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What is the difference between iodometric titration and iodimetric titration?
Iodometric titration involves the titration of iodine with a reducing agent, while iodimetric titration involves the titration of iodide with an oxidizing agent. In iodometric titration, iodine is detected by a starch indicator to determine the end point, while in iodimetric titration, iodide ion concentration is determined by titration with a standard solution of an oxidizing agent.
Why you do not use H2SO4 in iodometric titration?
Using H2SO4 in iodometric titration can lead to the formation of H2O2, which interferes with the reaction. It can also oxidize iodide ions prematurely, affecting the accuracy of the titration. Therefore, a different acid like HCl is typically used in iodometric titration.
Why the amount of potassium iodide to potassium iodateV does not affect the iodine liberated in iodometric titration?
The amount of potassium iodide does not affect the iodine liberated because potassium iodide is used as a reducing agent in the reaction, converting iodate to iodine. The stoichiometry of the reaction ensures that the amount of iodine liberated is solely determined by the initial amount of iodate present, not the amount of potassium iodide added.
Why potassium iodide added in excess?
Potassium iodide is added in excess in order to ensure that all available iodine is converted to iodide ions, which are then neutralized by thiosulfate ions in the back-titration method for determining the concentration of oxidizing agents, such as in the iodometric method. This ensures accurate and precise results by guaranteeing the complete reaction of all the iodine formed in the titration.
Why is potassium iodide used in iodometric titrations instead of sodium iodide?
I would guess that this is so because of potassium's mass, being much more than, sodium's molar mass per ion. So can sodium iodide be used instead of potassium iodide? Perhaps, but maybe not to the same level effectiveness. Potassium molecules have been known to dissolve better than sodium molecules. One example is Potassium Chloride and Sodium Chloride thanks
Does the amount of potassium iodide added to the potassium iodate solution affect the amounts of iodine liberated in iodometric titration?
Yes, the amount of potassium iodide added to the potassium iodate solution in iodometric titration affects the amount of iodine liberated. Potassium iodide serves as a reducing agent, reacting with the iodate ion to form iodine. The quantity of potassium iodide added determines the rate and completeness of this reaction, impacting the amount of liberated iodine available for titration.
What is the difference between iodometric titration and iodimetric titration?
Iodometric titration involves the titration of iodine with a reducing agent, while iodimetric titration involves the titration of iodide with an oxidizing agent. In iodometric titration, iodine is detected by a starch indicator to determine the end point, while in iodimetric titration, iodide ion concentration is determined by titration with a standard solution of an oxidizing agent.
Why you do not use H2SO4 in iodometric titration?
Using H2SO4 in iodometric titration can lead to the formation of H2O2, which interferes with the reaction. It can also oxidize iodide ions prematurely, affecting the accuracy of the titration. Therefore, a different acid like HCl is typically used in iodometric titration.
Why the amount of potassium iodide to potassium iodateV does not affect the iodine liberated in iodometric titration?
The amount of potassium iodide does not affect the iodine liberated because potassium iodide is used as a reducing agent in the reaction, converting iodate to iodine. The stoichiometry of the reaction ensures that the amount of iodine liberated is solely determined by the initial amount of iodate present, not the amount of potassium iodide added.
Why potassium iodide added in excess?
Potassium iodide is added in excess in order to ensure that all available iodine is converted to iodide ions, which are then neutralized by thiosulfate ions in the back-titration method for determining the concentration of oxidizing agents, such as in the iodometric method. This ensures accurate and precise results by guaranteeing the complete reaction of all the iodine formed in the titration.
Why is potassium iodide used in iodometric titrations instead of sodium iodide?
I would guess that this is so because of potassium's mass, being much more than, sodium's molar mass per ion. So can sodium iodide be used instead of potassium iodide? Perhaps, but maybe not to the same level effectiveness. Potassium molecules have been known to dissolve better than sodium molecules. One example is Potassium Chloride and Sodium Chloride thanks
Why is not possible to determine iodide by mohr titration?
Iodide cannot be determined by Mohr titration because it does not form a precipitate with silver nitrate. Mohr titration relies on the formation of a colored precipitate to indicate the end point, which is not observed in the case of iodide ions. Other methods, such as iodometric titration or spectrophotometry, are used to determine iodide ions quantitatively.
Why potassium iodate is added to potassium iodide in iodometry titration?
Iodometric titration means the titration of triiodide. Preparation of triiodide can be prepared by adding solid iodine to excess potassium iodide, however since iodine sublimes it is more difficult to weigh than potassium iodate. The triiodide would then need to be standardized with primary standard grade arsenious oxide. A better way is to weigh potassium iodate and add to a small excess of potassium iodide. The two ions (iodide and iodate) will also form the needed triiodide in an acidic environment. If the reagent is made fresh this way it can be used to standardize thiosulfate. Iodide iodate of known normality can also be used to titrate unknown concentrations of sulfite. For example, steam boiler treatment applications.
Why add excess KI in iodometric titration?
Excess KI is added in iodometric titration to ensure that all the oxidizing agent (e.g., H2O2, Cl2) has reacted with the iodide ions (I-) present in the solution. This ensures complete reaction and accurate determination of the analyte concentration. The excess iodide ions also help prevent the oxidation of iodide to iodine by atmospheric oxygen, which can interfere with the titration.
Effect of oxidizing agents on iodometric titration?
Oxidizing agents can interfere with iodometric titration by oxidizing iodide ions to iodine prematurely, leading to an inaccurate measurement of the analyte's concentration. This interference can be minimized by adding a reducing agent to the titration solution to consume any excess oxidizing agent before reacting with the iodide ions. Additionally, careful selection of the titration conditions and proper sample preparation can help mitigate the effect of oxidizing agents on the titration results.
What is iodometric titration?
In this titration iodine is liberated ....Added:... from (excess of) iodide by an oxidant. The Iodine is then titrated with thio (di-sodium thio-sulfate) and starch as indicator added just before the expected equivalence point.
Why you use iodine in iodometric titration?
Iodine is used in iodometric titration as the titrant because it can easily react with reducing agents to form iodide ions. Its reaction with reducing agents leads to a change in color, making it useful for visual endpoint detection. This allows for the determination of the concentration of the reducing agent being analyzed in the titration process.
