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Why methyl orange is used instead of phenolphthalein in hcl and naoh titration?
This is so since the pH at the end point of Phenolphthalein is 9.1 and methyl orange is 3.7. For a strong acid strong base titration which the end point is between 3-11 phenolphthalein is used
Why do you use ethanolic NaOH instead of aq NaOH in titration?
Ethanolic NaOH is used instead of aqueous NaOH in titration to avoid side reactions with water and reduce error in the titration process. The absence of water in ethanolic NaOH helps maintain the concentration and stability of the solution, resulting in more accurate and precise titration results.
Why is phenolphthalein indicator not used in EDTA titration?
Phenolphthalein is not suitable for use in EDTA titration because it changes color at a pH range that is much lower than the pH range at which the EDTA-metal complex formation occurs. EDTA titration typically requires indicators that change color in a more acidic pH range.
Why is a back titration sometimes used for an analysis rather than a direct titration?
Back titrations are used when a reaction occurring in the conical flask can not be detected using an indicator such as phenolphthalein. So, after this titration has been performed, the 'excess' is then titrated with something that can be detected more easily using phenolphthalein etc.
How to calculated NaOH concentration be affected if the colour change in the solution is too dark?
I presume you are titrating a standardized solution of (eg) HCl with NaOH to determine the molarity of the alkali. You would normally use an indicator which will change colour at the end point (eg colourless to pink for phenolphthalein). If the solution is very coloured to begin with it can mask the colour change and so make the end point hard to see and lead to a miscalculation of molarity.
Why methyl orange is used instead of phenolphthalein in hcl and naoh titration?
This is so since the pH at the end point of Phenolphthalein is 9.1 and methyl orange is 3.7. For a strong acid strong base titration which the end point is between 3-11 phenolphthalein is used
Why do you use ethanolic NaOH instead of aq NaOH in titration?
Ethanolic NaOH is used instead of aqueous NaOH in titration to avoid side reactions with water and reduce error in the titration process. The absence of water in ethanolic NaOH helps maintain the concentration and stability of the solution, resulting in more accurate and precise titration results.
Why is phenolphthalein indicator not used in EDTA titration?
Phenolphthalein is not suitable for use in EDTA titration because it changes color at a pH range that is much lower than the pH range at which the EDTA-metal complex formation occurs. EDTA titration typically requires indicators that change color in a more acidic pH range.
How you determine the concentration of hcl of new bottle?
To determine the concentration of hydrochloric acid (HCl) in a new bottle, you can perform a titration using a standard solution of a strong base, such as sodium hydroxide (NaOH). First, you would dilute a known volume of HCl and then gradually add the NaOH solution until you reach the endpoint, indicated by a color change from a pH indicator like phenolphthalein. By applying the titration formula (M1V1 = M2V2), you can calculate the concentration of the HCl based on the volume and concentration of the NaOH used. Additionally, you could use techniques like pH measurement or conductometric titration for more precise results.
Why is a back titration sometimes used for an analysis rather than a direct titration?
Back titrations are used when a reaction occurring in the conical flask can not be detected using an indicator such as phenolphthalein. So, after this titration has been performed, the 'excess' is then titrated with something that can be detected more easily using phenolphthalein etc.
What will happen to the molarity of NaOH If a drop of NaOH falls out of the flask during the titration?
You have to realise that a drop from the burette for instance is insignificant, if you are dealing with at least 10ml solution which you usually deal with on a titration. If you don't want to regard it as insignificant, then if NaOH is in the burette, then the solution doesn't become more concentrated with NaOH because that drop escaped.
Why is titration method applicable in aspirin analysis?
When I am using back titration and direct titration as my two methods for determining the purity of aspirin tablets. doesn't the direct titration not take into consideration of the excess sodium hydroxide added to the aspirin?In both these titrations when I reach the end-point it turns pink but I kept these solution the next day and they turned back to colourless. Is this meant to happen and what chemical reaction has happened here?I titrated this again with more sodium hydroxide till the end-point then added this to the overall amount of NaOH i added in the flask.Is the only difference between back titration and direct titration not addding the HCl at the end to determine the excess amount of NaOH?Are there any methods for direct titration.Would really appreciate any help.The best you can obtain is an end point lasting 20-30 seconds. Any excess base will slowly hydrolyze the ester and liberate acetate ion from the act's because aspirin is such a weak acid that it reacts slowly with the NaOH, making it difficult to accurately get a good endpoint in a reasonable time.With back titration, you react with an excess of NaOH (known amount), heat it to make the reaction go to completion quickly, then use HCl to determine the amount of NaOH that is remaining. This reaction will go quickly, and is much easier to measure.elylsalicylic acid,aspirin.
How to calculated NaOH concentration be affected if the colour change in the solution is too dark?
I presume you are titrating a standardized solution of (eg) HCl with NaOH to determine the molarity of the alkali. You would normally use an indicator which will change colour at the end point (eg colourless to pink for phenolphthalein). If the solution is very coloured to begin with it can mask the colour change and so make the end point hard to see and lead to a miscalculation of molarity.
Why does an increase of NaOH indicate an increase of CO2?
An increase in NaOH consumption during a titration with CO2 indicates an increase in CO2 concentration because CO2 reacts with NaOH to form sodium carbonate. The greater the amount of CO2 present, the more NaOH will be consumed to neutralize it.
Why you use oxalate potassium in formol titration?
In formol titration, amino acids with formaldehyde are titrated with NaOH to measure the amount of amino acids in the solution. Potassium is also necessary for this titration and is supplied by using potassium oxalate. If calcium is present, it will react with the NaOH to form Ca(OH)2. This will make it appear to need more of the NaOH solution (and overestimate the titration). Potassium oxalate will chelate the calcium, and prevent it from reacting (forming calcium oxalate).
WHY IT IS NECESSARY TO DILUTE THE VINEGAR TITRATION WITH O.1 m naoh?
Diluting the vinegar in a titration with 0.1 M NaOH is necessary to ensure that the reaction occurs within a measurable and interpretable range. Vinegar, being an acetic acid solution, can have a high concentration that may lead to overshooting the endpoint if not diluted. This dilution allows for a more accurate determination of the acetic acid concentration by providing a clearer endpoint and reducing the potential for errors in measurement. Additionally, it helps in achieving a more gradual reaction, improving the precision of the titration results.
Which is more polar bromophenol blue or phenolphthalein?
Phenolphthalein is more polar than bromophenol blue due to its structure and functional groups. Phenolphthalein contains more oxygen atoms that can participate in hydrogen bonding, making it a more polar compound compared to bromophenol blue.
