Reactions Flashcards
A Bronsted acid is a…
proton donor
A Bronsted base is a…
proton acceptor
A Lewis acid is an…
electron pair acceptor
A Lewis acid is an…
electron pair donor
What is an amphoteric substance?
A substance that reacts with both acids and bases
What is an amphiprotic substance?
A substance that can accept or donate protons
What is the difference between amphoteric and amphiprotic substances?
Amphiprotic substances specifically involve proton transfer while amphoteric is a more general term.
What is the autoprotolysis constant of water?
Kw = [H3O+][OH-]
How is pH found?
pH = -log[H3O+]
How is pOH found?
pOH = -log[OH-]
What is the correlation of pH and pOH in aqueous solutions?
pH + pOH = 14.00
What determines if an acid is strong/weak?
Deprotonation (full = strong, partial = weak)
What determines if a base is strong/weak?
Protonation (full = strong, partial = weak)
What is the value of Kw?
1.0 * 10^-14
What is a typical weak acid reaction?
Acetic acid (CH3COOH)
What is a typical weak base reaction?
Ammonia (NH3)
pKa values for strong acids are…
low
pKa values for weak acids are…
high
How can you determine a weaker or stronger oxoacid?
The amount of oxygen atoms (more oxygen = weaker bonds = lower pKa)
What are hypohalous acids?
A hydroxyl group bound to a halogen
What is the periodic trend of acid strength?
Increasing to the right (electronegativity)
Increasing downward (decreasing bond strength)
How is protonation percentage calculated?
(concentration of protonated species)/(initial concentration) * 100
How is the 5% rule checked?
What formula?
x / initial concentration
What equivalents of acid/base correspond to pKa values of a triprotic acid?
0.5 = pKa1
1.5 = pKa2
2.5 = pKa3
How can pH be calculated with similar concentrations of acid and conjugate base?
pH = (pka1 + pka2) / 2
How is solubility product expressed?
Ksp = [A+]^a [B-]^b
What is the common-ion effect?
The solubility of a solution will decrease if ions of a similar type are added
How does pH change affect solubility?
Solubility increases if pH decreases to account for decomposed ions
