CHEM 1C Lecture Notes - Lecture 11: Nitric Acid, Equilibrium Constant, Barium Hydroxide
Document Summary
Poh and ph are related to each other through the water ion-product constant. [h+][oh-] = kw = 1. 0 x 10 -14. Log [h+] log [oh-] = 14. 00. Example) the ph of lemon juice is 3. 5. Hat is the h+ ion concentration in the juice? ph = -log [h+] [h+] = 10 -ph = 10 -3. 5 = 3. 2 x 10 -4 m. Hno3(aq) + h2o (l) (cid:314) h3o+(aq) + no3-(aq) 0. 005 m 0. 005 m ph = -log [h+] = -log [h3o+] = -log(0. 005) = 2. 3. 0. 014 m ph = 14. 00 poh = 14. 00 + log(0. 028) = 12. 4. Pka is not exactly the same as ph; numerically different. Ph: measure of the concentration of [h+] only. Monoprotic acids: ha h+ + a- Even weak acids become fully ionized at low enough concentrations. If ka is very small, assume that: (cid:312) If ka is very large, assume that: Identify all the major species that can affect the ph.
