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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
Q

pH calculation of Strong Bases

A

pH = 14 + log (n_OH × [OH])

26
Q

pH calculation of Weak Acids

A

pH = -1/2 log (Ka × [A])

27
Q

pH calculation of Weak Bases

A

pH = 14 + 1/2 log (Kb × [B])

28
Q

strong acid + weak base

A

acidic salt

29
Q

strong base + weak acid

A

basic salt

30
Q

strong acid + strong base

A

neutral salt

31
Q

pH calculation of Acidic Salts

A

pH = 7 - 1/2 log ( Csalt / Kb )

32
Q

pH calculation of Basic Salts

A

pH = 7 + 1/2 log ( Csalt / Ka )

33
Q

solutions that contain weak acid/base and its conjugate salt; these tend to resist changes in pH

A

Buffer Solutions

34
Q

pH calculation of a Buffer Solution

A

Henderson-Hasslebalch Equation

pH = pKa - log [acid]/[base]

pH = 14 - pKb - log [acid]/[base]

35
Q

Primary Standards for Bases

A

Benzoic Acid, C6H5COOH
Oxalic Acid, H2C2O4•2H2O
Potassium Biiodate, KH(IO3)2
Potassium Hydrogen Phthalate (KHP), C6H4(COOH)(COOK)
Sulfamic Acid, HSO3NH2

36
Q

Primary Standards for Acids

A

CaCO3
HgO
Na2CO3
THAM, (CH2OH)3CNH2

37
Q

[Indicators for Acid-Base Titration]

Bromocresol Green
- pH transition range
- color change
- pKa

A

Bromocresol Green
- pH transition range: 3.8-5.4
- color change: yellow to blue
- pKa = 4.66

38
Q

[Indicators for Acid-Base Titration]

Methyl Red
- pH transition range
- color change
- pKa

A

Methyl Red
- pH transition range: 4.2-6.3
- color change: red to yellow
- pKa = 5

39
Q

[Indicators for Acid-Base Titration]

Bromothymol Blue
- pH transition range
- color change
- pKa

A

Bromothymol Blue
- pH transition range: 6.2-7.6
- color change: yellow to blue
- pKa = 7.1

40
Q

[Indicators for Acid-Base Titration]

Methyl Orange
- pH transition range
- color change
- pKa

A

Methyl Orange
- pH transition range: 3.1-4.4
- color change: orange to yellow
- pKa = 3.46

41
Q

[Indicators for Acid-Base Titration]

Phenolphthalein
- pH transition range
- color change
- pKa

A

Phenolphthalein
- pH transition range: 8.3-10
- color change: colorless to pink
- pKa = 9

42
Q

application of acid-base titration

for determination of organic nitrogen

A

Kjeldahl Method

43
Q

Kjeldahl Method Catalysts

A

K2SO4 - increases BP of H2SO4
HgO - increases rate of reaction
H2SeO3 - best catalyst

44
Q

formula for %protein in sample

A

%protein = %N × f

f = 5.7 (cereal)
f = 6.25 (meat)
f = 6.38 (dairy)

45
Q

precipitation titration is also called _____ titration since _____ is commonly employed in such technique

A

argentometric, AgNO3

46
Q

indicators in precipitimetry

A

Mohr Method
Volhard Method
Fajans Method

47
Q

Differentiate oxidation and reduction reactions

A

OIL RIG
Oxidation Is Loss of electrons / RA
Reduction Is Gain of electrons / OA

48
Q

Balancing Redox Reactions

A

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
Q

cathode, anode, reduction, oxidation

A

AN OX
anode is where oxidation occurs

RED CAT
reduction occurs in cathode

50
Q

electrochemical cell that stores electrical energy; reaction occurs spontaneously

A

galvanic/voltaic cell

51
Q

requires an external source of electrical energy to operate

A

electrolytic cell

52
Q

high positive reduction potential means…

A

good oxidizing agent

53
Q

thermodynamic potential of an electrochemical cell

A

Ecell = Ecathode - Eanode

54
Q

Nernst Equation

A

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
Q

describes absorption of radiant energy by matter

A

Beer’s Law

56
Q

Beer’s Law formula

A

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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