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Physical Pharmacy > pH and Buffer > Flashcards

pH and Buffer Flashcards

1
Q

Substances that dissociates when dissolved in water and produces H+

A

Arrhenius Acids

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2
Q

Substances that dissociates and release OH- ions

A

Arrhenius Bases

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3
Q

Limitations onf Arrhenius Theory

A
  1. Arrhenius theory is limited to behavior of acids and bases in aqeous solutions and not in non-aqueous media.
  2. Manu substances do not have H+, but behave as acids (NH4Cl, CO2)
  3. Substances do not have Oh-, but behave as bases (Na2CO3, CaO)
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4
Q

The complete separation of ions in a crystal lattice when a salt is dissolved

A

Ionization

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5
Q

Separation of ions in solution when the ions are associated by interionic attraction

A

Dissociation

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6
Q

Hydrogen-containing substance that donates a proton/H+ to another substance

A

Bronsted-Lowry Acids

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7
Q

Substance that accepts a proton/H+

A

Brownsted-Lowry Bases

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8
Q

Molecule that can accept a pair of e- to form a dative bond

A

Lewis Acids

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9
Q

Molecule that can donate a pair of e- to form a dative bond

A

Lewis Bases

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10
Q

Acid dissociation constant/Acidity Constant

A

Ka

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11
Q

TF:
↑ Ka ↑Acidity
↓ pka ↑Acidity

A

True

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12
Q

Kb

A

Base ionization constant/Basicity Constant

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13
Q

TF:
↑ Kb ↑Basicity
↓ pkb ↑Basicity

A

True

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14
Q

pKa

A

pKa = -logka

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15
Q

pKb

A

pKb = -logkb

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16
Q

Formula for Strong Acids and Bases

A

pH = -log [H+]
pOH = -log [OH-]

pH + pOH = pKw
pKa + pKb = pKw

pKw = 14

17
Q

Formula for Weak acid and Weak Base

A

WA: pH = √ ka x ca
WB: pOH = √ kb x cb

18
Q

Solutions that resist pH change even if small amount og strong acid or strong base is added

19
Q

Primary buffer in Blood

A

Carbonic Acid-Bicarbonate Buffer System

20
Q

Acid Buffer

A

Weak acid + Conjugate Base

Ex. Acetic acid and Sodium citrate

21
Q

Basic Buffer

A

Weak Base + Conjugate Acid

Ex. Ammonia and Ammonium Chloride

22
Q

Buffer Equations

A

Henderson-Hasselbach Equation

23
Q

Calculate the pH of a buffer Solution

A

Henderson-Hasselbach Equation

24
Q

Henderson-Hasselbach Equation
Weak Acid

A

pH = pKa + log(salt/acid)
pH = (14 - pKb) + log (salt/acid)

25
Q

Henderson-Hasselbach Equation
Weak Base

A

pH = pKa + log (base/salt)

26
Q

The magnitude of resistance of a buffer to pH changes

A

Buffer Capacity/Effect/Index/Value/Efficiency

27
Q

Buffer Capacity Equation

A

Van Slyke’s

28
Q

Maximum Buffer Capacity formula

29
Q

Maximum Buffer Capacity

Physical Pharmacy (14 decks)

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