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Get ready for upcoming exams and lab activities! Learn about metal hydroxide solubility, pH titration, LeChatelier's Principle, and more. Quick open-book quiz at the end of class today!

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Announcements

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  1. Exams will be handed back in lab next week. Quick “open-book” quiz at end of class today. Announcements

  2. Lab Information • Metal hydroxide solubility • pH titration (on Friday)

  3. An equilibrium will shift in response to change in the system or its environment • LeChatelier’s Principle If a chemical system at equilibrium experiences a change in concentration, temperature, volume, or partial pressure, then the equilibrium shifts to counteract the imposed change and a new equilibrium is established.

  4. The effect of concentration changes on equilibria Add product [C] Remove reactant [A] Remove all of reactant [B] and product [D]

  5. The effect of volume changes on equilibria • Equilibrium will shift to side with fewer moles of gas

  6. The effect of temperature changes on equilibria • Endothermic reactions • Exothermic reactions

  7. LeChatelier’s Principle- Quantitative • 1-Liter flask contains 0.50 mol butane and 1.25 mol isobutane (at equilibrium). We then add 0.50 mol and butane. What happens and what are the final concentrations of isobutane and butane?

  8. Chapter 16 Acid-base equilibria

  9. Acids and Bases- Overview • pH and pOH • Relationship of conjugate pair acid-base strength. • When acids or bases control pH: • determine K • predict pH • When pH controls acid/base state: • predict acid/base state • use acid/base state to determine pH • Buffer action • pH titration curves

  10. pH and pOH

  11. Water autoionization

  12. pH and pOH calculations • What is the pH of [H3O+] = 4.6 x 10-5? • What is the pOH of [OH-] = 3.3 x 10-4? • What is the pOH of [H3O+] = 4.6 x 10-5? • What is the [H3O+] when the pH = 4.2? [H3O+][OH-] = 1.0 x 10-14 pH = -log[H3O+] pOH = -log[OH-] [H3O+] = 10-pH [OH-] = 10-pH pH + pOH = 14.00

  13. What is the pH when [H3O+] = 0.045 M? • 0.045 • 13.995 • -1.35 • 1.35

  14. What is the pH when [OH-] = 6.5 x 10-4 M? • 3.18 • -3.18 • 10.81 • 15.18

  15. What is the [H3O+] when pH = 3.66 M? • 2.18 x 10-4 • 10.34 • 4570 • 3.66

  16. What is the [OH-] when pH = 5.84 M? • 1.45 x 108 • 3.31 x 10-6 • 6.92 x 10-9 • 5.84

  17. Strong acids and bases ionize completely • Strong monoprotic acids [H3O+] = [acid] • Strong diprotic acid [H3O+] = 2[acid] • Strong monoprotic base [OH-] = [base] • Strong diprotic base [OH-] = 2[base]

  18. Quiz time!

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