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Objective/Warm-Up

Objective/Warm-Up. SWBAT distinguish between weak and strong acids and write equilibrium expressions. Name these acids: HBr H 3 P H 2 SiO 3 HNO 2. Acid/Base Equilibrium. General formula for an Acid dissociation reaction: HA + H 2 O ↔ H 3 O + + A - Or: HA ↔ H + + A -.

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Objective/Warm-Up

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  1. Objective/Warm-Up • SWBAT distinguish between weak and strong acids and write equilibrium expressions. • Name these acids: • HBr • H3P • H2SiO3 • HNO2

  2. Acid/Base Equilibrium • General formula for an Acid dissociation reaction: • HA + H2O ↔ H3O+ + A- • Or: HA ↔ H+ + A-

  3. Write the dissociation equation for each of the following acids: • HCl • HC2H3O2 • NH4+ • C6H5NH3+ • H2O

  4. Equilibrium Constant • HA + H2O ↔ H3O+ + A- • HA ↔ H+ + A- • Ka = [H3O+][A-] or Ka = [H+][A-] [HA] [HA] • Brackets indicate concentration (molarity).

  5. Write the Ka equation for each of the following acids: • HCl • HC2H3O2 • NH4+ • C6H5NH3+ • H2O

  6. What does Ka tell us?

  7. Figure 14.4Graphic Representation of the Behavior of Acids of Different Strengths in Aqueous Solution

  8. Same for bases: Kb • B + H2O ↔ HB+ + OH- • Kb = [HB+][OH-] [B]

  9. ICE box calculations • Calculate the [H+] and [F-] in a 1.00 M solution of HF if the Ka is 7.2 x 10-4. • Write Ka expression.

  10. ICE box calculations • Calculate the initial concentration of HF in a solution where the pH = 4.7 and the Ka is 7.2 x 10-4. • Write Ka expression.

  11. Practice Problems 18-2

  12. Objective/Warm-Up • SWBAT solve ICEbox problems for acids and bases. • Write dissociation equations and equilibrium expressions for the following acids: • HNO2 • H2C2O4 • HF

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