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Physical Chemistry
4 Mar 2008 20:34:59 IST
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4 Mar 2008 23:55:41 IST
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And before anyone disagrees,
I googled it and
"I got a note from Frank Brown gently reminding me that the
first step in the autodissociation of water does not restrict
the pH to be positive. As a result I have gone and done some reading.
My confusion arose from the fact that the autodissociation
of water can be a controlling factor in certain regimes...but
definitely not in the strong acid / strong base regime.
As it turns out, commercial concentrated HCl (37% by weight)
has a pH of approximately -1.1....and saturated NaOH
solution has a pH of about 15.0
So, the answer is, although pH TENDS to range between 1 and 14
for most household chemicals and substances encountered in natural
earth conditions, there is nothing which fundamentally restricts it
to this range even at 25C."
from the site:
http://www.newton.dep.anl.gov/askasci/chem99/chem99230.htm
I googled it and
"I got a note from Frank Brown gently reminding me that the
first step in the autodissociation of water does not restrict
the pH to be positive. As a result I have gone and done some reading.
My confusion arose from the fact that the autodissociation
of water can be a controlling factor in certain regimes...but
definitely not in the strong acid / strong base regime.
As it turns out, commercial concentrated HCl (37% by weight)
has a pH of approximately -1.1....and saturated NaOH
solution has a pH of about 15.0
So, the answer is, although pH TENDS to range between 1 and 14
for most household chemicals and substances encountered in natural
earth conditions, there is nothing which fundamentally restricts it
to this range even at 25C."
from the site:
http://www.newton.dep.anl.gov/askasci/chem99/chem99230.htm
pH 
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