Acid-Base Equilibria Flashcards

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
Formula for % ionization
% 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
What are buffers?
Solutions that resist drastic pH changes upon addition of small amounts of acids or bases
27
Criteria for buffers (3)
1. Weak acid and salt of its conjugate base 2. Weak base and salt of its conjugate acid 3. 1 proton difference
28
How to know if it's a salt?
No charge since it should form an ionic compound
29
CH3COOH - NaCH3COO Equilibrium Rxn Buffering Action (Acid) Buffering Action (Base)
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
NH3 - NH4Cl Equilibrium Rxn Buffering Action (Acid) Buffering Action (Base)
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
Are buffering actions complete or partial dissociation?
Complete dissociation