A AWolfman Full Member 7+ Year Member Joined Aug 27, 2015 Messages 27 Reaction score 2 May 4, 2016 #1 Won't chlorinating the methyl group add electron withdrawing groups, therefore decreasing the amount which acetic acid ionizes? Members don't see this ad. Attachments upload_2016-5-4_19-59-17.png 293.3 KB · Views: 51 upload_2016-5-4_20-0-38.png 15.8 KB · Views: 51
Won't chlorinating the methyl group add electron withdrawing groups, therefore decreasing the amount which acetic acid ionizes? Members don't see this ad.
popopopop Full Member 10+ Year Member Joined Dec 18, 2011 Messages 1,690 Reaction score 1,373 May 4, 2016 #2 You're making it a better Lewis Acid in the process, and making the acidic hydrogen more ionizable. Upvote 0 Downvote
Wolfpack93 Full Member 7+ Year Member Joined Jul 25, 2014 Messages 883 Reaction score 632 May 4, 2016 #3 Think of this like common ion effect. HCl fully dissociates to H+ and Cl- so if you have extra H+, less of your weak acid would dissolve Upvote 0 Downvote
Think of this like common ion effect. HCl fully dissociates to H+ and Cl- so if you have extra H+, less of your weak acid would dissolve
Wolfpack93 Full Member 7+ Year Member Joined Jul 25, 2014 Messages 883 Reaction score 632 May 4, 2016 #4 electron withdrawing groups would stabilize the anion, so that would increase the ionization Upvote 0 Downvote
A AWolfman Full Member 7+ Year Member Joined Aug 27, 2015 Messages 27 Reaction score 2 May 4, 2016 #5 That makes a whole lot more sense. I keep making silly mistakes which seem to be the bane of my MCAT existence. Upvote 0 Downvote
That makes a whole lot more sense. I keep making silly mistakes which seem to be the bane of my MCAT existence.