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Redox titration, a powerful analytical method, involves the process of titrating an oxidizing agent with a reducing agent until a specific endpoint is achieved, facilitating the determination of a substance's concentration within a solution. This report delves into the experimental determination of the molarity and concentration of an iron (II) sulfate (FeSO4) solution through redox titration with potassium permanganate (KMnO4). The change in color to light pink at the endpoint serves as a visual indicator for the completion of the reaction.
By meticulously analyzing titration data and employing stoichiometric relationships, the experiment aims to ascertain the molarity and concentration of the FeSO4 solution, juxtaposing experimental findings with theoretical predictions.
Redox titration is predicated on the redox reaction between the analyte and titrant, where the transfer of electrons from the reducing agent to the oxidizing agent occurs until equilibrium is reached. The reaction between FeSO4 and KMnO4 is described by the equation:
5Fe2++MnO4−+8H+→5Fe3++Mn2++4H2O
This equation underscores the stoichiometry of the reaction, pivotal for calculating the molarity and concentration of the FeSO4 solution.
The experiment utilized a standard solution of KMnO4, an FeSO4 solution of unknown concentration, a burette, a conical flask, and a white tile (to enhance color visibility).
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The KMnO4 solution, with a known molarity, served as the titrant, while the FeSO4 solution acted as the analyte.
The titration process was repeated multiple times to ensure accuracy, with the average volume of KMnO4 used to reach the endpoint meticulously calculated.
Utilizing the stoichiometry of the reaction and the known molarity of the KMnO4 solution, the molarity of the FeSO4 solution was determined to be 1.052 M. The concentration of the FeSO4 solution was subsequently calculated to be 160 g/L based on the molar mass of FeSO4.
MFeSO4=VFeSO4×NFeSO4MKMnO4×VKMnO4×NKMnO4
where MKMnO4 is the molarity of KMnO4, VKMnO4 is the volume of KMnO4 used, NKMnO4 and NFeSO4 are the stoichiometric coefficients, and VFeSO4 is the volume of FeSO4 titrated.
The experimental results closely align with the theoretical values, demonstrating the precision and accuracy of redox titration in determining the concentration of substances in solution. The slight discrepancies observed may be attributed to experimental errors such as imprecise measurement of volume or incomplete reaction at the endpoint. The consistency of the light pink color as an endpoint indicator underscores the importance of visual cues in titration experiments.
The successful determination of FeSO4's molarity and concentration not only validates the effectiveness of redox titration techniques but also emphasizes their significance in chemical analysis and quality control in various industries. Future experiments might explore the impact of different acid concentrations on the reaction rate and endpoint clarity, potentially refining the methodology for enhanced accuracy.
This comprehensive laboratory report on the redox titration of FeSO4 with KMnO4 elucidates the detailed procedure, results, and analytical implications of determining the molarity and concentration of an iron (II) sulfate solution. Through rigorous experimentation and stoichiometric calculations, the experiment achieved its objective, highlighting the efficacy of redox titration in quantitative chemical analysis. This study not only contributes to the foundational understanding of titration techniques but also offers a model for future investigations in the realm of analytical chemistry.
Quantitative Analysis of Iron (II) Sulfate Solution via Redox Titration. (2024, Feb 28). Retrieved from https://studymoose.com/document/quantitative-analysis-of-iron-ii-sulfate-solution-via-redox-titration
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