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18 Dec 2019
1) Find the pH of 0.151 M phenol, C6H5OH. The H bonded to the O is acidic, that is,
C6H5OH(aq) + H2O(l) â H3O+(aq) + C6H5O-(aq). Ka = 1.0 x 10-10 M.
2) Calculate the approximate [OH-] and [NH4+] in a 0.15 M ammonia solution, NH3(aq).
NH3(aq) + H2O(l) â OH-(aq) + NH4+(aq). Kb = 1.75 x 10-5M.
3) Calculate the pH of 0.197 M ammonia.
NH3(aq) + H2O(l) â OH-(aq) + NH4+(aq) Kb = 1.75 x 10-5
4) Calculate the pH of 0.124 M phosphoric acid (H3PO4, a triprotic acid). Ka1 = 7.5 x 10-3, Ka2 = 6.2 x 10-8, and Ka3 = 4.8 x 10-13.
1) Find the pH of 0.151 M phenol, C6H5OH. The H bonded to the O is acidic, that is,
C6H5OH(aq) + H2O(l) â H3O+(aq) + C6H5O-(aq). Ka = 1.0 x 10-10 M.
2) Calculate the approximate [OH-] and [NH4+] in a 0.15 M ammonia solution, NH3(aq).
NH3(aq) + H2O(l) â OH-(aq) + NH4+(aq). Kb = 1.75 x 10-5M.
3) Calculate the pH of 0.197 M ammonia.
NH3(aq) + H2O(l) â OH-(aq) + NH4+(aq) Kb = 1.75 x 10-5
4) Calculate the pH of 0.124 M phosphoric acid (H3PO4, a triprotic acid). Ka1 = 7.5 x 10-3, Ka2 = 6.2 x 10-8, and Ka3 = 4.8 x 10-13.
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