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

Question 1

(Volume and concentration)

Answer 1

Solution

Question 2

• amount
• concentration
• % purity

Answer 2

sample

Question 3

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)

Answer 3

Analytical method

Question 4

known concentration

Answer 4

STANDARD SOLUTION

Question 5

sample being analyzed

Answer 5

analyte

Question 5

Acetic acid

Answer 5

VINEGAR

Question 6

• solution added from the buret

Answer 6

Titrant

Question 6

sodium hydroxide

Answer 6

Base

Question 7

Acetic acid
(Analyte or Standard Solution?)

Answer 7

ANALYTE

Question 7

NaOH
(Analyte or Standard Solution?)

Answer 7

STANDARD SOLUTION

Question 8

mass

Answer 8

ANALYTE

Question 9

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

Answer 9

TITRATION

Question 9

solution of known concentration

Answer 9

• Standard solution

Question 10

Sodium acetate

Answer 10

Salt

Question 11

–substance in a sample being analyzed

Answer 11

Analyte

Question 11

• substance being titrated

Answer 11

Titrand

Question 12

Analysis

Answer 12

ASSAY

Question 13

Content/purity not yet determined

Answer 13

UNKNOWN

Question 14

Neutralization (Acid-Base) Reaction

Answer 14

Acid + Base → Salt + Water

Question 14

Known Concentration

Answer 14

KNOWN

Question 15

Indicator of Acetic acid in Vinegar sample

Answer 15

Phenolphthalein

Question 16

During ASSAY

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

Answer 16

TITRANT - SS
TITRAND - Analyte

Question 16

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

Answer 16

Biogesic Tablet
Coffee powder
Mineral water

Question 17

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

Answer 17

End point

Question 18

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

Answer 18

Equivalence Point

Question 19

* 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.]

Answer 19

Indicators

Question 20

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

Answer 20

Ph Values

Question 21

Low pH values; pH < 7

Answer 21

Acid

Question 22

pH = 7

Answer 22

Neutral

Question 23

High pH values; pH > 7

Answer 23

Base/alkali

Question 24

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.

Answer 24

just be familiar

Question 25

Indicator of Sodium bicarbonate, NaHCO3

Answer 25

METHYL RED

Question 26

0.1N H2SO4

Answer 26

Acid

Question 27

NaHCO3

Answer 27

Base

Question 28

An ideal standard solution should be

Answer 28

1. Stable 2. Reacts rapidly 3. Reacts completely 4. Selective

Question 29

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

Answer 29

Standardization

Question 30

highly purified compound that serves a reference material

Answer 30

– Primary Standard

Question 31

Primary Standard

Answer 31

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

Question 32

Sulfuric acid solution is considered a

Answer 32

SECONDARY STANDARD

Question 33

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

Answer 33

secondary standard

Question 34

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

Answer 34

n/a

Question 35

- A highly pure substance - Dried solid - Ex. Sodium carbonate

Answer 35

PRIMARY STANDARD

Question 36

- Usually, a solution with known concentration - Standard Solution (liquid) - Ex. Sulfuric acid solution

Answer 36

SECONDARY STANDARD

Question 37

– 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

Answer 37

Normality (N)

Question 38

– 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

Answer 38

Molarity (M)

Question 39

𝒎𝑬𝒒 𝒘𝒕 = 𝑴𝑾/𝒇𝒆𝒒 𝒙 𝟏𝟎𝟎0 𝑬𝒒𝒖𝒊𝒗𝒂𝒍𝒆𝒏𝒄𝒆 𝑭𝒂𝒄𝒕𝒐𝒓 = 𝒇𝒆𝒒 = 𝒗𝒂𝒍𝒆𝒏𝒄𝒆 – For neutralization reactions, feq represents the number of reacting H+ or OH- ions

Answer 39

Milliequivalent Weight (mEq wt)

Question 40

Equivalence Factor (feq)

Answer 40

* 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

Question 41

Types of Analysis based on Reaction

Answer 41

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