Reactions Flashcards

1
Q

A Bronsted acid is a…

A

proton donor

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2
Q

A Bronsted base is a…

A

proton acceptor

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3
Q

A Lewis acid is an…

A

electron pair acceptor

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4
Q

A Lewis acid is an…

A

electron pair donor

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5
Q

What is an amphoteric substance?

A

A substance that reacts with both acids and bases

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6
Q

What is an amphiprotic substance?

A

A substance that can accept or donate protons

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7
Q

What is the difference between amphoteric and amphiprotic substances?

A

Amphiprotic substances specifically involve proton transfer while amphoteric is a more general term.

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8
Q

What is the autoprotolysis constant of water?

A

Kw = [H3O+][OH-]

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9
Q

How is pH found?

A

pH = -log[H3O+]

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10
Q

How is pOH found?

A

pOH = -log[OH-]

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11
Q

What is the correlation of pH and pOH in aqueous solutions?

A

pH + pOH = 14.00

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12
Q

What determines if an acid is strong/weak?

A

Deprotonation (full = strong, partial = weak)

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13
Q

What determines if a base is strong/weak?

A

Protonation (full = strong, partial = weak)

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14
Q

What is the value of Kw?

A

1.0 * 10^-14

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15
Q

What is a typical weak acid reaction?

A

Acetic acid (CH3COOH)

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16
Q

What is a typical weak base reaction?

A

Ammonia (NH3)

17
Q

pKa values for strong acids are…

18
Q

pKa values for weak acids are…

19
Q

How can you determine a weaker or stronger oxoacid?

A

The amount of oxygen atoms (more oxygen = weaker bonds = lower pKa)

20
Q

What are hypohalous acids?

A

A hydroxyl group bound to a halogen

21
Q

What is the periodic trend of acid strength?

A

Increasing to the right (electronegativity)
Increasing downward (decreasing bond strength)

22
Q

How is protonation percentage calculated?

A

(concentration of protonated species)/(initial concentration) * 100

23
Q

How is the 5% rule checked?

What formula?

A

x / initial concentration

24
Q

What equivalents of acid/base correspond to pKa values of a triprotic acid?

A

0.5 = pKa1
1.5 = pKa2
2.5 = pKa3

25
Q

How can pH be calculated with similar concentrations of acid and conjugate base?

A

pH = (pka1 + pka2) / 2

26
Q

How is solubility product expressed?

A

Ksp = [A+]^a [B-]^b

27
Q

What is the common-ion effect?

A

The solubility of a solution will decrease if ions of a similar type are added

28
Q

How does pH change affect solubility?

A

Solubility increases if pH decreases to account for decomposed ions