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Sep28-03, 05:24 PM
P: 324
Originally posted by FZ+
I am not really sure about this, but when we gauge the strength of acids, we refer to it's acidity at standard conditions of 25C, or so. Thus, it may well be that at that temperature, H2SO4 is better as a proton donor than HCl.

H2SO4(aq) <-> 2H(aq) (+) + SO4(aq) (-)

What is significant is the position of this equilibrium at various temps. At higher temps, the equilibrium should increase the pH value of the acidic solution.
Careful, are you saying the equilibrium would go to the left? Because if it goes to the right the pH would go down. pH = -log[H+]