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Day 1: Physical and Chemical Principles > Analytical Chemistry > Flashcards

Analytical Chemistry Flashcards

1
Q

Methods of Analyses

A

Classical Methods
1. Gravimetric Method
2. Volumetric Method

Modern Methods
1. Spectroscopic Method
2. Electroanalytic Method

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2
Q

deals with measurement of the mass of a substance that is chemically related to the analyte

A

Gravimetric Method

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3
Q

measures the volume of solution necessary to react completely with the analyte

A

Volumetric Method

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4
Q

measures the electromagnetic radiation produced by the analyte or its interactions with it

A

Spectroscopic Method

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5
Q

measures the electrical properties of the analyte such as current (A), potential (V), resistance (Ω), and amount of charge (coul)

A

Electroanalytic Method

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6
Q

Steps on Gravimetric Method

A

Gravimetric Factor = (MW of analyte / MW of ppt) × (x analyte / y ppt)

%analyte = (m_ppt × GF) / m_sample × 100

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7
Q

[Volumetric Method of Analysis]

solution of known concentration

A

Standard Solution

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8
Q

[Volumetric Method of Analysis]

process of determining the concentration of an unknown solution

A

Standardization

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9
Q

[Volumetric Method of Analysis]

a substance of high purity used for standardization

A

Primary Standard

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10
Q

[Volumetric Method of Analysis]

Characteristics of Good Primary Standard

A
  1. high purity and eq. wt.
  2. stable towards air, high T, humidity
  3. soluble in water
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11
Q

type of titration

the analyte reacts with the standard solution directly

A

Direct Titration

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12
Q

type of titration

an excess standard solution is added and the excess is determined by the addition of another standard solution

A

Back Titration

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13
Q

type of titration.
the analyte is converted to a product chemically related to it and the product of such reaction is titrated with a standard solution

A

Replacement Titration

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14
Q

type of titration

A

the analyte is converted to a product chemically related to it and the product of such reaction is titrated with a standard solution

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15
Q

Lewis Acid and Base

A

Lewis Acid = electron-pair acceptor
Lewis Base = electron-pair donor

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16
Q

Bronsted-Lowry Acid and Base

A

Bronsted-Lowry Acid = proton donor
Bronsted-Lowry Base = proton acceptor

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17
Q

Arrhenius Acid and Base

A

Arrhenius Acid = produces H+ in soln
Arrhenius Base = produces OH- in soln

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18
Q

reaction involving formation of ions

A

Ionization Reaction

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19
Q

Strong Acids (completely ionized in solution)

A

HI, HCl, HBr
HNO3, HClO4, H2SO4 (1st ion)

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20
Q

Strong Bases (completely ionized in solution)

A

Group 1A and 2A bases

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21
Q

Weak Acids (partially ionized in solution)

A

HF, HCN
H2SO3, H3PO4, organic acids

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22
Q

Weak Bases (partially ionized in solution)

A

ammonia and derivatives

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23
Q

Autoprotolysis of Water

A

H2O + H2O ↔️ H3O+ + OH-

Kw = 1×10-¹⁴ at 25°C

24
Q

pH calculation of Strong Acids

A

pH = -log [A]

25
pH calculation of Strong Bases
pH = 14 + log (n_OH × [OH])
26
pH calculation of Weak Acids
pH = -1/2 log (Ka × [A])
27
pH calculation of Weak Bases
pH = 14 + 1/2 log (Kb × [B])
28
strong acid + weak base
acidic salt
29
strong base + weak acid
basic salt
30
strong acid + strong base
neutral salt
31
pH calculation of Acidic Salts
pH = 7 - 1/2 log ( Csalt / Kb )
32
pH calculation of Basic Salts
pH = 7 + 1/2 log ( Csalt / Ka )
33
solutions that contain weak acid/base and its conjugate salt; these tend to resist changes in pH
Buffer Solutions
34
pH calculation of a Buffer Solution
Henderson-Hasslebalch Equation pH = pKa - log [acid]/[base] pH = 14 - pKb - log [acid]/[base]
35
Primary Standards for Bases
Benzoic Acid, C6H5COOH Oxalic Acid, H2C2O4•2H2O Potassium Biiodate, KH(IO3)2 Potassium Hydrogen Phthalate (KHP), C6H4(COOH)(COOK) Sulfamic Acid, HSO3NH2
36
Primary Standards for Acids
CaCO3 HgO Na2CO3 THAM, (CH2OH)3CNH2
37
[Indicators for Acid-Base Titration] Bromocresol Green - pH transition range - color change - pKa
Bromocresol Green - pH transition range: 3.8-5.4 - color change: yellow to blue - pKa = 4.66
38
[Indicators for Acid-Base Titration] Methyl Red - pH transition range - color change - pKa
Methyl Red - pH transition range: 4.2-6.3 - color change: red to yellow - pKa = 5
39
[Indicators for Acid-Base Titration] Bromothymol Blue - pH transition range - color change - pKa
Bromothymol Blue - pH transition range: 6.2-7.6 - color change: yellow to blue - pKa = 7.1
40
[Indicators for Acid-Base Titration] Methyl Orange - pH transition range - color change - pKa
Methyl Orange - pH transition range: 3.1-4.4 - color change: orange to yellow - pKa = 3.46
41
[Indicators for Acid-Base Titration] Phenolphthalein - pH transition range - color change - pKa
Phenolphthalein - pH transition range: 8.3-10 - color change: colorless to pink - pKa = 9
42
application of acid-base titration for determination of organic nitrogen
Kjeldahl Method
43
Kjeldahl Method Catalysts
K2SO4 - increases BP of H2SO4 HgO - increases rate of reaction H2SeO3 - best catalyst
44
formula for %protein in sample
%protein = %N × f f = 5.7 (cereal) f = 6.25 (meat) f = 6.38 (dairy)
45
precipitation titration is also called _____ titration since _____ is commonly employed in such technique
argentometric, AgNO3
46
indicators in precipitimetry
Mohr Method Volhard Method Fajans Method
47
Differentiate oxidation and reduction reactions
OIL RIG Oxidation Is Loss of electrons / RA Reduction Is Gain of electrons / OA
48
Balancing Redox Reactions
Write half cell reactions Determine no. of electrons based on oxidation state Balance by adding H2O to O-deficient side and H/OH on other side
49
cathode, anode, reduction, oxidation
AN OX anode is where oxidation occurs RED CAT reduction occurs in cathode
50
electrochemical cell that stores electrical energy; reaction occurs spontaneously
galvanic/voltaic cell
51
requires an external source of electrical energy to operate
electrolytic cell
52
high positive reduction potential means...
good oxidizing agent
53
thermodynamic potential of an electrochemical cell
Ecell = Ecathode - Eanode
54
Nernst Equation
E = E° - (RT/nF) ln [C]^c[D]^d / [A]^a[B]^b at 25°C: E = E° - (0.0592/n) ln [C]^c[D]^d / [A]^a[B]^b R = 8.314 J/mol-K T [=] K F = 96500 coul/mol e- n = no. of e- in half cell reaction
55
describes absorption of radiant energy by matter
Beer's Law
56
Beer's Law formula
A = εbc = log Po/P = log 1/T T = transmittance A = absorbance P = emergent radiation Po = entering radiation ε = molar absorptivity b = thickness c = concentration

Day 1: Physical and Chemical Principles (2 decks)

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