Acids and Bases

The study of Equilibrium- how far a reaction goes - accounts for 15-20% of the AP Chemistry Exam and is fundamental to understanding future units.

BIG IDEA 1: SCALE, PROPORTION, AND QUANTITY (SPQ)

Quantities in chemistry are expressed at both the macroscopic and atomic scale. Explanations, predictions, and other forms of argumentation in chemistry require understanding the meaning of these quantities, and the relationship between quantities at the same scale and across scales.

BIG IDEA 2: STRUCTURE AND PROPERTIES (SAP)

Properties of substances observable at the macroscopic scale emerge from the structures of atoms and molecules and the interactions between them. Chemical reasoning moves in both directions across these scales. Properties are predicted from known aspects of the structures and interactions at the atomic scale. Observed properties are used to infer aspects of the structures and interactions.

8: Acids and Bases

9: Buffers

10: Titration Curves

Show you have mastered the following 4 skills by...

Chemical equilibrium is a dynamic, reversible state in which rates of opposing processes are equal.
1. Read Chapter 15 pages 623 - 644 and complete the following:
  1. The Equilibrium Constant: 15.2, 15.5, 15.11, 15.13-15.19(odd), 15.23, 15.27
  2. Calculating Equilibrium Constants: 15.31-15.37 (odd), 15.7, 15.79, 15.47-15.59 (odd)
Systems at equilibrium respond to disturbances by partially countering the effect of the disturbance
1. Read Chapter 15 pages 644 - 654 and complete the following:
  1. Le Chatelier’s Principle: 15.61-15.67 (odd)
Chemical equilibrium plays an important role in acid-base chemistry
1. Read Chapter 16 pages 665 - 699 and complete the following:
  1. Bronsted-Lowry: 16.15-16.21 (odd)
  2. Autoionization of water: 16.27-16.31 (odd)
  3. Weak Acids: 16.51-16.57 (odd), 16.59 - 16.65 (odd)
  4. Ka & Kb: 16.77, 16.79
Chemical equilibrium plays an important role in acid-base chemistry and solubility
1. Read Chapter 17 pages 717 - 749 and complete the following:
  1. The Common-Ion Effect: 17.13-17.17 (odd)
  2. Buffers: 17.19-17.31 (odd)
  3. Acid-Base Titrations: 17.33-17.37 (odd), 17.43, 17.45
  4. Solubility Equilibria: 17.53-17.61 (odd), 17.69, 17.73, 17.75
  5. Visualizing Concepts: 17.1, 17.6-17.9
Solve all problems in the packet & master the unit vocabulary

The Equilibrium Constant: 15.13-15.27 (odd)
Calculating Equilibrium Constants: 15.31-15.37 (odd), 15.47-15.59 (odd)
Le Chatelier’s Principle: 15.61-15.67 (odd)
Visualizing Concepts: 15.2, 15.5, 15.7, 15.11
Additional Exercises: 15.76, 15.79, 15.82

Alignment to AP Learning outcomes

SPQ 4.B Identify the equivalence point in a titration based on the amounts of the titrant and analyte, assuming the titration reaction goes to completion.

SPQ 5.A Calculate the solubility of a salt based on the value of Ksp for the salt.

SPQ 5.B Identify the solubility of a salt, and/or the value of Ksp for the salt, based on the concentration of a common ion already present in solution.

SPQ 5.C Identify the qualitative effect of changes in pH on the solubility of a salt.

SPQ 5.D Explain the relationship between the solubility of a salt and changes in the enthalpy and entropy that occur in the dissolution process.

SAP 9.A Calculate the values of pH and pOH, based on Kw and the concentration of all species present in a neutral solution of water.

SAP 9.B Calculate pH and pOH based on concentrations of all species in a solution of a strong acid or a strong base.

SAP 9.C Explain the relationship among pH, pOH, and concentrations of all species in a solution of a monoprotic weak acid or weak base.

SAP 9.D Explain the relationship among the concentrations of major species in a mixture of weak and strong acids and bases.

SAP 9.E Explain results from the titration of a mono- or polyprotic acid or base solution, in relation to the properties of the solution and its components.

SAP 9.F Explain the relationship between the strength of an acid or base and the structure of the molecule or ion

SAP 10.A Explain the relationship between the predominant form of a weak acid or base in solution at a given pH and the pKa of the conjugate acid or the pKb of the conjugate base.

SAP 10.B Explain the relationship between the ability of a buffer to stabilize pH and the reactions that occur when an acid or a base is added to a buffered solution.

SAP 10.C Identify the pH of a buffer solution based on the identity and concentrations of the conjugate acid-base pair used to create the buffer.

SAP 10.D Explain the relationship between the buffer capacity of a solution and the relative concentrations of the conjugate acid and conjugate base components of the solution.

TRA 2.A Identify a reaction as acid-base, oxidation-reduction, or precipitation.

TRA 2.B Identify species as Brønsted-Lowry acids, bases, and/or conjugate acid-base pairs, based on proton-transfer involving those species.

TRA 6.A Explain the relationship between the occurrence of a reversible chemical or physical process, and the establishment of equilibrium, to experimental observations.

TRA 6.B Explain the relationship between the direction in which a reversible reaction proceeds and the relative rates of the forward and reverse reactions.

TRA 7.A Represent the reaction quotient Qc or Qp, for a reversible reaction, and the corresponding equilibrium expressions Kc=Qc or Kp=Qp.

TRA 7.B Calculate Kc or Kp based on experimental observations of concentrations or pressures at equilibrium.

TRA 7.C Explain the relationship between very large or very small values of K and the relative concentrations of chemical species at equilibrium.

TRA 7.D Represent a multistep process with an overall equilibrium expression, using the constituent K expressions for each individual reaction.

TRA 7.E Identify the concentrations or partial pressures of chemical species at equilibrium based on the initial conditions and the equilibrium constant

TRA 7.F Represent a system undergoing a reversible reaction with a particulate model.

TRA 8.A Identify the response of a system at equilibrium to an external stress, using Le Châtelier's principle.

TRA 8.B Explain the relationships between Q, K, and the direction in which a reversible reaction will proceed to reach equilibrium.

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