Why is it necessary to standardize a indophenol solution?
Why is it necessary to titrate blank samples?
Why might the Vitamin C content be underestimated in the case of a heat processed juice sample?
Standardization is doing a titration to work out the exact concentration of the solution you want to use to determine the concentration of an unknown solution.
A problem with indolphenol is that it can be easily reduced, and the purity of the compound cannot be readily reproduced or estimation. It is important to estimate the concentration of an indolphenol by titration with known concentration of a vitamin C solution. This procedure is called standardization.
Once the indophenol concentration is established or standardized, this can be used to determine the concentration of Vitamin C in unknown solutions. Chemically, vitamin C is a reducing agent and a weak acid, The reaction between vitamin C and indolphenol bleaches indolphenol, and the color of the reaction mixture can be used to detect the end point of the titration and the concentration of Vitamin C can be established.
Vitamin C content might be underestimated in heat processed samples because it decays upon heating in solution state. Over a period of time the the concentration decreases leading to underestimation.
A blank titration is carried out to nullify the error that may arise during analysing the samples. This is generally performed by titrating a fixed and known concentration of titrant into a solvent with zero analyte.This allows the amount of reactive substance within the plain solvent to be determined and the correction factor can be applied during calculations as required
Why is it necessary to standardize a indophenol solution? Why is it necessary to titrate blank...
Why is it necessary to standardize a indophenol solution? Why is it necessary to titrate blank samples? Why might the Vitamin C content be underestimated in the case of a heat processed juice sample?
A sample of pure NaCl can be used to standardize a solution of AgNO3 using the procedure performed in lab using the formation of Ag2CrO4 as an indicator. 32.71 mL of the AgNO3 titrant was required to titrate a 0.2012g sample of NaCl. What is the concentration of the AgNO3 titrant.?
Why is it important to standardize the base in our experiment before titrating it with vitamin C?
2. (5 pts) You perform an acid-base titration to standardize an HCl solution by placing 50.00 mL of 0.100M HCI in a flask with a few drops of indicator solution. You put 0.1292 M Ba(OH)2 into the buret, how many mL of the Ba(OH)2 are necessary to titrate the HCI?
A titration was performed to standardize an EDTA solution. a) A 25.00 mL aliquot of a standard solution containing 0.01500 M Ca2+ required 42.87 mL of EDTA to reach the endpoint. The molarity of the EDTA solution is: ________ M b) That same EDTA solution was then used to titrate an unknown hard water sample. A 40.00 mL aliquot of unknown hard water required 34.21 mL of EDTA solution to reach a distinct endpoint. The concentration of Ca2+ ions (assuming...
chemistry
1. Your boss asks you to prepare and then standardize a sodium hydroxide solution, which you do as you did in this lab. The average concentration is 0.1063M. He then hands you a solution of nitric acid and asks you to titrate it with your NaOH solution. It requires 27.33mL of your tandardized NaOH solution to titrate 24.79mL of the nitric acid solution. Write a chemical quation for the neutralization reaction and then calculate the molarity of the nitric...
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As part of Lab 11 you will make and standardize a solution of NaOH(aq). Suppose in the lab you measure the solid NaOH and dissolve it into 100.0 mL of water. You then measure 0.1993 g of KHP (204.22 g/mol) and place it in a clean, dry 100-mL beaker, and then dissolve the KHP in about 25 mL of water and add a couple of drops of phenolphthalein indicator. You titrate this with your NaOH(aq) solution and find that the...
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