This document provides the procedure for volumetrically estimating the amount of nitrite in a given sodium nitrite solution using potassium permanganate (KMnO4). Key steps include standardizing the KMnO4 solution using sodium oxalate, acidifying the solutions with sulfuric acid to promote the redox reaction between KMnO4 and nitrite ions, and titrating the nitrite solution with KMnO4 until the pink color disappears. The amount of nitrite in the original sample solution can then be calculated from the titration results.
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Determination of the order of reaction between potassium persulphate & potass...PRAVIN SINGARE
This presentation is based on the experimental demonstration of "Determination of the order of reaction between potassium persulphate & potassium iodide by fractional change method". The presentation is for chemistry Undergraduate student of Mumbai University.
Here we have discussed about the separation of binary organic mixtures and identification of the functional groups and preparation of solid derivatives.
To estimate amount of ferrous(fe2+) and ferric(fe3+) ions in the given soluti...Mithil Fal Desai
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In Job's method, the variation in concentration of the reactants is performed which can reveal the empirical formula of a complex. The method is employed to find the formula of the compound formed by reacting two or more chemical species. The absorption is recorded against different wavelengths and wavelength having maximum absorption is selected. The intensity of solutions with different stoichiometric ratios of the reactants is measured. The highest observed intensity reveals the maximum amount of compound formed. In this experiment, the Fe3+ and salicylic acid are reacted and the wavelength at which the complex absorbs strongly is selected. The absorbance of the different stoichiometric ration of Fe3+ and salicylic acid at a selected wavelength is determined. The maximum absorbance of the solution of the stoichiometric ratio reveals the empirical formula of the complex as the maximum amount of coloured complex is formed.
To estimate amount of ferrous(fe2+) and ferric(fe3+) ions in the given soluti...Mithil Fal Desai
To estimate amount of ferrous (Fe2+) and ferric (Fe3+) ions in the given solution containing ferric chloride and ferrous sulphate by using potassium dichromate
Determine the composition of the fe3+(jobs method)Mithil Fal Desai
In Job's method, the variation in concentration of the reactants is performed which can reveal the empirical formula of a complex. The method is employed to find the formula of the compound formed by reacting two or more chemical species. The absorption is recorded against different wavelengths and wavelength having maximum absorption is selected. The intensity of solutions with different stoichiometric ratios of the reactants is measured. The highest observed intensity reveals the maximum amount of compound formed. In this experiment, the Fe3+ and salicylic acid are reacted and the wavelength at which the complex absorbs strongly is selected. The absorbance of the different stoichiometric ration of Fe3+ and salicylic acid at a selected wavelength is determined. The maximum absorbance of the solution of the stoichiometric ratio reveals the empirical formula of the complex as the maximum amount of coloured complex is formed.
It consists of Titration experiments.It consists of four experiments
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Volumetric estimation of nitrite in the given solution of sodium nitrite using KMnO4
1. Aim: Volumetric estimation of nitrite in the given solution of sodium nitrite using KMnO4.
Chemicals: Potassium permanganate, sulphuric acid, sodium oxalate, sodium nitrite.
Apparatus: Standard volumetric flask, pipette, burette, conical flask, beakers, funnel and glass rod.
Theory: The aqueous solution of KMnO4 needs to be standardized using sodium oxalate. Nitrite is
oxidized using KMnO4 in an acidic medium. In the estimation of nitrite, the acidified KMnO4 is taken
in a beaker and titrated against sodium nitrite solution, as H2SO4 reacts with nitrite to give nitrous acid
which decomposes to nitrous oxide and water.
Reactions:
2KMnO4 + 5H2C2O4 + 3H2SO4 2MnSO4 + K2SO4 + 10CO2 + 8H2O
5NaNO2 + 2KMnO4 + 3H2SO4 5NaNO3 + 2MnSO4 + K2SO4 + 3H2O
Procedure:
i) Preparation of 0.01N KMnO4 (500 mL) [molecular weight check on the chemical container], calculate
ii) Preparation of 2N H2SO4 (250 mL) [Laboratory normality 36 N],calculate
iii) Preparation of 0.01N Na2C2O4 (500mL) [molecular weight check on the chemical container], calculate
vi) Standardization of KMnO4
Rinse the clean burette with a minimum quantity of KMnO4 and fill it appropriately. Pipette out 10 mL
of 0.01 N sodium oxalate solution in a clean conical flask. Add about 20 mL of 2N H2SO4. Heat the
solution in the flask to about 60 °C. Titrate it against KMnO4, until light pink color permanently
develops in the flask. Repeat the titration to get constant readings.
v) Estimation of nitrite.
Rinse the clean burette with a minimum quantity of sodium nitrite solution and fill it appropriately.
Pipette out 10 mL of given KMnO4 solution in a clean beaker and add 40 mL of 2N H2SO4. Warm the
solution from the beaker (40 °C). Dip the tip of the burette in solution in the beaker. Titrate the solution
from the beaker against the nitrite solution, until the pink color of KmNO4 disappears. Repeat the
titration to get the constant readings.
Results:
i) The amount of nitrite in 100 mL is ___g.
ii) The amount of sodium nitrite in 100 mL is ___g.
Further reading (available in the library)
1) Experiments in Applied Chemistry, S. Rattan, S. K Kataria and Sons.
2) Vogel’s textbook of quantitative chemical analysis, J. Mendham, R. C. Denney, J. D. Barns, M.
Thomas, B. Sivasankar, Pearson India Education, 6th
Edition.
Questions.
1) Calculate the oxidation state of nitrogen in nitrate and nitrite.
2) Can we use not HCl or HNO3 in redox titrations?
3) Is it possible to quantitatively determine ferric ions by this method?
4) Why the tip of the burette is dipped in the solution?
![Aim: Volumetric estimation of nitrite in the given solution of sodium nitrite using KMnO4.
Chemicals: Potassium permanganate, sulphuric acid, sodium oxalate, sodium nitrite.
Apparatus: Standard volumetric flask, pipette, burette, conical flask, beakers, funnel and glass rod.
Theory: The aqueous solution of KMnO4 needs to be standardized using sodium oxalate. Nitrite is
oxidized using KMnO4 in an acidic medium. In the estimation of nitrite, the acidified KMnO4 is taken
in a beaker and titrated against sodium nitrite solution, as H2SO4 reacts with nitrite to give nitrous acid
which decomposes to nitrous oxide and water.
Reactions:
2KMnO4 + 5H2C2O4 + 3H2SO4 2MnSO4 + K2SO4 + 10CO2 + 8H2O
5NaNO2 + 2KMnO4 + 3H2SO4 5NaNO3 + 2MnSO4 + K2SO4 + 3H2O
Procedure:
i) Preparation of 0.01N KMnO4 (500 mL) [molecular weight check on the chemical container], calculate
ii) Preparation of 2N H2SO4 (250 mL) [Laboratory normality 36 N],calculate
iii) Preparation of 0.01N Na2C2O4 (500mL) [molecular weight check on the chemical container], calculate
vi) Standardization of KMnO4
Rinse the clean burette with a minimum quantity of KMnO4 and fill it appropriately. Pipette out 10 mL
of 0.01 N sodium oxalate solution in a clean conical flask. Add about 20 mL of 2N H2SO4. Heat the
solution in the flask to about 60 °C. Titrate it against KMnO4, until light pink color permanently
develops in the flask. Repeat the titration to get constant readings.
v) Estimation of nitrite.
Rinse the clean burette with a minimum quantity of sodium nitrite solution and fill it appropriately.
Pipette out 10 mL of given KMnO4 solution in a clean beaker and add 40 mL of 2N H2SO4. Warm the
solution from the beaker (40 °C). Dip the tip of the burette in solution in the beaker. Titrate the solution
from the beaker against the nitrite solution, until the pink color of KmNO4 disappears. Repeat the
titration to get the constant readings.
Results:
i) The amount of nitrite in 100 mL is ___g.
ii) The amount of sodium nitrite in 100 mL is ___g.
Further reading (available in the library)
1) Experiments in Applied Chemistry, S. Rattan, S. K Kataria and Sons.
2) Vogel’s textbook of quantitative chemical analysis, J. Mendham, R. C. Denney, J. D. Barns, M.
Thomas, B. Sivasankar, Pearson India Education, 6th
Edition.
Questions.
1) Calculate the oxidation state of nitrogen in nitrate and nitrite.
2) Can we use not HCl or HNO3 in redox titrations?
3) Is it possible to quantitatively determine ferric ions by this method?
4) Why the tip of the burette is dipped in the solution?](https://image.slidesharecdn.com/volumetricestimationofnitriteinthegivensolutionofsodiumnitriteusingkmno4-210405065036/85/Volumetric-estimation-of-nitrite-in-the-given-solution-of-sodium-nitrite-using-KMnO4-1-320.jpg)
