Unit 8: Acids and Bases.

8.1 Introduction to Acids and Bases.

Calculate the value of pH, pOH, [H⁺], or [OH⁻] given one of the values.

  1. A solution has a pH of 8.00 at 25oC. What is the pOH?
  2. The [OH-] of a solution is 0.300M determine the [H3O+].

8.2 pH and pOH of Strong Acids and Bases.

Identify strong acids by memorization.

  1. List the 6 strong acids.

Calculate the pH, pOH, [H3O+], or [OH-] of a strong acid or base from its concentration.

  1. What is the pH of 2.5M HCl?
  2. What are the [H3O+] and [OH-] concentrations of a 1.0M Ca(OH)2 solution?

8.3 Weak Acid and Base Equilibria.

Compare strong vs. weak acids and bases.

Use a Ka expression to calculate the pH of a weak acid (or Kb for a weak base).

Calculate the pKa of a weak acid or pKb of a weak base.

Determine the % ionization of a weak acid or base given its pKa (or pKb) and starting concentration.

8.4 Acid-Base Reactions and Buffers.

Determine the pH of a solution after complete neutralization of a strong acid and strong base.

Write the equation for acid-base reactions (strong-strong, weak-strong, or weak-weak).

Determine the pH of a solution after neutralization.

8.5 Acid-Base Titrations.

Produce a titration curve.

Identify key areas on a titration curve: equivalence point, half-equivalence point, buffering region.

Use the shape of a titration curve to determine if an acid is mono-, di-, or triprotic.

Identify the major species present at any point on a titration curve.

8.6 Molecular Structure of Acids and Bases.

Identify a strong acid or base by memorization.

Identify the acidic proton in a carboxylic acid.

Justify the strength of an acid by examining the electronegativity of the anion.

8.7 pH and pKa.

Determine if a weak acid or conjugate base is in higher concentration by comparing pH and pKa.

Select an appropriate indicator for a titration.

8.8 Properties of Buffers.

Determine if a solution is a buffer.

Explain how a buffer solution stabilizes the pH of a system.

8.9 Henderson-Hasselbalch Equation.

Use the Henderson-Hasselbalch equation to determine the pH of a buffer solution.

Qualitatively describe how a buffer resists pH changes when acid or base is added.

8.10 Buffer Capacity.

Qualitatively describe whether a given buffer can accommodate additional acid or base.

8.11 pH and Solubility.

Determine if the solubility of a salt will be impacted by the pH of the solvent.s

Explain the impact of pH on solubility using Le Châtelier’s principle.

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