Acid-Base Vocabulary
What is the proton Acceptor in a Bronsted-Lowry reaction? What is the name of the molecule formed by this substance receiving a proton?
Bronsted-Lowry Base, Conjugate Acid.
What has a value of 1.0 x 10-14?
Kw
Which reaction correlates with a BCA Table? ICE Table?
BCA- Completion Reaction
ICE- Equilibrium Reaction
What determines if an ion is pH-neutral?
If it is the conjugate of a strong acid or strong base.
What term describes the maximum amount of acid or base a buffer can neutralize?
Buffer capacity.
What describes a molecule capable of donating OR accepting the proton in a Bronsted-Lowry reaction?
Amphipathic/Amphiprotic. Ex: Water
How do you convert from Ka to Kb or vice-versa?
Kw = Ka x Kb
What type of reaction is a Base Dissociation Reaction?
Completion- Strong bases fully dissociate into it's ions.
How will Sr(BrO)₂ affect pH?
The solution will become BASIC since BrO⁻ is the conjugate of a weak acid, HBrO.
(Sr2+ will not affect, as it is pH Neutral.)
What is the range where buffers are most effective?
When pH is +/- 1 pKa.
In an acid-base titration reaction, what do you call the solution of known concentration being added? The solution of unknown concentration being added to?
What do you call a compound used to visually indicate a pH range?
Titrant, Analyte, Indicator.
What has a value of 14.00?
The sum of pH and pOH, and the sum of pKa and pKb: pKw.
What determines the completion vs equilibrium status of the Acid Ionization Reaction?
Strong acids ionize to completion, weak acids ionize to equilibrium.
How will CH₃NH₃I affect pH?
The solution will become ACIDIC since CH₃NH₃⁺ is the conjugate of a weak base, CH₃NH₂.
(I- will not affect, as it is pH Neutral.)
What does the equivalence point represent in a buffer titration?
The point in which acids and bases are equal in solution. (the buffer is fully neutralized)
What is the term for an acid capable of donating multiple protons? What type of equilibrium is present here?
Bonus: What does this imply about it's uses in buffers?
Polyprotic acid. Multiple Equilibria.
Bonus: a polyprotic acid buffer will have multiple buffering regions due to it's multiple Ka values.
What K expression does Kw represent?
Kw= [H3O+] [OH-] aka Autoionization of Water
What does a BCA Table represent in acid-base equilibria, and what must happen afterwards to find a final concentration?
BCA Tables represent Neutralization, after which we must calculate the shift in equilibrium using an ICE table or the Henderson-Hasselbalch equation.
How do you determine how a salt affects pH with a weakly acidic cation and a weakly basic anion?
Compare the ka for the cation with the kb for the anion, usually derived from its conjugate's known k. [ex: ka NH4+ = kw / kb NH3]
ka cation > kb anion, acidic; ka cation < kb anion, basic.
Where along a titration curve is the half-equivalence point? What does the pH equal here?
The half-equivalence point lies in the buffering region, where pH = pKa (or pOH = pKb).