vik91 New Member 10+ Year Member Sep 8, 2013 #1 Advertisement - Members don't see this ad I have no idea how to do this question. I feel comfortable with the henderson equation but just not sure how to use that with this question. AN ACID HA HAS PKA = 5.3. Calculate pH at which 25% of this acid will be in its basic form (A-)
Advertisement - Members don't see this ad I have no idea how to do this question. I feel comfortable with the henderson equation but just not sure how to use that with this question. AN ACID HA HAS PKA = 5.3. Calculate pH at which 25% of this acid will be in its basic form (A-)
starnova Full Member 10+ Year Member Sep 8, 2013 #2 pH = pKa + log A-/HA pH = 5.3 + log (.25/.75)= 4.82 use mols HH equation, but in this one it doesn't matter Upvote 0 Downvote
pH = pKa + log A-/HA pH = 5.3 + log (.25/.75)= 4.82 use mols HH equation, but in this one it doesn't matter
H HdK Full Member 10+ Year Member Sep 8, 2013 #3 beat me to it =( or log (1/3). Makes sense cuz becomes a little more acidic as 25% of the acid is being converted into ionic H+ Upvote 0 Downvote
beat me to it =( or log (1/3). Makes sense cuz becomes a little more acidic as 25% of the acid is being converted into ionic H+
