though it should be basic to me. It is, however, quite acidic in solution - I might be missing something simple here, but, at the moment I'm not sure why it is acidic.
If you push the electrons from the nitrogen into the C-N bond and make it C=N, then you have a positive charge on the NH2 group, loss of hydrogen would fix this?
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Hmmm, so it is acidic. The NH2's also threw me.
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Google Search: *urea basic*...second result: http://answers.yahoo.com/question/index?qid=20070508144240AAqawz0
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Google Search: *urea basic*...second result: http://answers.yahoo.com/question/index?qid=20070508144240AAqawz0
Strange, because the pKa of urea is ~0.2.
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I'm really sorry gents - feel free to eat my snacks :-[
It was the urea phosphate I was using that gave the very low pH's (0.2 in water). The urea in water was around 7.5. Apologies.
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I'm really sorry gents - feel free to eat my snacks :-[
It was the urea phosphate I was using that gave the very low pH's (0.2 in water). The urea in water was around 7.5. Apologies.
That clears up some confusion i guess.