Equilibria Involving Ions

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Anonymous
ID:
192267
Filename:
Equilibria Involving Ions
Updated:
2013-01-11 13:17:15
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Chemistry
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Description:
Advanced Higher Chemistry - Unit Two - Equilibria involving ions
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  1. What is the Bronsted-lowry definition of an acid?
    An acid is a proton donor
  2. What is the Bronsted-lowry definition of an alkali?
    An alkali is a proton acceptor
  3. For every acid there is a conjugate base, formed by the ____ of a proton?
    loss
  4. For every alkali there is a conjugate acid, formed by the ____ of a proton?
    gain
  5. What equation can the ionisation of water be represented by?
    H2O(l) + H2O(l) ↔ H3O+(aq) + OH-(aq)
  6. Is water amphoteric?
    Yes, it can act as an acid or a base
  7. The dissociation constant for the ionisation of water is known as the ionic product and is represented by...?
    • Kw = [H3O+][OH-]
    • Or more simply Kw = [H+][OH-]
  8. What does the value of the ionic product vary with?
    Temperature
  9. At 25˚C what is the value of Kw?
    Approximately 1 x 10-14 mol l-1
  10. What equation is used to calculate the pH of a solution?
    pH = -log[H+]
  11. What does this equation represent?
    HA(aq) + H2O(l) ↔ H3O+(aq) + A-(aq)
    The dissociation in aqeous solution of an acid of general formula HA
  12. How is the acid dissociation constant of acid HA given by?
    Ka = [H3O+][A-] / [HA]
  13. What is the conjugate base of an acid of general formula HA?
    A-
  14. The dissociation constant of an acid can be represented by pKa where..?
    pKa = -log Ka
  15. How is the relationship of the pH of a weak acid to its dissociation constant represented?
    • pH = 0.5pKa - 0.5logc
    • (c = concentration)
  16. What does this equation represent?
    B(aq) + H2O(l) ↔ BH+(aq) + OH-(aq)
    The dissociation in aqueous solution of a base of general formula B
  17. What is the conjugate acid of a base of general formula B?
    BH+
  18. How can the dissociation of the conjugate acid of the base be represented as?
    BH-(aq) + H2O(l) ↔ B(aq) + H3O-(aq)
  19. How is the dissociation constant of the conjugate acide represented?
    Ka = [B][H3O-] / [BH+]

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