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Changes color at the endpoint of titration?
The color change at the endpoint of a titration is due to the indicator used in the titration process. The indicator changes color based on the pH of the solution, signaling the completion of the reaction between the analyte and titrant. This color change helps determine the equivalence point of the titration.
Why would phenolpthalein not be a suitable indicator for the standardisation of hydrochloric acid with Borax?
Phenolphthalein is not suitable for titration involving Borax and hydrochloric acid because it changes color at a pH lower (usually around pH 8-9) than the equivalence point of this specific titration. Borax reacts as a weak base while hydrochloric acid is a strong acid, making the equivalence point acidic in nature. A suitable indicator would need to change color near this acidic pH of the equivalence point.
How could you determine whether phenolphthalein remains in the residue of a titration reaction?
The easiest way is to add back some of the solution you were titrating. If phenolphthalein remains, it will react with the solution and change back to purple. Incidentally, phenolphthalein will always remain in the solution of the titration reaction - it changes color depending upon the pH of the solution, but the indicator itself is not affected by the titration reaction.
Describe a method to visually detect the end point of a titration without the use of instruments?
The method used most often in chemistry labs is by use of a pH indicator in the sample being titrated. When you reach the titration point, the indicator will change colors, demonstrating the end point of the titration.
If the equivalence point of a titration is 5 what range of pH should the indicator be?
An indicator should have a pKa close to the expected pH at the equivalence point. For a titration with an equivalence point at pH 5, an indicator with a pKa in the range of 4 to 6 would be suitable for visual detection of the endpoint.
Why phenolphthalein cannot be used as an indicator for titrating a weak base against a strong acid?
Phenolphthalein is not suitable for this titration because its color change occurs over a pH range that is beyond the equivalence point of the weak base and strong acid titration. At the equivalence point of this titration, the solution is acidic, which is below phenolphthalein's color change pH range. This can lead to inaccurate results and difficulty in determining the endpoint of the titration.
What color will a solution be at the equivalence point of titration?
The color of a solution at the equivalence point of a titration depends on the type of indicator used. The indicator changes color at a specific pH value, signaling the completion of the reaction. Common indicators like phenolphthalein turn pink at the equivalence point of an acid-base titration.
Why phenolphthalein used as best indicator against NaOH?
Phenolphthalein is a suitable indicator for NaOH because it changes color sharply from colorless to pink at the pH range of 8.2 to 10.0, which corresponds well to the endpoint of the titration of NaOH with an acid. This sharp color change allows for accurate and precise detection of the equivalence point in the titration process.
Why does the pink color at the first equivalence point fade only gradually?
The pink color at the first equivalence point in a titration involving phenolphthalein fades gradually because the solution is in a buffer region. At the equivalence point, there is a mix of weak acid and its conjugate base, which causes the pink color to fade slowly as the pH changes only slightly during the titration.
What is the purpose of adding phenolphthalein during titration?
Phenolphthalein is added as an indicator during titration to visually indicate the endpoint of the reaction. It changes color at a specific pH, usually from colorless to pink, which helps the titrator determine when the reaction is complete and the equivalence point has been reached.
What color indicates that a titration using phenolphthalein has reached the end point?
The color pink indicates that a titration using phenolphthalein has reached the end point.
Why phenolphthalein is chosen as the suitable indicator for sodium hydroxide?
Phenolphthalein is chosen as a suitable indicator for sodium hydroxide because its color change occurs in the pH range around 8.2 to 10.0, which is close to the pH range of the equivalence point for the titration of a strong base like sodium hydroxide with a strong acid. This allows for a sharp and easily detectable color change at the endpoint of the titration.
Why you use phenolphethalein indicator in titration?
Phenolphthalein is used as an indicator in titrations to visualize the endpoint of an acid-base titration. It changes color from colorless to pink in a basic solution, indicating the completion of the reaction between the acid and base. This change is easily detectable and helps to accurately determine the equivalence point of the titration.
What is the difference between end point titration and equivalence point?
Endpoint titration refers to the point in a titration where the indicator changes color, signaling that the reaction is complete. Equivalence point, on the other hand, is the point in the titration where the moles of the titrant are stoichiometrically equal to the moles of the analyte. The equivalence point does not necessarily coincide with the endpoint, as the indicator may change color before or after reaching the equivalence point.
Is methylorange the indicator used in the titration of Na2CO3 against HCl solution?
Methyl orange is not commonly used as an indicator in the titration of Na2CO3 against HCl solution. Phenolphthalein is a suitable indicator for this titration because it changes color in the pH range of the equivalence point.
What is the function of phenolphthalein in titration?
Phenolphthalein is a pH indicator commonly used in acid-base titrations. It changes color in a specific pH range (around pH 8.2 to 10), allowing the endpoint of the titration to be visually determined. This makes it easier to accurately measure the amount of titrant required to reach the equivalence point.
Changes color at the endpoint of titration?
The color change at the endpoint of a titration is due to the indicator used in the titration process. The indicator changes color based on the pH of the solution, signaling the completion of the reaction between the analyte and titrant. This color change helps determine the equivalence point of the titration.
