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ACIDS AND BASES

ACIDS AND BASES. Distinguish between strong and weak acids and bases. Include: electrolytes and non-electrolytes. Additional KEY Terms concentrated dilute monoprotic diprotic.

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ACIDS AND BASES

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  1. ACIDS AND BASES

  2. Distinguish between strong and weak acids and bases. • Include: electrolytes and non-electrolytes Additional KEY Terms concentrated dilute monoprotic diprotic

  3. For a solution to conduct an electric current, charged particles or ions must be present in the solution.

  4. Electrolytesconductan electric current when in aqueous solution or when in a molten state. • Allioniccompounds act as electrolytes • (as dohighlypolar molecular compounds) • Mostmolecularcompounds are non-electrolytes. NaCl(s) Na+(aq) + Cl–(aq) C11H22O11(s) C11H22O11(aq) electrolytes non-electrolytes

  5. Only hydrogen in a very polar bond is ionizable • (H must be bonded to a very electronegative element) H - + + δ+ H Cl δ- O H H δ- δ+ C H C H H + +

  6. Electrolytes are classified as strong OR weak • Strong: produces many ions in solution. • dissociates 100% in water (NaCl) • Weak: partially dissociates (<<100%) in solution. • usually weak polar molecules (vinegar) A (s) B+(aq) + C–(aq)

  7. polar ionic

  8. ionic polar

  9. HCl (s) H+(aq) + Cl-(aq) water Strong acids are strong electrolytes: • easily donate protons • completely dissociateor ionize Indicate complete dissociation using single arrow [HCl]i = [H+]e= [Cl-]e

  10. HC2H3O2+ H2O H3O+ + C2H3O2- acetic acid Weak acids are weak electrolytes: • incompletelyionize • equilibrium reached between ions and acid Indicate equilibrium using reversible arrow The reverse reaction is favored over the forward one. The ions formed react very easily to reform the acid and the water.

  11. Strong bases are strong electrolytes: • easily accept protons • completely dissociate into OH-, or oxide, (O-2) Indicate complete dissociation using single arrow. water NaOH (s) Na+(aq) + OH-(aq) [NaOH]i= [Na+]e= [OH-]e

  12. Basically, any hydroxide and Alkali (1A) or Alkali-Earth Metal (2A) would be a strong base because of 100% dissociation

  13. Weak bases are weak electrolytes: • incompletelyionize • equilibrium reached between ions and base Indicate equilibrium using reversible arrow NH3(g) + H2O (l) NH4+(aq) + OH-(aq) Does not produce hydroxide ions readily. The reverse reaction is favored.

  14. Common weak bases are usually conjugate bases of strong acids. weak HA+ H2O H3O+ + A- Con. acid Con. base base acid In fact: The stronger the A/B, the weaker its conjugate. The weaker the A/B, the stronger its conjugate.

  15. Acid Strength Table

  16. Any acid that contains only one ionizable hydrogen is called monoprotic. Contains two ionizable hydrogens - diprotic Three - triprotic H O O H H s O O H Cl O p s O H O O H Phosphoric acid Sulfuric acid

  17. Acid Strength Table

  18. The equilibrium reaction favours the strongest acid.

  19. HCO3– + PO43– Which direction is favoured and why? fwd reaction is favoured HCO3–is the stronger acid

  20. THOUGHTS: • Don't confuse weak and strong with dilute and concentrated • Weak and strong indicates the proportionof an acid or base which ionized • Dilute and concentrated refer only to the volume of acid and base dissolved in a total solution volume • It is possible to have a concentrated weak acid/base or dilute strong acid/base

  21. HA H+ + A- H3O+ Strong Acid [I] 0 2.5 M 0 +x + x - x [C] H+ H2O HA+ H2O + A- 2.5 M 2.5 M 0 [E] HA+ H2O H3O+ + A- Weak Acid [I] 0 0 10 M - x +x + x [C] 1.0 M [E] 9.0 M 1.0 M

  22. CAN YOU / HAVE YOU? • Distinguish between strong and weak acids and bases. • Include: electrolytes and non-electrolytes Additional KEY Terms concentrated dilute monoprotic diprotic

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