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Inorganic : %dissocation
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 Message 1 of 2 in Discussion 
From: dianna  (Original Message)Sent: 11/16/2004 5:46 AM
i was just wondering, if "the pH of a solution of a 0.5M weak acid HA is 2.5. To calculate the percent dissociation of this solution, could i first convert the pH 2.5 to a concentration of 0.00316M, and then go 0.00316M/0.5M times 100 to get the anwer 0.63%?
thanx for helping:)


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 Message 2 of 2 in Discussion 
From: MSN Nickname·Steve·Sent: 11/16/2004 6:39 AM
Hi Dianna, yes, that's right.  The H+ concentration will be equal to the concentration of the weak acid in dissociated form.  This number divided by the total concentration of the weak acid, undissociated plus dissociated, 0.5 M, times 100, is the percentage of the weak acid in dissociated form at equilibrium.

Steve