04-04-2005, 10:07 PM #1
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04-04-2005, 10:32 PM #4
04-04-2005, 11:38 PM #5Originally Posted by u5711
04-04-2005, 11:43 PM #6
04-05-2005, 12:56 AM #7
04-05-2005, 02:20 AM #8
04-05-2005, 02:23 AM #9
04-05-2005, 02:30 AM #10
- Join Date: Aug 2002
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Why do you have to ask questions? (Why do I have to answer a question with a question?) (Am I still answering questions with questions?) (How can you call it an answer if it is a question?) (Am I saying this out loud?) (Should I PWN this person for even caring about the ph of some dip**** water with a bunch of variables in the equation, resulting in only one definitive answer of "PIITB?")
Holy **** cigarette.Quote of the year (2003):
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Let me translate that so you people will understand:
Oh snap, you be talkin all the shiznit bout 50 cent all up in the bodybuilding house *****s, ya'll best back up into the misc section befo I pull my gat on yo bitch asses. I be tearing 50 cent up any day yo, i'll bite that *****'s arm off wit my platinum teef bling bling." - Tom Swanson
04-05-2005, 02:44 AM #11
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04-05-2005, 03:11 AM #13
04-05-2005, 04:11 AM #14Originally Posted by Diab0lic
Atmospheric CO2 would disolve in the water in small amounts, and thus form carbonic acid, shifting the pH slightly lower than 7.
As for the boiling... The capacity of gasses to disolve in water is largely influenced by temperature, i.e. the higher the temp, the harder it is for gasses to disolve in water. Thats why when you drink a warm softdrink it is very bubbly and fizzy.
Hence, it is was boiling, we would not expect to see much CO2 disolving, and as a result the pH would shift closer to 7.Good Times
04-05-2005, 06:30 AM #15
pH of pure water is 7 at room temperature...25 degree celsius..
pH is dependent upon temperature...
pH = -Log[H+]
H20 <=> (H+) + (OH-)
the forward reaction is endothermic
increasing the temperature favours the forward reaction
[H+] and [OH-] increase...
both pH and pKw thus increase.
opposite happens upon decreasing the temperature.