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Which indicator is used for the titration of weak acid and strong base?
Phenolphthalein is commonly used as the indicator for the titration of a weak acid and a strong base. It changes color from colorless to pink at the equivalence point of the titration when the weak acid is completely neutralized by the strong base.
Which indicator is used in titration for strong acid?
For the titration of a strong acid, the indicator typically used is phenolphthalein. Phenolphthalein changes color in the pH range of 8.2 to 10, which is suitable for titrating a strong acid with a strong base to determine the equivalence point.
What criterion is used in selecting an indicator for a particular acid-base titration?
The key criterion for selecting an indicator for an acid-base titration is that the indicator's color change should occur close to the equivalence point of the titration. This ensures that the indicator accurately signals when the reaction is complete. The pH range over which the indicator changes color should match the pH range around the equivalence point.
What indicator can you choose for the titration of oxalic acid with sodium hydroxide?
Phenolphthalein is a suitable indicator for the titration of oxalic acid with sodium hydroxide. It changes color from colorless to pink at the endpoint of the titration when the acid has been completely neutralized.
What are the best indicator use in titration of weak base against strong acid?
The best indicator to use in the titration of a weak base against a strong acid is phenolphthalein. Phenolphthalein changes color from colorless to pink at a pH range of about 8.2 to 10.0, which is suitable for detecting the endpoint of the titration when the weak base is completely neutralized by the strong acid.
Which indicator is used for the titration of weak acid and strong base?
Phenolphthalein is commonly used as the indicator for the titration of a weak acid and a strong base. It changes color from colorless to pink at the equivalence point of the titration when the weak acid is completely neutralized by the strong base.
Which indicator is used in titration for strong acid?
For the titration of a strong acid, the indicator typically used is phenolphthalein. Phenolphthalein changes color in the pH range of 8.2 to 10, which is suitable for titrating a strong acid with a strong base to determine the equivalence point.
What criterion is used in selecting an indicator for a particular acid-base titration?
The key criterion for selecting an indicator for an acid-base titration is that the indicator's color change should occur close to the equivalence point of the titration. This ensures that the indicator accurately signals when the reaction is complete. The pH range over which the indicator changes color should match the pH range around the equivalence point.
What indicator can you choose for the titration of oxalic acid with sodium hydroxide?
Phenolphthalein is a suitable indicator for the titration of oxalic acid with sodium hydroxide. It changes color from colorless to pink at the endpoint of the titration when the acid has been completely neutralized.
What are the best indicator use in titration of weak base against strong acid?
The best indicator to use in the titration of a weak base against a strong acid is phenolphthalein. Phenolphthalein changes color from colorless to pink at a pH range of about 8.2 to 10.0, which is suitable for detecting the endpoint of the titration when the weak base is completely neutralized by the strong acid.
Which indicator would you use in the titration sulphuric acid with naoh?
In the titration of sulfuric acid with sodium hydroxide (NaOH), a pH indicator suitable for a strong acid-strong base titration, such as phenolphthalein, can be used. Phenolphthalein changes color at around pH 8.2-10, which is suitable for detecting the endpoint of the neutralization reaction between sulfuric acid and sodium hydroxide.
What is the equation of titration with methyl orange?
The equation of the titration using methyl orange as an indicator depends on the specific reaction being titrated. Methyl orange is typically used in acid-base titrations, where the indicator changes color in the presence of a certain pH range. For example, in a titration of a strong acid (e.g., HCl) with a strong base (e.g., NaOH), the equation would involve the stoichiometry of the acid-base reaction, with the color change of methyl orange indicating the endpoint of the titration.
What is phenolphthalein used in titration labs?
Phenolphtalein is an indicator used to find the endpoint of a reaction (specifically an acid-base reaction). It has a pH range of 8.3 to 10.0 which means it can be used for a strong acid to strong base titration or a weak base to strong acid titration. Phenolphthalein is clear when it is in the presence of acid and pink when it is in the presence of a base.
Why is phenolpthalein used as the indicator for the assay of tartaric acid?
Phenolphthalein is used as an indicator during the titration of tartaric acid because the pH at which phenolphthalein changes color (around pH 8.2-10) is close to the equivalence point of the titration of tartaric acid with a strong base like NaOH. This makes it a suitable indicator for detecting the endpoint of the titration when the acid has been completely neutralized by the base.
In HCl and NaOH titration which indicator is used?
Phenolphthalein is commonly used as an indicator in the titration of hydrochloric acid (HCl) with sodium hydroxide (NaOH). Phenolphthalein changes color from colorless to pink at the endpoint of the titration when all the acid has been neutralized by the base.
Why phenolphtalein is use in titration of strong acid against strong base?
Phenolphthalein is used as an indicator in the titration of a strong acid and a strong base because its color transition occurs within a suitable pH range for this type of titration (pH 8.3-10.0). It changes from colorless in acidic solutions to pink in basic solutions, making it easy to observe the endpoint when the acid-base reaction is complete.
What colorimetric pH indicator should you use for ammonia and hydrochloric acid titration?
Since the titration is between a strong acid and a weak base, methylorange should be suitable as the equivalence point is around pH 5. The K of the indicator should be equal to the pH at the end point. Methyl orange is that indicator
