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Difference between Ka and pKa.
Ka: Acid dissociation constant, measures acid strength (higher = stronger). pKa: -log(Ka), also measures acid strength (lower = stronger).
Difference between a strong acid and a weak acid in the context of buffers.
Strong Acid: Completely dissociates in solution, not suitable for buffers. Weak Acid: Partially dissociates, forms a buffer with its conjugate base.
Difference between using molarity and moles in the Henderson-Hasselbalch equation.
Molarity: Can be used if the volumes of the acid and conjugate base solutions are the same, so the volume cancels out in the ratio. Moles: Can always be used, regardless of volume, as the ratio is what matters.
Difference between equivalence point and half-equivalence point in a titration.
Equivalence Point: Moles of acid = moles of base. Half-Equivalence Point: Moles of acid = moles of conjugate base, pH = pKa.
Difference between acid and conjugate base.
Acid: Donates a proton (H+). Conjugate Base: Accepts a proton (H+).
Define a buffer solution.
A solution that resists changes in pH, consisting of a weak acid and its conjugate base (or a weak base and its conjugate acid).
Define pH.
A measure of acidity, calculated as -log[H+].
Define pKa.
-log(Ka), which indicates the acid's strength. A lower pKa means a stronger acid.
Define Ka.
The acid dissociation constant, a measure of the strength of an acid in solution.
What is the conjugate base?
The species formed when an acid donates a proton (H+).
Steps to find pH of a buffer (directly stated).
1. Calculate pKa. 2. Apply the Henderson-Hasselbalch equation: pH = pKa + log([A-]/[HA]).
Steps to find pH during a titration using the Henderson-Hasselbalch equation.
1. Write the net ionic equation. 2. Use stoichiometry to determine the amounts of acid and conjugate base after the reaction. 3. Apply the Henderson-Hasselbalch equation.
How to calculate pKa from Ka?
pKa = -log(Ka)
How to determine the concentrations of acid and conjugate base after the addition of a base in a titration?
Use stoichiometry based on the balanced net ionic equation to determine the remaining moles of acid and the moles of conjugate base formed.
Steps to determine pH using ICE table.
1. Set up an ICE (Initial, Change, Equilibrium) table. 2. Write the Ka expression. 3. Solve for [H+]. 4. Calculate pH = -log[H+].