5. Contoh
titrasi
Analit Titran Indikator
Asam-basa Kadar asam
asetat dalam
minuman
Asam asetat
(CH3COOH)
NaOH (sodium
hydroxide)
Phenolphthalein
kompleksometri Mengukur
kesadahan air
(kalsium &
magnesium)
Kalsium dan
magnesium (Ca
2+
, Mg 2+
)
EDTA Eriochrome black
T
Murexide
Pengendapan Penentuan kadar
klorin dlm air
klorin AgNO3 (silver
nitrate)
Mohr, Volhard,
Fajans
Redox Penentuan kadar
hidrogen
peroksida (H2O2)
Hidrogen
peroksida (H2O2)
KMnO4
(potassium
permanganate)
Tanpa indikator
6. Redox Titrations
Titrasi Redoks
Berdasarkan pada reaksi reduksi-oksidasi antara analit dan titran
Banyak senyawa kimia, biologi, lingkungan, dan lainnya dapat ditentukan kadarnay
dengan titrasi redoks
Biochemistry 2005, 44, 1856-1863
Measurement of redox
potentials permit detailed
analysis of complex
enzyme mechanism
Electron path in multi-heme active site of P460
7. Redox Titrations
terjadi perubahan voltase seiring dengan penambahan titran
Contoh reaksi pada titrasi redoks berikut (reaksi berjalan sempurna):
Ce4+
ditambahkan dari buret pada larutan Fe2+
Elektroda Pt merespon perubahan konsentrasi dari:
Fe3+
/Fe2+
& Ce4+
/Ce3+
Elektroda Kalomel digunakan sebagai referensi
Eo
= 0.767 V
K ≈ 1016
Eo
= 1.70 V
8. Ada beberapa jenis titrasi redoks yang diklasifikasikan
berdasarkan titran yang digunakan.
1) Permanganometri: Titran KMnO4
2) Dikromatometric Titran K2Cr2O7
3) Titrasi melibatkan iodine (I2)
•Iodimetri
•Iodometri
Titrasi yang menggunkaan I2 termasuk jenis titrasi
yang sering digunakan.
9. Pereduksi adalah senyawa yang dalam reaksi redoks
mereduksi senyawa lain, dengan kata lain bertindak sebagai
oksidator, dan sebagai donor elektron dalam reaksi redoks.
Contoh senyawa pereduksi:
Logam natrium, magnesium, aluminium, dan zink
NaH, CaH2, dan LiAlH4, senyawa yang mengandung ion H-
.
10. Oksidator adalah senyawa yang dalam reaksi redoks
mengoksidasi senyawa lain, dengan kata lain
bertindak sebagai reduktor dan sebagai penangkap
elektron.
Contoh :
permanganat (MnO4
-
), chromat (CrO4
2-
), dan dichromat
(Cr2O7
2-
), natrium hipoklorit (bleach), asam nitrat (HNO3),
asam perklorat (HClO4), dan asam sulfat (H2SO4)
11. Titrasi dengan permanganat
Kalium Permanganat (KMnO4)
- Oksidator kuat
- Auto indikator
Titration of VO2+
with KMnO4
Before Near After
Equivalence point
Eo
= 1.507 V
Violet colorless
pH ≤ 1
Eo
= 1.692 V
pH neutral or alkaline
Violet brown
pH strolngly alkaline
Eo
= 0.56 V
Violet green
12. Titrasi iodimetri
Iodimetri: titrasi langsung dengan satu tahap reaksi :
Analit + titran (iodine I2
) produk (iodide I→ -
)
Tdk diketahui diketahui
Bila titrasi dilakukan dengan titran iodin maka disebut titrasi
iodimetri
13. Titrasi iodimetri
Contoh : penetapan kadar asam askorbat (Vitamin C)
C6H8O6 + I2 → CçH6O6 + 2I-
+ 2H+
Iodin mengoksidasi dengan cepat asam askorbat C6H8O6 , dan
menghaslkan asam dehidroaskorbat, C6H6O6 .
Asam askorbat asam dehidroaskorbat
Pictures taken from: http://en.wikipedia.org
14. Titrasi iodometri
Iodometri adalah titrasi terhadap iodin (I2) yang dihasilkan dari
oksidasi analit terhadap I-
yang ditambahkan.
Kemudian iodin (I2) biasanya dititrasi dengan larutan standar
tiosulfat.
Iodometri: bukan titrasi langsung karena tejadi 2 reaksi:
analit + I-
→ I2
Tdk diketahui
I2
+ titran (standar tiosulfat) produk→
diketahui
15. Titrasi iodometri
Contoh : penetapan kadar tembaga
Analit dgn
konsentrasi
tdk diketahui
Titran
-larutan standar : natrium
tiosulfat
-konsentrasi diketahui
2 Cu 2+
+ 4I-
→ 2CuI + I2
I2
+ 2S2
O3
2-
→ 2I-
+ S4
O6
2-
16. Titrasi Iodimetri:
a) Reduksi analit
b) Satu reaksi
c) Larutan standar: Iodin (I2)
Titrasi Iodometri:
a) Oksidasi analit
b) Dua reaksi
c) Larutan standar: natrium tiosulfat
17. Aplikasi analisis:
titrasi Iodimetri:
senyawa yang dianalisis
SO2
H2S
Zn2+
, Cd2+
, Hg2+
, Pb2+
Cisteine, glutathione, mercaptoethanol
Glucose (dan gula-gula pereduksi lain)
Section of a protein structure
Source: http://en.wikipedia.org
Slide 2:
Titrations are one of the two types of Classical Quantitative Analysis.
What is the other classical quantitative analysis?
Exactly, the other classical quantitative chemical analysis is gravimetry.
You will see gravimetry in other parts of the course.
Let’s continue by asking about titrations.
What are the four types of titrations?
Yes, remember the four types are:
Firstly, acid-base titrations, secondly complexometric titrations, thirdly precipitation titrations and fourthly redox titrations.
Remember that we started working with acid-base titrations, then we moved on to complexometric titrations and finally we saw precipitation titrations.
Today we will be looking at iodometric and iodimetric titrations, which are examples of redox titrations.
We have left redox titrations until now, because you needed to be familiar with the other three type of titrations.
So, let’s look at redox titrations in more detail.
Do you remember other redox titrations that we have done in the laboratory?
Yes, we have done other redox titrations like the determination of the percent of hydrogen peroxide and other ones.
Now, we are going to look at the redox titrations involving iodine.
Notice here that there are two types of redox titrations involving iodine.
The most important thing in this presentation is for you to understand the differences between iodometric and iodimetric titrations. Both involve iodine, but as you will see there are some differences.
The analysis that we will perform in the laboratory is the iodometric titration of cooper, which is a classical quantitative chemical analysis, a redox titration involving iodine. It is used because it is necessary to quantify copper in water, alloys, minerals and so on
Slide 5:
As we saw in slide 2, we classify redox titrations according to the titrant which is being used.
There are a lot of redox titrations and the most common ones are:
First we have Permanganimetric redox titrations where the titrant is KMnO4 (Potassium permanganate).
Then we have dichromatometric redox titrations where the titrant is K2Cr2O7 (Potassium dichromate).
And finally the titrations that interest us today are the titrations involving iodine (I2). We divide these titrations into two types.
Iodimetry –that is, i-o-DI-metry
Iodometry – and i-o-DO-metry
Notice that the two names are very similar; the objective of this talk is for you to learn the difference between the two types.
As we said before titrations that create or consume I2 are widely used in quantitative analysis.
Slide 7:
Now let’s move on to iodometric titrations
Unlike iodimetric titrations , in the iodometric ones two reactions are involved.
Let’s analyze these two reactions.
In this case the analyte is an oxidizing agent. Consequently, in the first reaction
The analyte reacts with an excess of iodur to generate iode
Slide 8:
To summarise the main information about iodimetric and iodometric titrations:
In iodimetric titrations:
The anlyte is a reducing agent.
One reaction is involved.
The standard solution is Iodine (I2)
On the other hand in iodometric titrations:
The analyte is an oxidizing agent.
Two reactions are involved.
The standard solution is sodium thiosulfate.