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Quality Control > M3-1 INTRODUCTION TO TITRIMETRIC ANALYSIS; NEUTRALIZATION TITRATIONS - PART 1 - > Flashcards

M3-1 INTRODUCTION TO TITRIMETRIC ANALYSIS; NEUTRALIZATION TITRATIONS - PART 1 - Flashcards

1
Q

(Volume and concentration)

A

Solution

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2
Q
  • amount
  • concentration
  • % purity
A

sample

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3
Q

method of determining the
quantity of a reagent of known concentration (STANDARD SOLUTION) that is required to react completely with the amount of active constituent is sample being analyzed (analyte)

A

Analytical method

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4
Q

known concentration

A

STANDARD SOLUTION

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5
Q

sample being analyzed

A

analyte

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5
Q

Acetic acid

A

VINEGAR

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6
Q
  • solution added from the buret
A

Titrant

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6
Q

sodium hydroxide

A

Base

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7
Q

Acetic acid
(Analyte or Standard Solution?)

A

ANALYTE

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7
Q

NaOH
(Analyte or Standard Solution?)

A

STANDARD SOLUTION

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8
Q

mass

A

ANALYTE

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9
Q

A process in which a standard reagent is added to a solution of analyte until the reaction is judged to be complete.

A

TITRATION

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9
Q

solution of known concentration

A
  • Standard solution
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10
Q

Sodium acetate

A

Salt

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11
Q

–substance in a sample being analyzed

A

Analyte

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11
Q
  • substance being titrated
A

Titrand

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12
Q

Analysis

A

ASSAY

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13
Q

Content/purity not yet determined

A

UNKNOWN

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14
Q

Neutralization (Acid-Base) Reaction

A

Acid + Base → Salt + Water

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14
Q

Known Concentration

A

KNOWN

15
Q

Indicator of Acetic acid in Vinegar sample

A

Phenolphthalein

16
Q

During ASSAY

The standard solution is considered
as the ___________; while the
analyte/sample as the __________

A

TITRANT - SS
TITRAND - Analyte

16
Q
  • Determine the analyte.
    1. Paracetamol in Biogesic tablet.
    2. Caffeine in Coffee powder
    3. Calcium ions in mineral water
A

Biogesic Tablet
Coffee powder
Mineral water

17
Q

When a physical change occurs that is associated with the condition of equivalence

A

End point

18
Q

When the amount of added titrant is chemically equivalent to the amount of analyte in the sample

A

Equivalence Point

19
Q
  • Acid base indicators are mostly complex organic molecules which are either weak acid or weak bases
  • Added to the analyte solution to give an [observable physical change.]
A

Indicators

20
Q

Acid → Low pH values; pH < 7
Neutral → pH = 7
Base/alkali → High pH values; pH > 7

A

Ph Values

21
Q

Low pH values; pH < 7

A

Acid

22
Q

pH = 7

A

Neutral

23
Q

High pH values; pH > 7

A

Base/alkali

24
Q

Rules for the Use of Indicators

  1. Two (2) drops
  2. SA (titrant) + SB (titrand) → MO, MR, PP
  3. SB (titrant) + WA (titrand) → PP
  4. SA (titrant) + WB (titrand) → MO
  5. WA (titrant) + WB (titrand) → N/A
  6. Appearance of color is preferred.
A

just be familiar

25
Q

Indicator of Sodium bicarbonate, NaHCO3

A

METHYL RED

26
Q

0.1N H2SO4

A

Acid

27
Q

NaHCO3

A

Base

28
Q

An ideal standard solution should be

A
  1. Stable
  2. Reacts rapidly
  3. Reacts completely
  4. Selective
29
Q

Used to establish the [concentration] of a solution by titrating it against a [primary standard.]

A

Standardization

30
Q

highly purified compound that serves a reference material

A

– Primary Standard

31
Q

Primary Standard

A
  1. High purity
  2. Stable
  3. Modest cost
  4. Soluble in medium
  5. High MW
32
Q

Sulfuric acid solution is considered a

A

SECONDARY STANDARD

33
Q

is a substance whose content/purity/concentration has been found by comparison against a primary standard

A

secondary standard

34
Q

Remember: H2SO4 was standardized using Na2CO3
(a primary standard).

A

n/a

35
Q
  • A highly pure substance
  • Dried solid
  • Ex. Sodium carbonate
A

PRIMARY STANDARD

36
Q
  • Usually, a solution with known concentration
  • Standard Solution (liquid)
  • Ex. Sulfuric acid solution
A

SECONDARY STANDARD

37
Q

– It is defined as the number of equivalents of solute per liter of solution.
– Or milliequivalents per milliliter (mEq/mL)
𝑵 = 𝑬𝒒/𝑳
𝒐𝒓 𝒎𝑬𝒒/𝒎𝑳

A

Normality (N)

38
Q

– It is defined as the number of moles of solute per liter of solution.
– Or millimoles per milliliter (mmol/mL)

𝑴 = 𝒎𝒐𝒍/𝑳
𝒐𝒓 𝒎𝒎𝒐𝒍/𝒎𝑳

A

Molarity (M)

39
Q

𝒎𝑬𝒒 𝒘𝒕 =
𝑴𝑾/𝒇𝒆𝒒 𝒙 𝟏𝟎𝟎0

𝑬𝒒𝒖𝒊𝒗𝒂𝒍𝒆𝒏𝒄𝒆 𝑭𝒂𝒄𝒕𝒐𝒓 = 𝒇𝒆𝒒 = 𝒗𝒂𝒍𝒆𝒏𝒄𝒆

– For neutralization reactions, feq represents the number of reacting H+ or OH- ions

A

Milliequivalent Weight (mEq wt)

40
Q

Equivalence Factor (feq)

A
  • For acids:
    feq = no. of reactive H+
    – HCl
  • feq = 1
    – H2
    SO4
  • feq = 2
  • For bases:
    feq = no. of reactive OH-
    – Mg(OH)2
  • feq = 2
    – NaOH
  • feq = 1
41
Q

Types of Analysis based on Reaction

A
  1. Neutralization
    a) Acidimetry
    b) Alkalimetry
  2. Precipitation
  3. Redox
  4. Complexation

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