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Chemistry 12 > Properties of Acids and Bases > Flashcards

Properties of Acids and Bases Flashcards

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1
Q

Acids

A

Donate a proton (H+ or H3O+)

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2
Q

Monoprotic Acid

A

Can only donate one proton
HCL –> H+ +Cl-

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3
Q

Diprotic Acid

A

Can donate two protons
H2SO4 –> H+ +HSO4-
HSO4- –> H+ +SO4 (2-)

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4
Q

Triprotic Acid

A

Can donate three protons
H3PO4 –> H+ +H2PO4-
H2PO4- –> H+ +HPO4 (2-)
HPO4 (2-) –> H+ +PO4 (3-)

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5
Q

Bases

A

Reacts with acids to produce salt and water

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6
Q

Hydroxide

A

NaOH –> Na+ +OH-

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7
Q

Oxide (with water)

A

Na2O + H2O –> 2Na+ + 2OH-

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8
Q

Ammonia (with water)

A

NH3 + H2O –> NH4+ +OH-

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9
Q

Acid/base strength

A

Strong acid/base dissociates completely in water
Weak acid/base dissociates partially in water

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10
Q

Acid/base concentration

A

Concentrated: large amount of acid/base dissolved in solvent
Dilute: small amount of acid/base dissolved in solvent

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11
Q

Bronsted Lowry Acid

A

Donates a proton (H+)

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12
Q

Bronsted Lowry Base

A

Accepts a proton (H+)

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13
Q

Conjugate Acid Base Pairs

A

Two species that differ by a proton
An acid donates a proton to become a conjugate base
A base accepts a proton to become a conjugate acid

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14
Q

Amphiprotic Substance

A

Can act as an acid or base

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15
Q

pH+ pOH

A

14

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16
Q

Calculating pH with H+ concentration (same for oH)

A

pH = -log H+ concentration

17
Q

Calculating H+ concentration with pH (same for OH- concentration)

A

H+ concentration = 10 ^ -pH

18
Q

Ionic Product Constant of Water

A

Equilibrium constant for the reaction in which water acts as both a base and an acid simultaneously
H2O (reversible arrow) H+ + OH-

Kw = 10^-14

Kw= Ka X Kb

19
Q

pKa (same for pKb)

A

-log Ka

20
Q

Initial pH on a titration curve

A

Shows if acid or base is in conical flask, and strength of acid/base
Can calculate initial H+ concentration using pH

21
Q

Equivalence point on a titration curve

A

pH value where all moles of base have reacted with all moles of acid in conical flask (solution is neutral)

22
Q

Half equivalence point on titration curve

A

When half the volume of base that is required to react with all the moles of acid has been added
pH = pKa at this point

23
Q

Buffer region on titration curve

A

Only occurs with weak acid/base in conical flask
Region before equivalence point where pH changes slowly due to weak acid/base behaving as a buffer - lots of undissociated molecules shifting right to replace H+

24
Q

Strong Acid Strong Base Titration Curve

A

Initial pH is low
Equivalence point when pH = 7
No buffer region

25
Q

Weak Acid Strong Base Titration Curve

A

Initial pH is higher than strong acid
Equivalence point when pH > 7
Buffer region

26
Q

Strong Acid Weak Base Titration Curve

A

Initial pH is lower than strong base
Equivalence point when pH < 7
Buffer region

27
Q

Acid dissociation constant

A

When acid dissolves in water it produces an anion and a hydronium ion ( H3O+ )

HA + H2O <–> H3O+ + A-

28
Q

Acid dissociation constant expression

A

HA + H2O <–> H3O+ + A-

Ka = [H3O+][A-]/[HA]

Ka value only applies to weak acids as strong acids completely dissociate
Large Ka value means a stronger acid, as there are more products meaning more dissociation

29
Q

Base dissociation constant

A

When a base dissolves in water it produces a cation and a hydroxide ion
B + H2O <–> BH+ + OH-

Kb values only applies to weak bases as strong bases completely dissociate
Large Kb value means a stronger base, as there are more products meaning more dissociation

30
Q

Base dissociation constant expression

A

B + H2O <–> BH+ + OH-

Kb = [BH+][OH-]/[B]

31
Q

Kw

A

Ka x Kb

32
Q

pKa

A

pKa is to Ka what pH is to [H+]

pKa = -log Ka

pKa values only apply to weak acids as strong acids completely dissociate

33
Q

Weak acid has a __ conjugate base

A

strong

34
Q

Strong acid has a __ conjugate base

A

weak

Chemistry 12 (25 decks)

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