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PHAN 1 LEC > VOLUMETRIC ANALYSIS > Flashcards

VOLUMETRIC ANALYSIS Flashcards

1
Q

the determination of the
volume of a solution of
known concentration
required to react with a
given amount of a
substance to be analyzed.

A

Volumetric
Analysis

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2
Q

What is the importance of
volumetric analysis?

A

It is used in
determining the
purity of drugs

Food industry –
determination of
salt, vit and fatty
acid content.

Water treatment
– determination
of contaminants
and pH

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3
Q

a common laboratory method of quantitative chemical
analysis where a solution of known concentration is used
to determine the concentration of an unknown solution.

A

TITRATION

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4
Q

Parts of a titration set-up

A
  1. Analyte/Titrand
  2. Standard solution/ Volumetric Solution/ Titrant
  3. Indicator
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5
Q

a solution which
concentration is
accurately known.

A

Standard solution

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6
Q

the
chemical substance
being analyzed or the
active constituent in
the sample.

A

Analyte

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7
Q

a chemical
which changes
color at or very
near the endpoint.

A

Indicator

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8
Q
A
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9
Q

point during a titration when an indicator shows that
the amount of reactant necessary for a complete
reaction has been added to a solution

A

Endpoint (practical

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9
Q

s the theoretical point at which equivalent amounts
of each substance have reacted

A

Equivalence point or stoichiometric point or
theoretical endpoint

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9
Q

reaction between an acid and
a base to form salt of water

A

Neutralization

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10
Q

reactions that from an
insoluble precipitate

A

Precipitimetry

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11
Q

reaction between metal ions
and a ligand

A

Complexometry

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12
Q

reaction that involves the
transfer of electrons

A

Redox titration

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13
Q

Chemical substance, which changes color at or
very near the endpoint.

A

INDICATORS

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14
Q

Used to avoid errors during titration

A

INDICATORS

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15
Q

INDICATORS Referred to as

A

TS or Test Solutions

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16
Q

TS or Test Solutions Usual concentration is

A

0.05%, with 0.1 to 0.2 ml
of indicator used for 10 ml of the analyte

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17
Q

pH range; Acid; Base
Malachite green

A

0 – 2.0; Yellow; Green

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18
Q

pH range; Acid; Base
Methyl orange

A

3.2 -4.4 Pink Yellow

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19
Q

pH range; Acid; Base
Methyl red

A

4.2 – 6.2 Red Yellow

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20
Q

pH range; Acid; Base
Bromothymol
blue

A

6.0 – 7.6 Yellow Blue

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21
Q

pH range; Acid; Base
Phenolphthalein

A

8 - 10 Colorless Pink or red

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22
Q

pH range; Acid; Base
Thymol blue

A

8 – 9.2 yellow blue

23
Q

Weak Acid Strong Base INDICATOR

A

Phenolphthalein

24
Q

Weak Base Strong Acid INDICATOR

A

Methyl red

25
Q

Strong Acid Strong Base INDICATOR

A

Phenolphthalein,
Methyl Orange,
Methyl Red

26
Q

Weak Base Weak Acid INDICATOR

A

NONE – No
endpoint

27
Q

PRECIPITATION INDICATORS

A
  • Dichlorofluororesc ein
  • Eosin Y
  • Potassium Chromate
  • FAS
28
Q

COMPLEXATION INDICATORS

A
  • Dithizone
  • Eriochrome Black
  • Hydroxynaphtol Blue
29
Q

REDOX INDICATORS

A
  • Iodine TS
  • Potassium
    Permangana
    te VS
  • Starch TS
30
Q

number of
moles of reactive unit
in a compound which
reacts or takes the
place of one mole of
Hydrogen ion

A

Equivalent

31
Q

Equivalent of salts

A

Valence of cation

32
Q

weight that is
chemically equivalent
to the reacting power
of one of one atomic
weight of hydrogen.

A

Equivalent weight

33
Q

called milliequivalent
weight

A

1/1000 of Eq. weight

34
Q

strength in grams equivalent to milliliter of
standard solution or the weight of a substance
chemically equivalent to 1 ml of a standard
solution.

A

TITER

35
Q

no. of equivalents of solute per liter

A

NORMALITY

36
Q

1N

A

NORMAL SOLUTION

37
Q

2N

A

DOUBLE NORMAL

38
Q

0.5N

A

HALF NORMAL

39
Q

TENTH NORMAL

A

0.1N

40
Q

TWENTIETH NORMAL

A

0.05N

41
Q

HUNDREDTH NORMAL

A

0.01N

42
Q

THOUSANDTH NORMAL

A

0.001N

43
Q

refers to the no. of moles of solute per liter of solution

A

MOLARITY

44
Q

refers to the no. of moles of solute per kilogram of solvent

A

MOLALITY

45
Q

a solution of known concentration or a solution
whose exact concentration is known

A

STANDARD SOLUTION

46
Q

Standard acid solution

A

HCl, H 2SO 4, HClO

47
Q

Standard alkali solution

A

NaOH, KOH,
CH 3ONa

48
Q

Process of determining exact concentration of a
solution.

A

STANDARDIZATION

49
Q

Types of volumetric solution:

A
  1. Primary Standard 2. Secondary Standard
50
Q

chemically pure solid substance almost 99.9%
pure used in the standardization of a solution

A

Primary Standard

51
Q

Other requirements for primary standard are:

A
  1. It must be easy to prepare and pure.
  2. It must be of definite known composition.
  3. It must be stable.
  4. It must react stoichiometrically with the substance
    present in the solution.
  5. It must be soluble in water.
  6. it must have a fairly high equivalent weight.
52
Q

Primary Standard for acid solutions:

A

Anhydrous
Na2 CO 3

CaCO 3

THAM

53
Q

Primary Standard for alkali solutions:

A

Benzoic acid

Potassium
biphthalate

Sulfamic acid

54
Q

substance that is not
necessarily pure but whose exact purity is
known.

A

Secondary Standard

55
Q

A standard solution is a commonly used

A

secondary standard

56
Q

to standardize only one of
the solutions by using a primary standard and
the other is standardized by using a
secondary standard

A

Common practice

57
Q

Titrate with HCl
until a _________ is
achieved even after
boiling the solution.

A

permanent
faint pink color

PHAN 1 LEC (13 decks)

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