2. Titrimetric methods
as an analytical method in which the volume of a
solution of known concentration consumed during an
analysis is taken as a measure of the amount of active
constituent in a sample analyzed
3. Analyte – or the active constituent in the sample
Titrant – solution of known concentration
Indicator – chemical which changes color at a point
equivalent quantities of analyte and titrant have
reacted
4. Stoichiometric point or Equivalence point – the
theoretical point at which equivalent amounts of each
have reacted
Endpoint – a sudden change apparent by use of
indicators
5. Standardization – determination of the exact
concentration of the solution
Standardized using 2 types of standards:
Primary standard – subs of known and high
degree of purity; used in direct standardization
Secondary standard – std. soln used in indirect
standardization
- std solution of known conc usually
standardized by primary std.
6. Requirements for Primary Standard:
1. High purity = 99.9%
2. Definite and known composition
3. Not affected by drying
4. Soluble in water
8. Example: standardization of HCL
Standardize titrimetrically using sodium carbonate of
known purity as a primary standard or
using standard NaOH as a secondary standard
16. Types of Titration:
DIRECT TITRATION – one titrant used, one volumetric
solution
RESIDUAL TITRATION – two titrants, two volumetric
solutions
1st VS – is added in excess
2nd VS – used to titrate the excess
17. Residual Titration - is used whenever the direct
titration is not practicable
- for compounds which react too slowly
with titrant
- poor solubility
- volatile substances are involved
Blank Determination – process of repeating the
procedure but omitting the sample
27. 1. Find the molarity of HCl soln. which contains the
volume of 2400 mL and also it contains 230 g of
HCl. MW of HCl=36.46
2. Find the normality of 20 g NaOH diluted to a volume
of 1L. MW of NaOH= 40
28. 3. Compute for normality of HCl that make use of a
primary standard (Na2CO3) that weighs 1.5 g. It
consumed 30 mL of HCl after titration. MW of
Na2CO3 = 106
4. Compute for normality of HCl using secondary
standard (NaOH) having a concentration of 2 N. It
consumed 35 mL of NaOH. The volume sample used
was 25 mL.
29. 5. A soln. with a final volume of 500 mL was prepared by
dissolving 25mL of methanol (density= 0.7914) in
chloroform. Calculate the molarity of methanol in the
soln. MW = 32
6. Calculate the normality of a NaCl soln. prepared by
dissolving 2.5 g of NaCl in water and then tapping it
off with more water to a total volume of 500 mL. MW
of NaCl= 58.44 g/mole
30. 7. What mass of oxalic acid, H2C2O4, is required to
make 250 mL of 0.05M soln.(MW=90)
8. Sulfamic acid is a primary standard that can be used
to standardize NaOH. What is the molarity if 34.26 mL
reacts with 0.3337 g of sulfamic acid. MW= 97
31. 9. What is the normality of H2SO4 containing 73.5 g/
500 mL of solution? MW of H2SO4= 98 g/mole
32. 10. The molecular wt. of NaOH is 40. How many grams
of NaOH pellets are needed to make 500 mL of 1.5 N
soln?
33. 11. Convert the following concentration as required:
0.5 M KOH to N
0.025 M H2SO4 to N
2 N NaCl to M
35. Standardization
determination of normality or molarity of solution
accomplished by the use of another standard solution
known as a SECONDARY STANDARD or by the use of
known purity substance as PRIMARY STANDARD
36. The wt. of substance chemically equivalent to 1 mL of
std. soln.
Express in mg/ mL
To get titer value:
N x meq wt.
1 meq X 60 g x 1000 mg
mL 1000 meq 1 g
= 60 mg/mL
37. Ex.
1. What would the titer value be of the soln. in terms of
CaCl2 of 0.05 N soln.? MW = 111
2. Compute for percent purity of 0.1 g sodium ascorbate
if the titer value is 9.905 mg/mL. It consumed 10 mL
thru direct titration with iodine.
39. Burets
Graduated glass tubes of uniform bore throughout the
whole length
Closed at the bottom by glass or stopcock
Volumes read at lower meniscus except highly colored
liquid
41. CHEMICAL REACTIONS USED IN TITRIMETRY
1. Neutralization (acid-base)
2. precipitation
3. complexation
4. redox
42. NEUTRALIZATION REACTION
a chemical process in which an acid (proton donor)
reacts with a base (proton acceptor)
the products are : water and salt
46. Commonly used pH indicators
Color Change
Indicator pH Range Acid Base
Malachite green 0.0 – 2.0 yellow green
Methyl Yellow 2.9 – 4.0 red yellow
Bromophenol blue 3.0 - 4.6 yellow blue
Methyl Orange 3.2 – 4.4pink yellow
Bromocresol green 4.0 -5.4 yellow blue
47. Methyl red 4.2 – 6.2 red yellow
Bromocresol purple 5.2 – 6.8 yellow purple
Bromothymol blue 6.0 – 7.6 yellow blue
Phenol red 6.8 – 8.2 yellow red
Cresol red 7.2 – 8.8 yellow red
Thymol blue 8.0 – 9.2 yellow blue
Phenolphthalein 8.0 – 10.0 colorless red
Thymolphthalein 9.3 – 10.5 colorless blue
48. Indicators:
Aqueous :
Phenolphthalein
Methyl orange
Methyl red
Strong Acid + Strong Base : php, MO, MR
Weak Acid + Strong base : php
Weak base + strong acid : MR
51. Standard Acid Solutions used in Acidimetry and
Alkalimetry
1. HCl – more preferable to sulfuric in the titration of
compounds that yield precipitate
2, Sulfuric Acid – preferable in hot titrations since HCl
will volatilize