Unit 13: Applications of Inorganic Chemistry
Learning aim B: Investigate oxidation-reduction reactions in order to understand their
many applications in analysis.
Index.
Introduction,
Oxidation and Reduction,
Half equations and Redox Reactions,
Standard cell voltages and Comparison,
Electrochemical cell half equations and redox reactions,
Balanced redox equations in terms of numbers of electrons,
Oxidation/Reduction sheet,
Observations,
Standardise solution by titration,
Redox equations involved in each titrations,
Evaluating techniques used in industry,
References.
Introduction.
This report will Demonstrate how to determine the concentration of analytes using analytical
procedures involving oxidation and reduction also demonstrate how to determine accurate oxidation
numbers for species in equations to identify reactions involving oxidation and reduction and a
comparison measured cell voltages for electrochemical cells involving metal/metal ion half-cells with
voltages calculated using oxidation, reduction and redox equations Furthermore explain the redox
reactions involved in analytical procedures in terms of the oxidation numbers for the species involved.
It will also express oxidation, reduction and redox equations and calculate standard cell voltages for
given pairs of half cells. Finally evaluating the industrial use of analytical procedures using redox
reactions.
Oxidation is the process of a molecule, atom, or ion losing electrons or increasing its oxidation state.
During the reaction process, a molecule, atom, or i on receives or loses electrons, depending on its
oxidation status.
Cell voltage of Given cells.
Copper and Zinc = 1.07V
Copper and Lead = 0.13V
Lead and Zinc = 1.9V
Iron Content of substances
Mass of 1 tablet = 0.6g
Determination titrate (ml)
1. 19.2
1
, 2. 18.7
3. 20
Mean = 19.3
Average % per tablet = 19.3 x0.002/1000
X5
X56/0.56
X100
= 18.01%
Concentration of bleach
1. 12M
2. 16M
3. 11M
Mean = 13M
Volume of HCl Volume of Volume of water Time taken to Temperature of
(ml) Na2SO3 (ml) (ml) turn opaque (s) solution when
opaque (C)
10 30 10 111 21
10 25 15 131 21
10 20 20 179 21
10 15 25 282 21
10 10 30 435 21
10 5 35 N/A 21
We also completed an experiment in which we put potassium dichromate, alcohol, and sulphuric acid
in a test tube and heated it. The colour changed from yellow to green. This is the result because the
alcohol has been transformed to an aldehyde and then to a carboxylic acid. Potassium dichromate
can also be used to assess chemical oxygen demand. Potassium dichromate is converted to Cr3+
when it is oxidised. Following the completion of the oxidation, the amount of Cr3+ is estimated, which
can subsequently be used as an indirect indicator of the water sample's organic composition. This is
how you can figure out how much chemical oxygen you'll need. Two ways for determining the amount
of chromium in a particular state are titrimetric and colorimetric approaches.
There are only a few examples of oxidation-reduction processes' consequences. In their most basic
form, these are electron-transfer processes. Oxidation-reduction analysis has been used as an
alternate method of analysing materials with many oxidation states over the years. This unit's goal is
to help us connect what happens at the sub microscopic level to the macroscopic electrochemistry
processes that we see.
Chemists frequently use the terms oxidising and reducing substances to describe the reactants in
redox reactions. Because oxidation entails the loss of electrons, an oxidising agent is any substance
that can cause an electron loss in another substance during a chemical process. As a result, an
oxidising agent obtains electrons, which lowers its oxidation number (a positive or negative number
that reflects an atom's oxidation state as defined below). On the other hand, reduction is the process
of gaining electrons, hence a reducing agent is a substance that can cause another substance to gain
electrons. On the other hand, as it oxidises the other reagent, an oxidising agent is decreased.
We can easily distinguish between oxidised and reduced elements by using oxidation numbers.
Higher oxidation number elements, such as hydrogen and sulphur in the examples above, are
oxidised. Their oxidation values are lower than before because chlorine and oxygen have been
reduced. It's worth noting that the sum of the H and Cl oxidation numbers (+1 and -1) in HCl is zero.
2
Learning aim B: Investigate oxidation-reduction reactions in order to understand their
many applications in analysis.
Index.
Introduction,
Oxidation and Reduction,
Half equations and Redox Reactions,
Standard cell voltages and Comparison,
Electrochemical cell half equations and redox reactions,
Balanced redox equations in terms of numbers of electrons,
Oxidation/Reduction sheet,
Observations,
Standardise solution by titration,
Redox equations involved in each titrations,
Evaluating techniques used in industry,
References.
Introduction.
This report will Demonstrate how to determine the concentration of analytes using analytical
procedures involving oxidation and reduction also demonstrate how to determine accurate oxidation
numbers for species in equations to identify reactions involving oxidation and reduction and a
comparison measured cell voltages for electrochemical cells involving metal/metal ion half-cells with
voltages calculated using oxidation, reduction and redox equations Furthermore explain the redox
reactions involved in analytical procedures in terms of the oxidation numbers for the species involved.
It will also express oxidation, reduction and redox equations and calculate standard cell voltages for
given pairs of half cells. Finally evaluating the industrial use of analytical procedures using redox
reactions.
Oxidation is the process of a molecule, atom, or ion losing electrons or increasing its oxidation state.
During the reaction process, a molecule, atom, or i on receives or loses electrons, depending on its
oxidation status.
Cell voltage of Given cells.
Copper and Zinc = 1.07V
Copper and Lead = 0.13V
Lead and Zinc = 1.9V
Iron Content of substances
Mass of 1 tablet = 0.6g
Determination titrate (ml)
1. 19.2
1
, 2. 18.7
3. 20
Mean = 19.3
Average % per tablet = 19.3 x0.002/1000
X5
X56/0.56
X100
= 18.01%
Concentration of bleach
1. 12M
2. 16M
3. 11M
Mean = 13M
Volume of HCl Volume of Volume of water Time taken to Temperature of
(ml) Na2SO3 (ml) (ml) turn opaque (s) solution when
opaque (C)
10 30 10 111 21
10 25 15 131 21
10 20 20 179 21
10 15 25 282 21
10 10 30 435 21
10 5 35 N/A 21
We also completed an experiment in which we put potassium dichromate, alcohol, and sulphuric acid
in a test tube and heated it. The colour changed from yellow to green. This is the result because the
alcohol has been transformed to an aldehyde and then to a carboxylic acid. Potassium dichromate
can also be used to assess chemical oxygen demand. Potassium dichromate is converted to Cr3+
when it is oxidised. Following the completion of the oxidation, the amount of Cr3+ is estimated, which
can subsequently be used as an indirect indicator of the water sample's organic composition. This is
how you can figure out how much chemical oxygen you'll need. Two ways for determining the amount
of chromium in a particular state are titrimetric and colorimetric approaches.
There are only a few examples of oxidation-reduction processes' consequences. In their most basic
form, these are electron-transfer processes. Oxidation-reduction analysis has been used as an
alternate method of analysing materials with many oxidation states over the years. This unit's goal is
to help us connect what happens at the sub microscopic level to the macroscopic electrochemistry
processes that we see.
Chemists frequently use the terms oxidising and reducing substances to describe the reactants in
redox reactions. Because oxidation entails the loss of electrons, an oxidising agent is any substance
that can cause an electron loss in another substance during a chemical process. As a result, an
oxidising agent obtains electrons, which lowers its oxidation number (a positive or negative number
that reflects an atom's oxidation state as defined below). On the other hand, reduction is the process
of gaining electrons, hence a reducing agent is a substance that can cause another substance to gain
electrons. On the other hand, as it oxidises the other reagent, an oxidising agent is decreased.
We can easily distinguish between oxidised and reduced elements by using oxidation numbers.
Higher oxidation number elements, such as hydrogen and sulphur in the examples above, are
oxidised. Their oxidation values are lower than before because chlorine and oxygen have been
reduced. It's worth noting that the sum of the H and Cl oxidation numbers (+1 and -1) in HCl is zero.
2
