CHM 109 Lecture Notes - Lecture 4: Sulfuric Acid, Equilibrium Constant, Ph
Document Summary
17 acids and bases or hydrogen ion/proton transfer rev f2012. 17. 1 arrhenius defined an acid as a substance that puts more h+ into solution than oh: he defined bases as substances that put more oh- into solution than h+ A neutral solution has equal amounts of h+ and oh- The acid for the forward reaction ha turns into its conjugate base a- by: amphoteric/ amphiprotic = substances that can be either acids or bases. 17. 4 conjugate acid-base pairs in reversible acid/base rx donating its h+ 17. 5 relative strengths of acids and bases acid base conjugates acid base. The base for the forward rx b turns into its conjugate acid by accepting the h+ Strong acids have weak bases and vice versa ex: hi h+1 + i -1 strong acid weak base. Strong acids want to dissociate into ions to make strongly electrolytic solutions.
