2) A solution of I2 was standardized with ascorbic acid. The titration of a 10.00 mL...
2) A solution of I2 was standardized with ascorbic acid. The titration of a 10.00 mL aliquot of a stock solution made by dissolving 0.1050 g sample of pure ascorbic acid to a final volume of 100.00 mL required 25.32 mL of I2 to reach the starch end point
a. What is the molarity of the iodine solution?
b. How many mg ascorbic acid is required to react with 1.00 mL
iodine solution?
Homework Answers
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2) A solution of I2 was standardized with ascorbic acid. The
titration of a 10.00 mL...
16 7-2 Titration Calculations Ascorbic acid (vitamin C) reacts with according to the equation Starch is used as an i...
16 7-2 Titration Calculations Ascorbic acid (vitamin C) reacts with according to the equation Starch is used as an indicator in the reaction. The end point is marked by the appearance of a deep blue starch-iodine complex when the first fraction of a drop of unreacted remains in the solution. TI (a) Stundurdization: If 29.41 mL of iodine solution is required to react with 0.197 0 g of pure ascorbic acid, what is the molarity of the iodine solution?! (b)...
Vitamin C (ascorbic acid) from foods can be measured by titration with I3-If 29.41 mL of...
Vitamin C (ascorbic acid) from foods can be measured by titration with I3-If 29.41 mL of I3- solution are required to react with 0.1970 g of pure ascorbic acid, what is the molarity of the I3- solution? A vitamin C tablet containing ascorbic acid plus inert binder was ground to a powder, and 0.4242 g was titrated by 31.63 mL of I3-. How many moles of ascorbic acid are present in the 0.4242 g sample? Find the weight percent of...
I understand part a, I need help with B and C. Thanks! 6-B. Vitamin C (ascorbic...
I understand part a, I need help with B and C. Thanks!
6-B. Vitamin C (ascorbic acid) from foods can be measured by titration with 13: CH4O6 + + H2O = C,H,O + 30 + 2H Ascorbic acid Triiodide Dehydroascorbic acid FM 176.126 Starch is used as an indicator in the reaction. The end point is marked by the appearance of a deep blue starch-iodine complex when unreacted 15 is present. (a) If 29.41 mL of Iz solution are required...
A selection of commercial fruit juices and fruit extracts were analysed for ascorbic acid content. A...
A selection of commercial fruit juices and fruit extracts were analysed for ascorbic acid content. A student took kiwifruit juice to analyse. This juice is reputed to have ascorbic acid concentrations about 3 times greater than that of orange juice. The student diluted the juice by taking a 25.00 mL sample to a final volume of 100.0 mL. The student analysed 25.00 mL aliquots of the diluted juice solution for ascorbic acid by titration using a standardised iodine solution. Data:...
A vitamin C (ascorbic acid) tablet was dissolved in approximately 50 mL of distilled water and...
A vitamin C (ascorbic acid) tablet was dissolved in approximately 50 mL of distilled water and titrated with the standardized NAOH solution. From the results of this titration, the mg of ascorbic acid in the tablet was calculated. Molecular formula of ascorbic acid: C6H806 Volume of NaOH required to neutralize ascorbic acid in Vitamin C tablet (mL) 14.47 Concentration of NaOH in mol/L, 0.1964 Calculate the amount of ascorbic acid in the Vitamin C tablet in (mg). Answer:
Determination of Vitamin C Concentration by Redox Titration An alternative titration method for determining the concentration...
Determination of Vitamin C Concentration by Redox Titration An alternative titration method for determining the concentration of vitamin C in a sample is to use an iodine solution. In this reaction iodine oxidizes the ascorbic acid to C&H&O 2. A 20.00 ml sample of a 1.00 mg/mL vitamin C solution is placed in a flask along with 1 mL of a 1% starch solution to serve as an indicator. A dilute solution of iodine is placed in a buret. A...
An aqueous solution of hydrochloric acid is standardized by titration with a 0.113 M solution of...
An aqueous solution of hydrochloric acid is standardized by titration with a 0.113 M solution of calcium hydroxide. If 11.3 mL of base are required to neutralize 10.0 mL of the acid, what is the molarity of the hydrochloric acid solution? M hydrochloric acid An aqueous solution of calcium hydroxide is standardized by titration with a 0.101 M solution of hydrochloric acid. If 19.7 mL of base are required to neutralize 22.1 mL of the acid, what is the molarity...
An aqueous solution of hydroiodic acid is standardized by titration with a 0.123 M solution of...
An aqueous solution of hydroiodic acid is standardized by titration with a 0.123 M solution of calcium hydroxide. If 10.7 mL of base are required to neutralize 10.9 mL of the acid, what is the molarity of the hydroiodic acid solution? ____M hydroiodic acid An aqueous solution of barium hydroxide is standardized by titration with a 0.114 M solution of hydrobromic acid. If 27.6 mL of base are required to neutralize 27.9 mL of the acid, what is the molarity...
Standardization of Iodine Solution. i need help with the last 3 calculations for Moles, Molarity...
Standardization of Iodine Solution.
i need help with the last 3 calculations for Moles, Molarity
and Titer of I2.
Data and Calculations: Analysis for Vitamin C A. Standardization of lodine Solution Mass of Ascorbic Acid Sample, g Moles of Ascorbic Acid n = Sample 0.10qg max10-4 (MM = 176 g) Initial buret reading, mL Final buret reading, mL Volume of I2 added, mL Moles of I, consumed Molarity of I, moles/L Titer of I2, mg Asc/mL I2 41
Data and...
1a.An aqueous solution of perchloric acid is standardized by titration with a 0.177 M solution of...
1a.An aqueous solution of perchloric acid is standardized by titration with a 0.177 M solution of barium hydroxide. If 11.6 mL of base are required to neutralize 23.6 mL of the acid, what is the molarity of the perchloric acid solution? 1b.An aqueous solution of calcium hydroxide is standardized by titration with a 0.168 M solution of hydroiodic acid. If 28.6 mL of base are required to neutralize 20.7 mL of the acid, what is the molarity of the calcium...
16 7-2 Titration Calculations Ascorbic acid (vitamin C) reacts with according to the equation Starch is used as an indicator in the reaction. The end point is marked by the appearance of a deep blue starch-iodine complex when the first fraction of a drop of unreacted remains in the solution. TI (a) Stundurdization: If 29.41 mL of iodine solution is required to react with 0.197 0 g of pure ascorbic acid, what is the molarity of the iodine solution?! (b)...
I understand part a, I need help with B and C. Thanks!
6-B. Vitamin C (ascorbic acid) from foods can be measured by titration with 13: CH4O6 + + H2O = C,H,O + 30 + 2H Ascorbic acid Triiodide Dehydroascorbic acid FM 176.126 Starch is used as an indicator in the reaction. The end point is marked by the appearance of a deep blue starch-iodine complex when unreacted 15 is present. (a) If 29.41 mL of Iz solution are required...
A vitamin C (ascorbic acid) tablet was dissolved in approximately 50 mL of distilled water and titrated with the standardized NAOH solution. From the results of this titration, the mg of ascorbic acid in the tablet was calculated. Molecular formula of ascorbic acid: C6H806 Volume of NaOH required to neutralize ascorbic acid in Vitamin C tablet (mL) 14.47 Concentration of NaOH in mol/L, 0.1964 Calculate the amount of ascorbic acid in the Vitamin C tablet in (mg). Answer:
Determination of Vitamin C Concentration by Redox Titration An alternative titration method for determining the concentration of vitamin C in a sample is to use an iodine solution. In this reaction iodine oxidizes the ascorbic acid to C&H&O 2. A 20.00 ml sample of a 1.00 mg/mL vitamin C solution is placed in a flask along with 1 mL of a 1% starch solution to serve as an indicator. A dilute solution of iodine is placed in a buret. A...
An aqueous solution of hydrochloric acid is standardized by titration with a 0.113 M solution of calcium hydroxide. If 11.3 mL of base are required to neutralize 10.0 mL of the acid, what is the molarity of the hydrochloric acid solution? M hydrochloric acid An aqueous solution of calcium hydroxide is standardized by titration with a 0.101 M solution of hydrochloric acid. If 19.7 mL of base are required to neutralize 22.1 mL of the acid, what is the molarity...
Standardization of Iodine Solution.
i need help with the last 3 calculations for Moles, Molarity
and Titer of I2.
Data and Calculations: Analysis for Vitamin C A. Standardization of lodine Solution Mass of Ascorbic Acid Sample, g Moles of Ascorbic Acid n = Sample 0.10qg max10-4 (MM = 176 g) Initial buret reading, mL Final buret reading, mL Volume of I2 added, mL Moles of I, consumed Molarity of I, moles/L Titer of I2, mg Asc/mL I2 41
Data and...
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