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Drill – 6/1/11

Drill – 6/1/11. How would the following shift the equilibrium in the equation (forward, reverse or no change): H + (aq) + Cl - (aq) ↔ HCl (aq) + 10.3 kJ Increasing temperature Decreasing pressure Adding NaCl Adding NaOH. Different Types of Equilibrium.

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Drill – 6/1/11

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  1. Drill – 6/1/11 • How would the following shift the equilibrium in the equation (forward, reverse or no change): H+ (aq) + Cl- (aq) ↔ HCl (aq) + 10.3 kJ • Increasing temperature • Decreasing pressure • Adding NaCl • Adding NaOH

  2. Different Types of Equilibrium

  3. Remember…equilibrium is where the rates of forward and reverse reactions are the same. It means that the concentrations do not change, NOT that they are identical.

  4. Because equilibrium expressions have to do with concentration (in molarity) we do not include items that are not in solution so NO LIQUID or SOLID states! They are in excess so can be ignored.

  5. Concentration Equilibrium Kc (or Keq) • nA + mB ↔ xC + yD • Kc = [C]x[D]y [A]n[B]m

  6. Acid Equilibrium • Acid + H2O ↔ H3O+ + Acid Ion or HA + H2O ↔ H3O+ + A- Ka = [H3O+][A-] Ka = [H3O+][A-] [HA][H2O] [HA] Because water is a solvent and it’s conc. greatly exceeds the acid, we can assume that the conc. of water does not change.

  7. Base Equilibrium • Base + H2O ↔ OH- + Base Ion or B + H2O ↔ OH- + HB+ Kb = [OH-][HB+] Kb = [OH-][HB+] [B][H2O] [B]

  8. Graphic Representation of the Behavior of Acids of Different Strengths in Aqueous Solution

  9. Solubility Equilibrium • Salt (s) ↔ Cation (aq) + Anion (aq) • Solids are not included in equilibrium equations! So… • Ksp = [Cation][Anion]

  10. Solubility Equilibrium Example • CaF2 (s) ↔ Ca+2 (aq) + 2F- (aq) • Solids are not included in equilibrium equations! So… • Ksp = [Ca+2][F-]2

  11. Workbook • Pg. 242 #2, 3, 4 • Pg. 250 #1 & 2 • Pg. 252 #1

  12. Drill – 5/25/10 • Consider the following equilibrium system: NaCN (s) + HCl (g) ↔ HCN (g) + NaCl (s) • Write the equilibrium expression for this system • The Keq for this reaction is 2.405x106. What is the concentration of HCl when the concentration of HCN is 0.8959M?

  13. Remember: No solids or liquids in equilibrium expressions

  14. A saturated solution of magnesium bromide has a concentration of 1.50x10-4M. Calculate the Ksp.

  15. Workbook • Pg. 242 #2, 3, 4 • Pg. 250 #1 & 2 • Pg. 252 #1

  16. ICE Box WS

  17. N2(g) + 3H2(g)  2NH3(g) Initially you have .86M nitrogen and .72M hydrogen. What is the concentration of ammonia at equilibrium if the Ksp is 4.5 x 10-5

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