0
An indicator shows when we have added just enough of the second reagent to react with the first. If you mean why do we add only a small amount of indicator, it is to keep the answer accurate. Some of the reagent is used changing the indicator so the answer is always slightly bigger than perfection, and the more indicator you add, the larger the error.
Wiki User
∙ 6y ago
Wiki User
∙ 6y agoIt is a pH indcator to identify the end of the reaction.
Add your answer:
Earn +20 pts
How half titration could be done using only an indicator solution without PH?
In a half titration, you can use an indicator solution without needing to measure pH by adding the indicator directly to the reacting mixture and observing the color change. This can help you identify the endpoint of the titration, where half of the analyte has been neutralized. The color change will indicate the completion of the reaction, signaling that half of the titrant has been added.
What is the chemical process for back titration?
In back titration, a known excess of a reagent is added to react with the analyte. After the reaction is complete, the amount of excess reagent is determined by titration with another reagent. The difference between the initial amount of excess reagent and the amount required in the back titration is used to determine the amount of analyte present.
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.
Why KI is added in redox iodometric titration even in the presence of sodium thiosulfate as a reducing agent?
KI is added in redox iodometric titration as an indicator because it reacts with iodine formed during the titration to form a starch-iodine complex, which gives a blue color. This color change helps detect the endpoint of the titration accurately. Sodium thiosulfate is used to titrate the excess iodine after the reaction with the analyte is complete.
Why potassium thiocyanate is added in redox iodometric titration of copper sulphate?
Potassium thiocyanate is added to the redox iodometric titration of copper sulfate to react with the excess iodine produced during the reaction. This reaction forms a stable product, potassium iodide, which helps reach the correct endpoint of the titration by preventing the iodine from reacting with other substances. It also helps improve the accuracy and precision of the titration results.
Is the indicator generally added to the titrant or analyte in a titration?
Analyte is the indicator that is generally added in titration.
Is the indicator generally added to the titrant or the analyte in titration?
Analyte is the indicator that is generally added in titration.
Is the indicator generally added to the titrant or the analyte in a titration?
The indicator is typically added to the analyte in a titration. It helps to visually signal the endpoint of the titration by changing color as the reaction progresses.
What is an indicator in an acid base titration?
An indicator is a substance that changes color in response to a change in pH during an acid-base titration. It is used to signal the endpoint of the titration when the amount of acid or base added is stoichiometrically equivalent to the amount of the other reactant. Common indicators include phenolphthalein, methyl orange, and bromothymol blue.
What is meant by the end point during a titration?
The end point in a titration is when the indicator used changes color, signaling that the reaction is complete. It indicates that the stoichiometric amount of titrant has been added to react completely with the analyte.
What is end point of titration?
The endpoint of a titration is when an indicator changes color, or a measurable physical change occurs, indicating that the reaction has reached its completion. This signals that the amount of titrant added is stoichiometrically equivalent to the amount of analyte present in the sample.
Why is the indicator not added to the titration flask at the begging of the iodomettic titration?
Adding the indicator at the beginning of the iodometric titration can react with the iodine present, which can lead to errors in the titration results. By adding the indicator after most of the iodine has reacted, it ensures that the endpoint is more accurate and reliable.
Why you add starch at the end of titration?
Starch is added at the end of titration as an indicator to signal the endpoint of the reaction. It forms a complex with the iodine produced during the titration, resulting in a color change from clear to blue-black, indicating that the titration is complete.
Why are indicators used in drops in titration?
Indicators are used in drops during titration to detect the endpoint of the reaction, which is when the reaction has reached completion. The indicator changes color when the pH of the solution changes, indicating that the correct stoichiometric amount of titrant has been added to the solution being titrated.
What is the difference between the end point in a titration and the equivalence point?
The end point in a titration is when the indicator changes color, signaling that the reaction is close to completion. The equivalence point, on the other hand, is the point at which the amount of added titrant is stoichiometrically equivalent to the amount of analyte in the sample, regardless of indicator color change.
What is the color of the indicator when an excess of hydrochloric acid has been added?
The indicator turns pink when an excess of hydrochloric acid has been added in a titration.
What is the difference between equivalent point and end point in analytical chemistry?
The equivalence point is the point in a titration when the amount of added standard reagent is chemically equal to the amount of analyte. The end point is the point in a titration when a physical change occurring immediate after the equivalence point
