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Strong Acids and Bases

hydrochloric, HCl . hydrobromic, HBr . hydroiodic, HI . chloric, HClO 3. perchloric, HClO 4. nitric, HNO 3. sulfuric, H 2 SO 4. -- these are strong electro- lytes that exist entirely as ions in aqueous solution . Strong Acids and Bases. -- memorize the names

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Strong Acids and Bases

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  1. hydrochloric, HCl hydrobromic, HBr hydroiodic, HI chloric, HClO3 perchloric, HClO4 nitric, HNO3 sulfuric, H2SO4 -- these are strong electro- lytes that exist entirely as ions in aqueous solution Strong Acids and Bases -- memorize the names and formulas of the seven strong acids... ...and the eight strong, hydroxide bases... the hydroxides of... Li, Na, K, Rb, Cs, Ca, Sr, Ba “strong base cations”

  2. e.g., HNO3(aq) H+(aq) + NO3–(aq) (“Who cares?”) o o o o o p p p p p Strong electrolytes are often written using a one-sided arrow. Find the pH of a 0.012 M perchloric acid solution. HClO4 H+ + ClO4– init. [ ] 0.012 0 0 final [ ] ~0 0.012 0.012 pH = –log [H+] = –log (0.012) = 1.92

  3. HNO3 H+ + NO3– If a nitric acid solution has pH = 2.66, find the solution’s concentration. [H+] = 10–pH = 10–2.66 = 2.2 x 10–3 M So orig. [HNO3] was also 2.2 x 10–3 M. Equipment for the production of nitric acid, formerly part of a U.S. military munitions plant in Joliet, IL.

  4. Barium hydroxide is used in the titration of weak acids, particularly organic acids, because a clear solution of Ba(OH)2 – unlike NaOH or KOH – will NOT contain any carbonates; carbonates would introduce errors into an analytical titration because the CO32– ion acts as a weak base. ** NOTE: Ca(OH)2, Sr(OH)2, and Ba(OH)2 are strong electrolytes, but have limited solubilities. This means that if you put a big chunk of any of these into water, little of the chunk will dissolve, BUT the little that does dissolve will float around as X2+(aq) and OH–(aq), NOT as X(OH)2(aq).

  5. (“w.c?”) 2.17 Find the pH of a 0.0034 M solution of calcium hydroxide. Ca(OH)2 Ca2+ + 2 OH– init. [ ] 0.0034 0 0 final [ ] ~0 0.0034 0.0068 pOH = –log [OH–] = –log (0.0068) = 2.17 pH + pOH = 14 pH = 11.83

  6. O2–(aq) + H2O(l) 2 OH–(aq) H–(aq) + H2O(l) H2(g) + OH–(aq) N3–(aq) + 3 H2O(l) NH3(aq) + 3 OH–(aq) OH! OH! OH! OH! OH! OH! OH! OH! OH! OH! OH! OH! OH! OH! OH! OH! OH! OH! Metal oxides, hydrides, and nitrides (containing O2–, H–, and N3–, respectively) also react with water to produce strongly basic solutions. e.g., -- -- --

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