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CHEM > Acid-Base Equilibria > Flashcards

Acid-Base Equilibria Flashcards

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1
Q

3 AUTHORS who defined Acids and Bases

A
  1. Arrhenius
  2. Bronsted-Lowry
  3. Lewis
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2
Q

DEFINITION OF ACIDS AND BASES

What did Arrhenius say?

A

Acid = [H+] in solution
Base = [OH-] in solution

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3
Q

DEFINITION OF ACIDS AND BASES

What did Bronsted-Lowry say?

A

Acid = (H+) donor
Base = (H+) acceptor

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4
Q

DEFINITION OF ACIDS AND BASES

What did Lewis say?

A

Acid = e- pair acceptor
Base = e-pair donor

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5
Q

2 properties of Water

A

Amphoteric = can be an acid or a base
Amphiprotic = can accept o donate a proton

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6
Q

Equation Reaction for Water

A

2H2O (l) -> <- H3O+ (aq) + OH- (aq)

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7
Q

What is the ION-PRODUCT CONSTANT and its value for water

A

Kw

Kw of water = 1.0 x 10^-14 at 25 C

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8
Q

4 formulas based on ion-product constant

A
  1. pH = -log [H3O+]
  2. pOH = -log [OH-]
  3. pKw = -log Kw
  4. pKw = pH + pOH = 14.00
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9
Q

Do K eq values have a unit? If so, what is it?

A

No

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10
Q

Shortcut in identifying shift of rxn based on acids and bases

A

If H3O + is a product, find and compare the reactant and product base. Weaker base -> dito ung shift

If OH- is a product, find and compare the reactant and product acid. Weaker acid -> dito ung shift

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11
Q

SHIFT IN ACID-BASE RXNS

HCl + H2O -> H3O+ + Cl-

A

H3O+ so compare the bases

RB: H2O
PB: Cl-

HCl is a strong acid so its conjugate base (Cl-) is a very weak base. Thus, the reaction shift is forward, and the formation of H3O+ is favoured

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12
Q

SHIFT IN ACID-BASE RXNS

CH3COOH + H2O -> <- H3O+ + CH3COO-

A

H3O+ so compare the bases

RB: H2O
PB: CH3COO-

CH3COOH is not a strong acid so its conjugate base (Cl-) is stronger base compared to water. Thus, the reaction shift is reverse, and the formation of CH3COOH is favoured

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13
Q

Relationship between Acids and Bases

A

The stronger the Acid, the weaker the Base

Kaya… every conjugate base of a strong acid is weaker than water

every conjugate acid of a strong base is weaker than water

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14
Q

Strong Acids Examples (8)

A

HCl
HBr
HI
HNO3
H2SO4
HClO3
HClO4
Sulfonic Acids

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15
Q

Strong Bases Examples (9)

A

Commonly Group 1 & 2 + OH

LiOH
NaOH
KOH
RbOH
CsOH
Ca(OH)2
Sr(OH)2
Ba(OH)2
ammonium hydroxides

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16
Q

What is the MOST important rule before doing anything?

A

BALANCE THE EQUATION

17
Q

REVIEW!!!

Name the Weak ACIDS/BASES and their conjugates

1.) H2O -> H3O+
2.) H2O -> OH-

A

1.) Weak Base: H2O ; Conjugate Acid: H3O+
2.) Weak Acid: H2O ; Conjugate Base : OH-

18
Q

SF rules in Logarithmics

A

The # of SF in argument will become the # of decimal points in final answer

19
Q

What will be the equation of Ca(OH)2 (aq)?

A

Ca(OH)2 is a strong base so one arrow will be used

+ will dissolve into ions

Ca(OH)2 -> (w/ H2O) -> Ca2+ + 2OH-

20
Q

What will be the equation of HCl (aq)?

A

HCl is a strong acid so one arrow will be used

+since acid, H2O (l) will be in reactants side to form H3O+

HCl + H2O (l) -> H3O+ + Cl -

21
Q

Formula for Kw using Ka and Kb

A

Kw = (Ka)(Kb)

22
Q

Relationship of

Ka & strength of acid
Kb & strength of base

A

both direct relationship

23
Q

What should be shown in solution when there is a need to solve for x using quadrating equation?

A

SHOW:

Ax^2 + Bx + C = 0

24
Q

If pH or pOH is given and we want to fine the value of H3O+ or OH -, WHAT to do?

A

antilog

10^NEGATIVE pH/pOH

25
Q

Formula for % ionization

A

% ionization = (amount dissociated) / (initial concentration) x 100

% ionization = (equilibrium concentration) / (initial concentration) x 100

% ionization = (conjugate / weak acid or base not h2o) x 100

26
Q

What are buffers?

A

Solutions that resist drastic pH changes upon addition of small amounts of acids or bases

27
Q

Criteria for buffers (3)

A
  1. Weak acid and salt of its conjugate base
  2. Weak base and salt of its conjugate acid
  3. 1 proton difference
28
Q

How to know if it’s a salt?

A

No charge since it should form an ionic compound

29
Q

CH3COOH - NaCH3COO

Equilibrium Rxn
Buffering Action (Acid)
Buffering Action (Base)

A

Since CH3COOH will donate a proton, it is a weak acid

CH3COOH + H2O (l) -><- CH3COO- + H3O+ (aq)

addition of ACID:
CH3COO- + H3O+ (aq) -> CH3COOH + H2O (l)

addition of BASE:
CH3COOH + OH- (aq) -> CH3COO- + H2O (l)

30
Q

NH3 - NH4Cl

Equilibrium Rxn
Buffering Action (Acid)
Buffering Action (Base)

A

Since NH3 will receive a proton, it is a weak base

NH3 + H2O (l) -><- NH4+ + OH- (aq)

addition of ACID:
NH3 + **H3O+ (aq) ** -> NH4 + H2O (l)

addition of BASE:
NH4+ + **OH- (aq) ** -> NH3 + H2O (l)

31
Q

Are buffering actions complete or partial dissociation?

A

Complete dissociation

CHEM (22 decks)

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