Why is there a need to immediately titrate the sample solution with the standard sodium thiosulfate solution after generating the iodine in the mixture?
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Q: Which of the following best describes the goal of an extraction procedure? a. the isolation of a…
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Q: Iodometric titration of vitamic C with sodium thiosulfate Why was the known excess of iodine…
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A: As per bartleby guidelines I answered only first question so please don't mind.Thanks in advance.
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Why is there a need to immediately titrate the sample solution with the standard sodium thiosulfate solution after generating the iodine in the mixture?
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- Why are many ionic precipitates washed with electrolyte solution instead of pure water?The NaOH titrant in this experiment was prepared to be approximately 0.1 M and then was standardized to determine its exact concentration. What possible reasons could there be for not simply weighing the solid NaOH, dissolving to a known volume and calculating its molarity?Write measurement of Carbon dioxide evolution during respiration of germinating seeds by the Titration method
- It is a solution of unknown concentration in which a solution of accurately known concentration is gradually added until the reaction is complete. Analyte Endpoint Indicator TitrantMention the types of volumetric titration and briefly point out their differences.An impure sample containing 2.00 g of sodium carbonate and bicarbonate was taken. It was dissolved in water and then crushed with hydrochloric acid (0.1 N). If the burette reading was at the end point of the phenolphthalein 7.5 ml and at the end of the orange methyl point was 20.0 ml. Calculate the ratio The percentage of sodium bicarbonate in the sample. Note that the molecular weight of sodium bicarbonate is 84 *
- For titration, what is the purpose of a dropwise rate?The chloride in the sample is to be determined gravimetrically by precipitating and weighing AgCl. What weight in grams of sample should be taken so that the percentage of Cl is obtained by simply multiplying the weight of the AgCl precipitate by 10?Q1)a) In the gravimetric analysis the precipitate should be free from impurities. Give the detailed justification for the above statement by identifying impurities. b) It is required to analyse the metal from its ore sample. Manganese (Mn)present in the ore sample was analysed by forming a precipitate of MnSO4. If 2.98 g of ore sample gives 0.19 g of MnSO4. Calculate the percentage of Mn present in the sample.
- A 50-mL solution of 0.5005 N standard NaOH was added to a 0.9250-g sample of Aspirin and was boiled for 10 minutes. After cooling a full pipet of phenolphthalein was added to the solution before it was titrated with 24.7 mL of 0.5015 N standard HCl solution until the disappearance of the pink color. The same procedure was carried using a blank which consumed 4.6 mL of the same standard acid. Calculate for the %Aspirin in the sample. Atom weights: C =12, H =1, O =16.Explain the importance of performing blank titration in a precipitation titration experiment.Suppose that extra volume (more than the actual volume) of 0.2 M NaOH solution was used to reach the end-point in the titration process for the determination of the % purity of aspirin sample (0.5 g). Which of the following is correct? The calculated and the actual percent purity values for the aspirin sample will be the same, since the extra added volume of NaOH solution has no effect on the % purity determination for the aspirin sample. We need to know the actual volume (the real volume that should be used in titration) as well as the used volume of NaOH solution to make a true comparison between the actual and the calculated % purity values for the aspirin sample. The calculated % purity value will be lower than the actual % purity value for the aspirin sample. The calculated % purity value will be higher than the actual % purity value for the aspirin sample.