PHC320H1 Lecture Notes - Lecture 3: Tris, Relative Permittivity, Conjugate Acid
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24 Mar 2015
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For tris buffer, the delta h of ionization is quite large: heating up the solution will change the ph, going from temp 0 -52 degrees c changes ph from 9. 0 to 7. 6. Pressure does play an important role as well, but this is beyond the scope of this course. The acid dissociates into conjugate base and hydronium ion. And, we have sodium in our solution. Let"s say there are two distinct, non-homoegenous regions: on the right hand, you have na+ and h2o, on the left hand, you have higher cocnetration of h+ due to presence of conjugate base. The na+ is stabilizing the conjugate base (a- ion). The stabilization causes the reaction of the acid to go forward from ha a- + h+ , allowing the acid to dissociate further. The na+ is a counterion that stabilizes the negative charge of the conjugate base. The equilibrium constant is going to become smaller and pka is going to change.
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