Chemical Forums
Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: curiousgeorge1234 on February 09, 2007, 02:00:36 PM
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I know how to calculate pH: -log [H+] for example.
But, if you are given the pH, ie. pH -1.00, how do you calculate the concentration?
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Law of logs. log(x) usually (and in this case) is log10(x)
if log(x) = y
x = 10y
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so, if the pH is -1.00
x= 10^ -1
is that correct?
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Careful, pH = -log[H] remember
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then, x = 10^1
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yes
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Last time I checked the pH scale was 0-14. -1 should be wrong unless you just made it up.
to calculate pH from a [H] or [OH-] you take the antilog.
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A negative number for a pH is perfect legit.
And you are right about the antilog. But what happens if you take the antilog of 1? You get 0. If you take the antilog of 2, you get a negative number. Are you saying it is impossible to have 2 Molar concentration of an acid?