Answered: Why is a titrant of very low…

Why is a titrant of very low concentration (0.002 M) used in this experiment? The experiment is the Determination of Vitamin C by Redox Titration.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter11: Solutions

Section: Chapter Questions

Problem 36P

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Why is a titrant of very low concentration (0.002 M) used in this experiment? The experiment is the Determination of Vitamin C by Redox Titration.

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Why do we use sodium hydroxide instead of a weaker base? What is the practical reason for the use of a strong base rather than something like sodium bicarbonate?
In the titration calculation, moles of KOH were calculated from the known molarity and measured volume. Reaction stoichiometry was then used to convert that to moles of succinic acid. At this point, how could the moles of succinic acid be converted to a mass of succinic acid rather than a concentration?
What happens when a non-standard titrant is used in the titration of an unknown sample?a - The volume of the acid used will not be accurate.b - The normality of the acid used will not be accurate.c - The weight of the analyte will not be accurate.d - It will not matter.
A 20 ml sample of water from the Taal lake was brought to the laboratory for analysis. The dissolved oxygen (DO) was calculated to be 10.5 mg/L when titrated with .035 N NażS2O3. How much (in mL) of the titrant was used? 0.075 1.075 0.75 1.75
Which of the statements given below is correct? A. Iodometry is a method in which 12 solution is used as a titrant and the substances that can reduce iodine to iodine can be determined. B. Starch indicator is added to the medium at the beginning of the titration. C. All metal salts other than alkali salts dissolved in water cause hardness properties. D. 1 German hardness is the hardness of water containing cation equivalent to 1 mg CaCO3 per 100 mL.
Suppose the concentration of the NaOH solution was 0.5 M instead of 0.1 M. Would this titration have required more, less, or the same amount of NaOH solution for a complete reaction? Suppose you used 0.5 M NaOH to titrate your vinegar sample instead of 0.1 M. What effect does the concentration of base added have on the reliability of the results of your titration? Consider a 0.238 M aqueous solution of sodium hydroxide, NaOH, How many individual hydroxide ions (OH−) are found in 23.46 mL and How many moles of sulfuric acid, H2SO4, are neutralized by 23.46 mL of 0.238 M NaOH(aq)? [Hint: begin by writing a balanced equation for this neutralization reaction.]
An HCl solution was titrated to determine its concentration using 15.00 mL 0.02500 M sodium carbonate standard solution. It required exactly 20.000 mL acid to completely neutralize the reaction between the titrant and analyte. What is the concentration of HCl solution? a 0.06667 M b 0.03750 M c 0.01875 M d 0.03333 M
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?
A student did not read the directions to the experiment properly and mixed up where to put the NaOH and the HCl solutions. He put the HCl in the buret and the NaOH in the flask. He then added a drop of phenolphthalein to the solution in the flask. Does the student need to empty out all of the solutions and start over again or can he go ahead and run the titration? Explain
Two 24.91 ml samples of apple juice were analyzed using 0.1000 M NAOH solution by the method in this experiment. The corrected mean titration volume of the NaOH solution was 15.87 mL. Calculate the malic acid concentration of the apple juice in units of g/L. Assume that only malic acid is present in the juice. State the value to 2 places after the decimal point, Do not enter units.
The results of a titration experiment were as follows: Volume of aqueous NaOH pipetted into the conical flask = 10.00 mL Average volume of dilute HCI added from the burette to reach the endpoint = 12.54 mL Molarity of the dilute HCI = 1.196 M i) Write the chemical reaction equation for the titration reaction ii) Calculate the number of moles of HCI added during the titration iii) What is the number of moles of NaOH that has reacted during the titration iv) What is the molarity of the aqueous NaOH
Why is it all right to use a wet flask or to use water during the titration?