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Conjugate Acid & Base Pairs Chapter 16

Conjugate Acid & Base Pairs Chapter 16

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Conjugate Acid & Base Pairs Chapter 16

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  1. Conjugate Acid & Base PairsChapter 16 John D. Bookstaver St. Charles Community College St. Peters, MO  2006, Prentice Hall, Inc. Chemistry, The Central Science, 10th edition Theodore L. Brown; H. Eugene LeMay, Jr.; and Bruce E. Bursten

  2. Some Definitions Arrhenius Acid: Substance that, when dissolved in water, increases the concentration of hydrogen ions. Base: Substance that, when dissolved in water, increases the concentration of hydroxide ions.

  3. Some Definitions Brønsted–Lowry Acid: Proton donor Base: Proton acceptor

  4. A Brønsted–Lowry acid… …must have a removable (acidic) proton. A Brønsted–Lowry base… …must have a pair of nonbonding electrons.

  5. If it can be either… is amphiprotic/amphoteric . HCO3− HSO4− H2O

  6. What Happens When an Acid Dissolves in Water? Water acts as a Brønsted–Lowry base and abstracts a proton (H+) from the acid. As a result, the conjugate base of the acid and a hydronium ion are formed.

  7. Conjugate Acids and Bases: From the Latin word conjugare, meaning “to join together.” Reactions between acids and bases always yield their conjugate bases and acids because a proton (H+) is transferred

  8. Practice Problem: • Label the acids and bases and their conjugates for the following: HCN + H2O ↔ CN- + H3O+

  9. Acid and Base Strength Strong acids are completely dissociated in water. Their conjugate bases are quite weak. Weak acids only dissociate partially in water. Their conjugate bases are weak bases.

  10. Strong Acids Review You will recall that the seven strong acids are HCl, HBr, HI, HNO3, H2SO4, HClO3, and HClO4. These are, by definition, strong electrolytes and exist totally as ions in aqueous solution. For the monoprotic strong acids, [H3O+] = [strong acid].

  11. Acid and Base Strength Substances with negligible acidity do not dissociate in water. Their conjugate bases are exceedingly strong.

  12. Strong Bases Strong bases are the soluble hydroxides, which are the alkali metal and heavier alkaline earth metal hydroxides (Ca2+, Sr2+, and Ba2+). Example: NaOH Again, these substances dissociate completely in aqueous solution. [OH-] = [strong base]

  13. Acid and Base Strength In any acid-base reaction, the equilibrium will favor the reaction that moves the proton to the stronger base. HCl(aq) + H2O(l) H3O+(aq) + Cl−(aq) H2O is a much stronger base than Cl−, so the equilibrium lies so far to the right K is not measured (K>>1).

  14. Acid and Base Strength C2H3O2(aq) + H2O(l) H3O+(aq) + C2H3O2−(aq) Acetate is a stronger base than H2O, so the equilibrium favors the left side (K<1).

  15. Strong or Weak, Acid or Base? • NaOH • HI • HF • Mg(OH)2 • CH3COOH • NH3 • H2SO4 • HCN • Ca(OH)2 • HClO4 • CN- • HCl • C2H2O2- • LiOH • HPO42- • HNO3