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

Analytical Chemistry Flashcards

1
Q

It is a branch of chemistry involved with the analysis of a chemical substance.

A

Analytical Chemistry

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2
Q

It establishes the chemical identity of the species in a sample.

A

Qualitative Analysis

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3
Q

It determines the relative amounts of these species, or analytes, in numerical terms.

A

Quantitative Analysis

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4
Q

Determination of mass of the analyte or some compound chemically related to it.

A

Gravimetric Methods

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5
Q

Measurement of the volume of a solution containing sufficient reagent to react completely with the analyte.

A

Volumetric Methods

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6
Q

Measurement of electrical properties (potential, current, resistance, quantity of electric charge, etc.), emission of radiation by analytes, etc.

A

Instrumental Methods

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7
Q

A general expression for an amount of solute in a given amount of material.

A

Concentration

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8
Q

Molarity (M)

A

amount of solute (mol) / volume of solution (L)

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9
Q

molality (m)

A

amount of solute (mol) / mass of solvent (kg)

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10
Q

Allows for simplified calculations involved with certain types of problems

A

Normality

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11
Q

Based on measuring the amount of a substance required to react with an analyte completely.

A

Normality

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12
Q

The reaction ratio still must be taken into account, but it is done by combining it with the molarity to produce a new unit of concentration called

A

“normal”

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13
Q

Normality (N)

A

amount of solute (eq) / volume solution (L)

Normality = Molarity × h

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14
Q

h = number of electrons lost or gained in the reaction

A

Redox Reactions

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15
Q

h = number of participating H+ or OH− ions

A

Neutralization Reactions

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16
Q

Water, as an amphiprotic solvent, undergoes

A

self-ionization or autoprotolysis

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17
Q

Strong acids and bases ionize completely in

A

water

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18
Q

Weak acids and bases ionize only partially in

A

water

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19
Q

extent of ionization depends on the dissociation constants, which are

A

equilibrium constants

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20
Q

Mixtures of weak acids or bases and their conjugate.

A

pH Buffers

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21
Q

Have the ability to resist changes in pH upon dilution or addition of small amounts of acid or base.

A

pH Buffers

22
Q

Henderson-Hasselbalch Equation:

A

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

23
Q

the quantity of strong acid or strong base needed to cause 1L of the buffer to undergo a pH change of 1.

A

Buffer capacity

24
Q

The buffer capacity increases as the concentration ratio approaches

A

1

25
Q

A solution is basic if:

A

[OH-] > [H+]

26
Q

Water at room temperature usually has a slightly acidic pH. This is largely attributed to what compound(s)?

A

Carbonic Acid

27
Q

When benzoic acid dissolves in water, it partially reacts with water and ionizes to form benzoate and hydronium ions. In this reaction, what is the conjugate acid?

A

Hydronium Ions

28
Q

Define a salt in terms of acid and base.

A

A salt is a compound (other than water) produced by the reaction of an acid and a base.

29
Q

When a can of soda is opened and CO2 is released to the atmosphere, what is the resultant pH of the soda?

A

Increases

30
Q

Which of the following pairs will form a buffer solution in the course of a titration?

A

Acetic acid, sodium hydroxide

31
Q

Buffer capacity is maximum when:

A

pH = pKa

32
Q

Which of the following acids would be most suitable for preparing a buffer of pH 3.1?

A

Sulfanilic acid, pKa = 3.232

33
Q

Determination of nitrogen based on the conversion of organic nitrogen to ammonia, which is then separated by distillation and determined by titration.

A

Kjeldahl Method

34
Q

Bases that can be titrated with a strong acid such as HCl.

A

Carbonate, bicarbonate, and hydroxide ions

35
Q

There are 5 possible sample compositions:

A

Na2CO3 alone, NaOH alone, NaHCO3 alone,
Na2CO3+NaOH, and Na2CO3+NaHCO3.

36
Q

Titrations based on reactions that produce sparingly soluble substances (precipitates).

A

Precipitation Titrations

37
Q

Among the oldest titrations known, but are limited in scope because it is sometimes non-stoichiometric, has a slow reaction rate, and has issues of co-precipitation.

A

Precipitation Titrations

38
Q

Only procedures using silver ion (Ag+, argentometric titrations) as the titrant or analyte have remained competitive with newer analytical methods.

A

Precipitation Titrations

39
Q

Analyte: Cl-, Br-, CN-
Titrant: AgNO3 (Ag+)
Indicator: Na2CrO4
Titration reaction: Ag+ + Cl− ↔ AgCl (s)
Indicator reaction: 2Ag+ + CrO2− ↔ Ag2CrO4 (s)
Carried out at 6.5<pH<10.3 to prevent formation of a soluble complex (pH<6.5) or an unwanted insoluble hydroxide or oxide (pH>10.3).

A

Mohr Method

40
Q

Analyte: Cl-, Br-, I-, SCN-
Titrant: AgNO3 (Ag+)
Indicator: Dichlorofluorescein (Cl-, Br-, I-, SCN-), eosin (Br-, I-, SCN-)
Titration reaction: Ag+ + Cl− ↔ AgCl(s)
Indicator reaction: AgCl ∙ Ag+ + DCF− ↔ AgCl ∙ Ag+ ∙ DCF−(s)
Done with vigorous shaking to avoid coagulation.
Addition of dextrin inhibits undesired coagulation of the AgCl.

A

Fajans Method

41
Q

Analyte: Cl-, Br-, I-
Titrant: SCN-
Indicator: FeSCN2+ (comes from ferric alum)
Analyte reaction: Ag+ + Cl− ↔ AgCl(s)
Titration reaction: Ag+ + SCN− ↔ AgSCN(s)
Indicator reaction: Fe3+ + SCN− ↔ FeSCN2+(s)
Nitrobenzene may be added to mask AgCl from reacting with SCN-

A

Volhard Method

42
Q

bonds where both bonding electrons come from one of the two atoms involved.

A

coordinate covalent bonds

43
Q

the molecule or ion containing the donor atom.

A

Ligand or coordinating agent

44
Q

the product resulting from the reaction between a metal ion and a ligand

A

Coordination compound or complex ion

45
Q

the number of pairs of electrons accepted by a particular metal ion (at least 4, often 6)

A

Coordination number

46
Q

can be classified according to how many donor atoms it contains (dentate)

A

Ligands

47
Q

When polydentate ligands coordinate with metal ions, ring structures known as ______ are formed.

A

chelates

48
Q

A hexadentate, containing 4 oxygen and 2 nitrogen donor atoms.

A

Ethylenediaminetetraacetic Acid (EDTA)

49
Q

EDTA

A

Ethylenediaminetetraacetic Acid

50
Q

can exist in a variety of protonated forms

A

tetraprotic acid

51
Q

Any or all of its protonated forms may react with a given metal to yield a metal

A

EDTA complex

52
Q

Theory of Complexation Indicators

A

M + In ↔ MIn

MIn + Y ↔ MY + In

Day 1 - Physical and Chemical Principles (3 decks)

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