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Iodide can be oxidized by an atom in its most highly oxidized form, which releases iodine gas, which can be volumetrically quantified by iodometric titration using hypo. Pb+2. Iodide cannot be oxidized to I2 in the lowest possible oxidation state.
Who is unable to perform an iodometric titration?
Which one of the following is not capable of giving an iodometric titration? The correct answer is choice ‘A’: a) Fe3, b) Cu2 c) Pb2 d) Ag
Which of these methods is capable of iodometric titration?
A starch solution is utilized as an indicator in an iodometric titration because of its ability to absorb the I2 that is emitted throughout the process. As a result of this absorption, the solution’s color will shift from a dark blue to a pale yellow when it is titrated with a solution that has had its thiosulfate concentration standardised.
Why is the Karl Fisher constant (KI) employed in iodometric titration?
Iodometric titration requires the use of potassium iodide, often known as KI, because iodide can be converted to iodine when it is in the presence of an oxidizing agent.
The iodometric titration requires the use of which of the following reagents?
In the laboratory, the iodometric titration is carried out using sodium thiosulfate as the reagent.
Which one of the following does not have the capability to give iodometric titrations?
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What exactly is the fundamental idea behind iodometric titration?
The determination of the concentration of an oxidizing agent in solution is the fundamental principle underlying iodometric titration. [Clarification needed] Iodometry is performed by doing an indirect titration of the iodine that has been released as a result of the reaction with the analyte.A starch solution is utilized as an indicator in an iodometric titration because of its ability to absorb the I2 that is emitted throughout the process.
While performing an iodometric titration, why do we add hydrogen sulfide?
In the procedure of redox titration, sulphuric acid (H2SO4) is utilized since it contributes the H+ ions that are required for the reaction to proceed more rapidly, whereas the sulphate-bearing ions scarcely react at all over the course of the reaction…. Because of this, sulfuric acid is added to the solution in order to make it acidic.
Why is the starch solution not introduced until after the titration has been completed?
Because the Starch-Iodide combination is not very soluble in water, the starch is introduced to an iodine titration near the endpoint, when the quantity of iodine is low…. This avoids errors that could have occurred as a result of the possibility that some iodine would stay adsorbed on the complex despite being tested for.
Why does the iodine solution need to be stored in the dark?
Before beginning the titration procedure, the reaction mixture should be kept in the dark. This is because light speeds up a side reaction in which iodide ions are converted to iodine by atmospheric oxygen.
What is the correct representation of sodium thiosulfate in a chemical equation?
The chemical formula for the inorganic compound known as sodium thiosulfate (sometimes spelled sodium thiosulphate) is Na2S2O3.xH2O. In most cases, it is sold in the form of the colorless pentahydrate, denoted by the formula Na2S2O35H2O. The solid is a crystalline substance that dissolves very easily in water. It is efflorescent, which means it loses water easily.
In the process of titration, which indicator is utilized?
One of the most typical indicators for use in acid and base titration is phenolphthalein.
When doing the titration, why do we use a solution containing 0.025 N sodium thiosulfate?
hydroxide will generate a mixture of higher oxides, which will have a brownish color. These higher oxides, when acidified in the presence of an iodide, will release iodine in an amount that is chemically comparable to the oxygen content of the water sample. The newly available iodine is subsequently titrated using a reference solution consisting of sodium thiosulfate.
In iodine titration, which indicator is most commonly used?
Starch is the indicator that is typically selected for titrations that involve iodine (triiodide). When combined with iodine, starch produces a dark blue complex. Iodimetry comes to a close at the point where there is an abrupt transition from red to blue.
Iodine and iodide seem to be used interchangeably, but what’s the difference?
Iodine can exist in two different states: as the elemental diatomic iodine (I2) and as the ionic monoatomic iodide (I-). Iodide, denoted by the symbol I, is almost the only form that can be found in nature. Iodide is the ionic state of iodine, which is produced when iodine combines with another element to form a salt, such potassium. Iodine can also exist in the molecular state.
Is it possible to mix iodine solution with water?
Nevertheless, iodine does not dissolve in water, but it does dissolve easily in chloroform and hexane…. Iodine molecules that are non-polar cannot dissolve in water, but when they interact with iodide ions, they produce triiodide ions, which are soluble in water.
Why does mixing iodine with starch result in a blue color?
In the presence of iodine, a dark blue color is produced as a result of the reaction between amylose in starch and the iodine. The molecule of iodine manages to squeeze its way within the amylose coil… An vivid blue-black hue is produced as a result of this process, which results in the formation of a linear triiodide ion complex that is soluble and which slips into the coil of the starch.
Is a starch solution capable of acting as an indicator?
A solution of starch is frequently utilized as an indicator for the purpose of determining the presence of iodine. A dark blue starch-iodine complex is produced whenever starch and iodine are in the same location at the same time.
When does the titration come to an end?
During a titration, the end point is the point at which an indicator demonstrates that the quantity of reactant required for a successful completion of the reaction has been added to a solution.
Why isn’t feso4 used in the titration process?
When dissolved in water to generate a solution, FeSO4 is particularly prone to the oxidation that leads to the formation of Fe2(SO4)3. The titration requires the conversion of Fe2+ to Fe3+, and because of this conversion, an inaccuracy in the determination will be produced.
Why isn’t hno3 used in the titration process?
This titration makes use of diluted sulphuric acid as the acid that is being measured. Hydrochloric acid is typically avoided because, according to the equation given below, it reacts with KMnO4 to produce chlorine, which is also an oxidizing agent in the aqueous solution. Nitric acid is not used because it is itself an oxidizing agent, and hydrochloric acid is typically avoided because it reacts with KMnO4 to produce chlorine.
Before doing a titration, oxalic acid is heated; why is this done?
Answer : We heat oxalic acid solution because without heating it is a slow process as an energy greater than the activation energy is required for a reaction. Hence, in order to raise the amount of available energy, the temperature needs to be raised, which can only be accomplished by heating the oxalic acid solution.
What is the role of sodium thiosulfate in iodometric titration?
One can perform a titration of the iodine solution against the sodium thiosulfate solution, which has a color that is similar to a golden brown. After placing the sodium thiosulfate solution in the burette, it is transferred to the conical flask, where it has a reaction with the iodine and causes the solution’s color to become less vibrant.
In the titration of oxalic acid Naoh, which indicator is most commonly used?
Hence, phenolphthalein is the indicator that is utilized during the process of titrating oxalic acid with sodium hydroxide.
Iodine and sodium thiosulfate—what kind of a reaction do they have?
Prior to the iodine being able to mix with the starch and produce the distinctive blue-black color, sodium thiosulfate is utilized in order to convert the iodine back into iodide. After all of the thiosulfate has been used up, the iodine may combine with the starch to form a complex.