Conductance of electrolyte solution, specific, equivalent and molar conductance. Determination conductance of electrolyte solution, Cell constant its determination and problems
This presentation consists of three topics that are:
1. conductance of electrolytic solution
2. Specific Conductance, Molar Conductance & Equivalent Conductance
3. Kohlrausch's Law
This presentation consists of three topics that are:
1. conductance of electrolytic solution
2. Specific Conductance, Molar Conductance & Equivalent Conductance
3. Kohlrausch's Law
Conductometry / conductometric titrationRabia Aziz
more chemistry contents are available
1. pdf file on Termmate: https://www.termmate.com/rabia.aziz
2. YouTube: https://www.youtube.com/channel/UCKxWnNdskGHnZFS0h1QRTEA
3. Facebook: https://web.facebook.com/Chemist.Rabia.Aziz/
4. Blogger: https://chemistry-academy.blogspot.com/
conductometric titration
ELECTRICAL DOUBLE LAYER-TYPES-DYNAMICS OF ELECTRON TRANSFER-MARCUS THEORY-TUNNELING - BUTLER VOLMER EQUATIONS-TAFEL EQUATIONS-POLARIZATION AND OVERVOLTAGE-CORROSION AND PASSIVITY-POURBAIX AND EVAN DIAGRAM-POWER STORAGE-FUEL CELLS
Conductometry / conductometric titrationRabia Aziz
more chemistry contents are available
1. pdf file on Termmate: https://www.termmate.com/rabia.aziz
2. YouTube: https://www.youtube.com/channel/UCKxWnNdskGHnZFS0h1QRTEA
3. Facebook: https://web.facebook.com/Chemist.Rabia.Aziz/
4. Blogger: https://chemistry-academy.blogspot.com/
conductometric titration
ELECTRICAL DOUBLE LAYER-TYPES-DYNAMICS OF ELECTRON TRANSFER-MARCUS THEORY-TUNNELING - BUTLER VOLMER EQUATIONS-TAFEL EQUATIONS-POLARIZATION AND OVERVOLTAGE-CORROSION AND PASSIVITY-POURBAIX AND EVAN DIAGRAM-POWER STORAGE-FUEL CELLS
This portion of power point presentation on electrochemistry includes, electrolytic conduction, conductivity, cell constant, molar conductivity, variation with concentration & temperature, Debye Huckel Onsager equation, Limiting molar conductivity, Kohlrausch law of independent migration of ions, its application & numerical problems.
Introduction to Electrochemistry
- Electrochemistry explores the interplay between electrical energy and chemical reactions, focusing on oxidation-reduction (redox) reactions and electrochemical cells.
**Oxidation and Reduction**
- Oxidation involves the loss of electrons, while reduction involves the gain of electrons, summed up by the mnemonic OIL RIG. An example reaction is Zn + Cu²⁺ → Zn²⁺ + Cu.
**Redox Reactions in Everyday Life**
- Examples include the rusting of iron, cellular respiration, and the combustion of fuels.
**Electrochemical Cells**
- Two main types are Galvanic (Voltaic) cells, which convert chemical energy into electrical energy, and Electrolytic cells, which use electrical energy to drive chemical reactions. Components include the anode (where oxidation occurs), the cathode (where reduction occurs), and an electrolyte.
**Galvanic Cells**
- A common example is the Daniell Cell, which generates electrical energy through spontaneous redox reactions.
**Electrolytic Cells**
- These cells drive non-spontaneous reactions using electrical energy, such as the electrolysis of water to produce hydrogen and oxygen gases.
**Applications of Electrochemistry**
- Includes batteries (e.g., lithium-ion, alkaline), electroplating, corrosion prevention methods like galvanization, and fuel cells that directly convert chemical energy into electrical energy.
**Electrochemistry in Nature**
- Involves biochemical processes like the electron transport chain in mitochondria and natural galvanic cells, such as those influenced by lightning in soil.
**Summary**
- Understanding redox reactions and electrochemical cells is essential. Electrochemistry has a wide range of practical applications, making it a significant field of study.
**Discussion and Q&A**
- Engage with the audience to explore real-life applications and recent advancements in electrochemistry.
This summary encapsulates the key points and themes of the presentation, providing a concise overview of the fundamental concepts and applications of electrochemistry.
ELECTROCHEMISTRY - I
4.1 - Metallic and Electrolytic Conductors-Faraday’s Laws-Electro plating Specific conductance and Equivalent conductance - Measurement of equivalent conductance - Variation of Equivalent Conductance and Specific Conductance with Dilution Kohlrausch Law and its applications - Ostwald’s Dilution Law and its Limitations.
• Electrolytes : Definition, Strong and weak electrolytes and their conductance measurement, Ions and electrical conductivity by ions
• Kohlrausch law of Independent Migration of Ions
• Applications of Kohlrausch law
• Transference No. and its determination using Moving Boundary Method
• Factors affecting transport number
Quantum yield, experimental arrangement, reasons for high and low Quantum yield, problems, photochemical reactions, kinetics of photochemical decomposition of HI, photosensitized reaction, mechanism of photosensitization,
Nernst distribution law and its application to association and dissociation of solute in one of the solvent. Processes of extraction, derivation of formula for the amount of solute left unextracted after nth extraction.
This presentation explain most important property of liquid viscosity. This presentation includes definition, its experimental determination, effect of temperature and Application which is very useful to the B Sc-II (Sem-III) student of SGBAU, Amravati
This presentation includes the most important property of liquid that is surface tension. This Presentation is useful for the B Sc II students of SGBAU, Amravati
This presentation includes the most important cell used in polarography Dropping Mercury Electrode. Its structure, uses/Advantages and limitations are explain here
More from Shri Shivaji Science College Amravati (20)
How to Split Bills in the Odoo 17 POS ModuleCeline George
Bills have a main role in point of sale procedure. It will help to track sales, handling payments and giving receipts to customers. Bill splitting also has an important role in POS. For example, If some friends come together for dinner and if they want to divide the bill then it is possible by POS bill splitting. This slide will show how to split bills in odoo 17 POS.
Synthetic Fiber Construction in lab .pptxPavel ( NSTU)
Synthetic fiber production is a fascinating and complex field that blends chemistry, engineering, and environmental science. By understanding these aspects, students can gain a comprehensive view of synthetic fiber production, its impact on society and the environment, and the potential for future innovations. Synthetic fibers play a crucial role in modern society, impacting various aspects of daily life, industry, and the environment. ynthetic fibers are integral to modern life, offering a range of benefits from cost-effectiveness and versatility to innovative applications and performance characteristics. While they pose environmental challenges, ongoing research and development aim to create more sustainable and eco-friendly alternatives. Understanding the importance of synthetic fibers helps in appreciating their role in the economy, industry, and daily life, while also emphasizing the need for sustainable practices and innovation.
Palestine last event orientationfvgnh .pptxRaedMohamed3
An EFL lesson about the current events in Palestine. It is intended to be for intermediate students who wish to increase their listening skills through a short lesson in power point.
Model Attribute Check Company Auto PropertyCeline George
In Odoo, the multi-company feature allows you to manage multiple companies within a single Odoo database instance. Each company can have its own configurations while still sharing common resources such as products, customers, and suppliers.
This is a presentation by Dada Robert in a Your Skill Boost masterclass organised by the Excellence Foundation for South Sudan (EFSS) on Saturday, the 25th and Sunday, the 26th of May 2024.
He discussed the concept of quality improvement, emphasizing its applicability to various aspects of life, including personal, project, and program improvements. He defined quality as doing the right thing at the right time in the right way to achieve the best possible results and discussed the concept of the "gap" between what we know and what we do, and how this gap represents the areas we need to improve. He explained the scientific approach to quality improvement, which involves systematic performance analysis, testing and learning, and implementing change ideas. He also highlighted the importance of client focus and a team approach to quality improvement.
Unit 8 - Information and Communication Technology (Paper I).pdfThiyagu K
This slides describes the basic concepts of ICT, basics of Email, Emerging Technology and Digital Initiatives in Education. This presentations aligns with the UGC Paper I syllabus.
The Art Pastor's Guide to Sabbath | Steve ThomasonSteve Thomason
What is the purpose of the Sabbath Law in the Torah. It is interesting to compare how the context of the law shifts from Exodus to Deuteronomy. Who gets to rest, and why?
Welcome to TechSoup New Member Orientation and Q&A (May 2024).pdfTechSoup
In this webinar you will learn how your organization can access TechSoup's wide variety of product discount and donation programs. From hardware to software, we'll give you a tour of the tools available to help your nonprofit with productivity, collaboration, financial management, donor tracking, security, and more.
Welcome to TechSoup New Member Orientation and Q&A (May 2024).pdf
Lect. 6. conductivity cell constant-problems
1. Dr. Y. S. THAKARE
M.Sc. (CHE) Ph D, NET, SET
Assistant Professor in Chemistry,
Shri Shivaji Science College, Amravati
Email: yogitathakare_2007@rediffmail.com
B Sc- II Year
SEM-III
PAPER-III
PHYSICAL CHEMISTRY
UNIT- VI
Introduction to electrochemistry
16-October -20 1
2. Education is the most powerful weapon
which you can use to change the world.
-Nelson Mandela
Be kind whenever possible. It is always
possible.
-Dalai Lama
There is no substitute for hard work.
-Thomas A. Edison
3. Electrochemistry: The Branch of physical chemistry which
deals with the study of interconversion of electrical energy
in to chemical energy or vice-versa
Electrolytic Cell: Conversion of electrical energy in to
chemical energy
Electrochemical Cell: Conversion of chemical energy into
electrical energy
Electrode – The metal rod dipped in its salt solution
5. A substance which decomposes on passing current through it is
known as electrolyte and phenomenon of decomposition is called
electrolysis.
6.
7.
8.
9.
10. Conductance of electrolyte solutions:
The capacity of conductor to carry the electrical current
(energy) is known as the conductance or conductivity. We generally
come across with two conductors i.e. metallic and electrolytic
conductors.
The conductance of electrolyte solution is due to migration of ions
through the solution to the electrodes. The conductance (C) of an
electrolyte is the reciprocal of its resistance (R).
Thus, 𝐶 =
1
𝑅
It is measured in ohm-1 or mho or Siemens (S).
Resistance of any uniform conductor varies directly as its
length and inversely to its area of cross section.
R ∝
𝑙
𝑎
OR R = ρ
𝑙
𝑎
Where, ρ = constant called specific resistance or resistivity
l = length of conductor
a = cross sectional area of conductor
11. R = ρ
𝑙
𝑎
When l = a = 1,
R = ρ
Hence, specific resistance is the resistance of
length and unit cross sectional area
OR It is the resistance of 1 m3 material.
12. Specific conductance ( ): “The conductance of one centimeter
cube (1 cm3) or one cubic meter (1 m3) solution of an electrolyte
an electrolyte is known as specific conductance.” It is denoted by
is denoted by ‘ ’ (Kappa).
Specific conductance () is reciprocal of specific resistance (ρ).
.˙.
13. For electrolytes specific conductance is the conductance of one
meter cube of solution.
Unit of Conductance
We know that
= C
𝑙
𝑎
CGS unit
= 𝑜ℎ𝑚−1
𝑐𝑚
𝑐𝑚2
= 𝑜ℎ𝑚−1𝑐𝑚−1 = 𝑚ℎ𝑜 𝑐𝑚−1 = 𝑆𝑐𝑚−1
SI Unit
= 𝑜ℎ𝑚−1
𝑚
𝑚2
= 𝑜ℎ𝑚−1
𝑚−1
= 𝑚ℎ𝑜 𝑚−1
= 𝑆𝑚−1
Its CGS unit is ohm-1 cm-1 or S cm-1 & SI unit is ohm-1 m-1 or S m-1.
14. Equivalent conductance : It is defined as the conductance of a
solution containing one Kg equivalent of electrolyte placed between
placed between two parallel electrodes 1 meter apart. It is denoted
It is denoted by 𝑣 .
OR
“The conductance of one gram equivalent of an electrolyte, dissolved
electrolyte, dissolved in ‘V’cc of water.”
It is the product of specific conductivity and the volume of solution
containing 1 kg equivalent of electrolyte.
𝑣 = V
In general, if an electrolyte solution contains ‘N’ gram equivalent in
1000 cc of solution. Then,
𝑣 =
× 1000
𝑁
15. Unit of Equivalent conductance
We know that
𝑣 =
× 1000
𝑁
CGS unit
𝑣 =
𝑆𝑐𝑚−1 × 𝑐𝑚3
𝑒𝑞
= 𝑆𝑐𝑚2
𝑒𝑞−1
= 𝑜ℎ𝑚−1
𝑐𝑚2
𝑒𝑞−1
= 𝑚ℎ𝑜 𝑐𝑚2𝑒𝑞−1
SI Unit
𝑣 =
𝑆𝑚−1 × 𝑚3
𝑒𝑞
= 𝑆𝑚2𝑒𝑞−1 = 𝑜ℎ𝑚−1𝑚2𝑒𝑞−1 = 𝑚ℎ𝑜 𝑚2𝑒𝑞−1
In CGS system its unit is mho cm2 eq-1 or S cm2 eq-1. The SI unit of
equivalent conductance is mho m2 eq-1 or S m2 eq-1
16. Molar conductance (µ𝑣): “It is defined as conductance of solution
containing one mole of electrolyte placed between two parallel
parallel electrodes one meter apart.” It is denoted by (µ𝑣 ).
).
OR
“The conductance of the solution containing one gram mole of
mole of electrolyte is known as molar conductance”.
If one gram mole of electrolyte dissolved in ‘V’cc of solution, then its
molar conductance is given as
µ𝑣 = V
= specific conductance
V = volume of solution in meter cube containing 1 gm molecular
molecular weight of an electrolyte.
µ𝑣 =
× 1000
𝑀
17. Unit of Molar Conductance
We know that
µ𝑣 =
× 1000
𝑀
CGS unit
µ𝑣 =
𝑆𝑐𝑚−1
× 𝑐𝑚3
𝑚𝑜𝑙
= 𝑆𝑐𝑚2
𝑚𝑜𝑙−1
= 𝑜ℎ𝑚−1
𝑐𝑚2
𝑚𝑜𝑙−1
= 𝑚ℎ𝑜 𝑐𝑚2𝑚𝑜𝑙−1
SI Unit
µ𝑣 =
𝑆𝑚−1 × 𝑚3
𝑚𝑜𝑙
= 𝑆𝑚2
𝑚𝑜𝑙−1
= 𝑜ℎ𝑚−1
𝑚2
𝑚𝑜𝑙−1
= 𝑚ℎ𝑜 𝑚2
𝑚𝑜𝑙−1
In CGS system its unit is mho cm2 𝑚𝑜𝑙 -1 or S cm2 𝑚𝑜𝑙 -1. The SI unit of
equivalent conductance is mho m2 eq-1 or S m2 𝑚𝑜𝑙 -1
18. Determination of conductance of electrolyte solution using
Wheatstone bridge method :
Conductance of an electrolytic solution is the reciprocal of
resistance (C=1/R). Therefore, measurement of conductance is
done indirectly by determining the resistance of the solution. The
resistance is measured by Wheatstone AC bridge method. Direct
current cannot be used in this process as this will give wrong result
due to
1. Change in concentration due to electrolysis.
2. Change in resistance due to polarization at electrodes
19.
20. These difficulties are overcome by using alternating current within
audio frequency range and galvanometer in Wheatstone bridge is
replaced by headphone. The schematic diagram of the apparatus is
shown in fig.
The solution whose conductivity is to be determined is taken in a
suitable conductivity cell ‘C’. When current is flowing know resistance
‘R’ is introduced through resistance box. The sliding contact ‘X’ is then
moved along the wire ‘AB’ of uniform thickness until a point of
minimum sound is detected in headphone (G). At this stage,
𝑅𝑒𝑠𝑖𝑠𝑡𝑎𝑛𝑐𝑒 𝑜𝑓 𝑠𝑜𝑙𝑢𝑡𝑖𝑜𝑛
𝑅𝑒𝑠𝑖𝑠𝑡𝑎𝑛𝑐𝑒 𝑓𝑟𝑜𝑚 𝑟𝑒𝑠𝑖𝑠𝑡𝑎𝑛𝑐𝑒 𝑏𝑜𝑥
=
𝐿𝑒𝑛𝑔𝑡ℎ 𝐵𝑋
𝐿𝑒𝑛𝑔𝑡ℎ 𝐴𝑋
As all values from above equation are known, resistance of solution
can be determined. From this resistance, conductance of solution can
be determined.
21. Determination of cell constant:
Cell constant () is defined as the ratio of length (distance) between the
electrodes ‘l’ and area of cross section ‘a’ of electrode.
𝐶𝑒𝑙𝑙 𝑐𝑜𝑛𝑠𝑡𝑎𝑛𝑡 = =
𝑙
𝑎
In order to determine cell constant () it is necessary to determine ‘l’ & ‘a’.
But actually it is not possible. So indirect method based on measurement of
conductance of standard KCl solution is employed as follows:
We know that
= C
𝑙
𝑎
Specific conductance = Observed conductance × 𝐶𝑒𝑙𝑙 𝑐𝑜𝑛𝑠𝑡𝑎𝑛𝑡
To determine the cell constant, a standard solution of KCl of known specific
conductance at a given temperature is used. Its conductance is determined
experimentally at the same temperature. Substituting the two values in
above equation, the cell constant can be calculated.
22. Variation of specific and equivalent conductance with
dilution:
The solution of electrolyte conducts electricity due to the
presence of ions. The conductivity at constant temperature is
approximately proportional to number of ions. According to
ionic theory the number of ions increases as the solution of the
electrolyte is progressively diluted. Therefore, equivalent
conductivity increases as the dilution increases.
The specific conductivity decreases on dilution because on
dilution the number of ions per dm3 of solution decreases in spite
of increase in dissociation.
The equivalent and molecular conductivity increases because
these are the product of specific conductivity and volume
containing on gram equivalent or one mole of an electrolyte.
𝑣 = V
On dilution, decrease in specific conductance is compensated by
increase in volume ‘V’. This behavior can be illustrated from the
table.
24. Example: 1
A conductivity cell was filled with 0.01 M KCl which was known to have specific
conductivity of 0.1404 mho m-1 at 298 K. Its measured resistance at 298 K was 99.3
ohm. When the cell was filled with 0.02M AgNO3, the resistance was 50.3 ohm.
Calculate (i) Cell constant, (ii) Specific Conductance of AgNO3 solution.
Solution: Given that
(i) For 0.01 M KCl, = 0.1404 mho m-1
T = 298 K
R = 99.3 ohm
We know that
Cell constant =
Sp. Conductance ( )
Observe Conductance
=
0.1404
1/99.3
= 0.1404 × 99.3
= 13.94
(ii) For 0.02 M AgNO3, R = 50.3 ohm
Sp. Conductance ( ) = Cell constant × Observe Conductance
= 13.94 X 1/50.3
= 13.94 X 50.3
= 0.2771 mho m-1
25. Example: 2
0.5 N solution of salt occupying volume between two platinum electrodes
0.0172 m apart and 0.04499 sq. m. area has resistance 25 ohm. Calculate
equivalent conductance of solution.
Solution: Given that
distance between electrodes, l = 0.0172 m
area of cross section of electrode a = 0.04499 sq. m.
resistance of salt solution R = 25 ohm
Concentration of salt solution C = 0.5N
Sp. conductance () = Cell constant × Observed conductance
=
0.0172
0.04499
×
1
25
= 0.3823 × 0.04
= 0.01529 mho 𝑚−1
Equivalent Conductance λv = Sp. conductance × V
𝑣 =
× 1000
𝑁
=
0.01529 × 1000
0.5
= 0.01529 X 0.04499=30.58 S 𝑚2𝑒𝑞𝑢𝑖−1
26. Example: 3
The resistance of conductivity cell was 7.02 ohm when filled with 0.1 N KCl solution
(k=0.1480 ohm-1 m-1) and 69.2 ohm, when filled with N/100 NaCl solution at same
temperature. Calculate the cell constant and equivalent conductance of NaCl solution.
Solution:
(i) For 0.1 N KCl, R = 7.02 ohm
= 0.1480 ohm-1 m-1
Cell constant =
Sp. Conductance ( )
Observe Conductance
=
0.1480
1
7.02
= 0.1480 × 7.02
= 1.038 𝑚−1
(ii) For N/100 or 0.01 N NaCl,
R = 69.2 ohm
Sp. conductance () = Cell constant × Observed conductance
= 1.038 X 1 / 69.2
= 0.015 S m-1
=
Equivalent Conductance λv = Sp. conductance × V
𝑣 =
0.015 × 1000
0.01
=15000 𝑚2𝑒𝑞𝑢𝑖−1