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Understanding Acid-Base Equilibrium and Ka Calculations

In this lesson, students will learn to distinguish between weak and strong acids and write equilibrium expressions for various acids including HBr, H2SiO3, and HNO2. We will explore acid dissociation reactions and their Ka expressions, examining the dissociation of acids like HCl and HC2H3O2 while applying ICE box calculations. Students will also solve problems to find concentrations in solutions and understand what Ka values indicate about acid strength.

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Understanding Acid-Base Equilibrium and Ka Calculations

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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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