Strong Acid-Strong Base: Equivalence point pH is 7, no buffer region. Weak Acid-Strong Base: Equivalence point pH is >7, has a buffer region before the equivalence point.

Weak acid/strong base: pH > 7 at equivalence point. Strong acid/strong base: pH = 7 at equivalence point.

Equivalence point: Moles of titrant = moles of analyte. Half-equivalence point: Half the volume to reach the equivalence point; pH = pKa (or pOH = pKb) for weak acids/bases.

Weak acid with strong base: pH at equivalence point is basic. Weak base with strong acid: pH at equivalence point is acidic.

Strong acid-strong base: Sharp, abrupt change in pH near the equivalence point. Weak acid-strong base: More gradual change in pH, buffer region present, less sharp change at the equivalence point.

The solution with the unknown concentration in a titration.

The solution with the known concentration that is added to the analyte in a titration.

The point in a titration where the moles of titrant added equals the moles of analyte in the solution.

A plot of pH change versus the volume of titrant added during a titration.

The point in a weak acid/base titration where half of the acid/base has been neutralized, resulting in pH = pKa or pOH = pKb.

A solution that resists changes in pH due to the presence of a weak acid and its conjugate base, or a weak base and its conjugate acid.

1. Use the equation $M_aV_a = M_bV_b$. 2. Plug in the known values: $M_a(10 \text{mL}) = (0.1 \text{M})(20 \text{mL})$. 3. Solve for $M_a$: $M_a = (0.1)(20)/10 = 0.2 \text{M}$.

1. Write the balanced reaction equation. 2. Determine the initial moles of weak acid and strong base. 3. Perform stoichiometry to find the remaining moles of weak acid and conjugate base after the reaction. 4. Use the Henderson-Hasselbalch equation to calculate the pH.

1. Prepare the solutions of titrant and analyte. 2. Carefully add titrant to the analyte using a burette. 3. Monitor the pH change using an indicator or pH meter. 4. Stop adding titrant when the equivalence point is reached (indicated by a color change or a sharp pH change). 5. Calculate the unknown concentration using stoichiometry.

1. Write the balanced reaction equation. 2. Determine the initial moles of weak base and strong acid. 3. Perform stoichiometry to find the remaining moles of weak base and conjugate acid after the reaction. 4. Use the Henderson-Hasselbalch equation (for bases) to calculate the pOH. 5. Convert pOH to pH using pH = 14 - pOH.

1. Determine the moles of conjugate base formed at the equivalence point. 2. Calculate the concentration of the conjugate base. 3. Set up an ICE table for the hydrolysis of the conjugate base. 4. Calculate the hydroxide ion concentration using the Kb expression. 5. Calculate the pOH and then the pH.