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ARRHENIUS ACID

ARRHENIUS ACID. Any compound that contains hydrogen and dissociates in aqueous solution to form H + ions. HNO 3 (aq) H + (aq) + NO 3 (aq). ¾. H. O. 2. ¾. ¾. ®. Nitric acid dissociates completely, as shown below:. ARRHENIUS BASE.

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ARRHENIUS ACID

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  1. ARRHENIUS ACID Any compound that contains hydrogen and dissociates in aqueous solution to form H+ ions.

  2. HNO3(aq) H+ (aq) + NO3 (aq) ¾ H O 2 ¾ ¾ ® Nitric acid dissociates completely, as shown below:

  3. ARRHENIUS BASE Any compound that contains OH- ions and dissociates to produce OH- ions in aqueous solutions.

  4. KOH (s) K+ (aq) + OH-(aq) ¾ H O 2 ¾ ¾ ® Potassium hydroxide dissociates in water as shown in the following equation:

  5. TYPES OF ACIDS Monoprotic and polyprotic acids differ in relative number of ionizable hydrogen ions. • Monoprotic • HCl • HBr • HI

  6. BRONSTED ACIDS AND BASES A Bronsted acid is a proton (hydrogen ion) donor. A Bronsted base is a proton (hydrogen ion) acceptor.

  7. NH3 + H2O NH4+ + OH- The hydrogen ion H+ actually exists only as the hydronium ion H3O+

  8. PROPERTIES OF ACIDS • sour taste • turn blue litmus red • an electrolite • react with bases to form water and salt • react with metals and release hydrogen

  9. PROPERTIES OF BASES • bitter taste. • electrolites. • slippery. • change red litmus blue. • react with acids to form water and salt.

  10. Equivalents One equivalent of an acid is equal to the quantity in grams that supplies one mole of protons.

  11. One equivalent of a base is the quantity in grams that accepts one mole of protons, or supplies one mole of OH- ions. Equivalents of solute = Normality Liters of solution

  12. + - 1 mole H O 1 mole OH 3 and 7 7 1 x 10 liters water 1 x 10 liters water Ionization of Water (Kw) Water ionizes only very slightly. The concentration of hydronium and hydroxide ions is:

  13. - + - - 7 7 1 x 10 moles H O 1 x 10 moles OH 3 and liter H O liter H O 2 2 Or:

  14. Using standard notation: [H3O+] = 1x10-7 mol/L [OH-] = 1x10-7 mol/L

  15. The ionization constant for water is as follows: Kw = [H3O+] x [OH-] = (1x10-7)2 = 1x10-14 Example: [H3O+] = .001 M or 1x10-3 M \ [OH-] = 1x10-14 ¸ 1x10-3 = 1x10-11 M

  16. pH The pH of a solution is equal to the negative log of the hydronium concentration. [H3O+] = 1x10-5 M pH = - (-5) = 5 pOH = (14 - 5) = 9

  17. If the pH of a solution is less than 7, it is considered to be acidic. If the pH is greater than 7, the solution is considered basic.

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