Exercise# 1 Calculation of ascorbic acid in Vitamin C tablet: (i) Starch is used as an indicator: starch + I; → starch-I; complex (deep blue) (clear) (ii) Titrate ascorbic acid with I;: но он но но, + 31 + 211* + lj + H,0 HOl. HO, но ascorbic acid (FW 176.124) dehydroascorbic acid (FW 192,124) 1 mole ascorbic acid → 1 mole I; Standardization of Titrant Followed by Analysis of Unknown OStandardization: Suppose 29.41 mL of I;' solution is required to react with 0.1970 g of pure ascorbic acid, what is the Molarity of the I; solution? DAnalysis of Unknown: A vitamin C tablet containing ascorbic acid plus an inert binder was ground to a powder, and 0.4242g was titrated by 31.63 mL of I;. Find the weight percent of ascorbic acid in the tablet.

Exercise# 1 Calculation of ascorbic acid in Vitamin C tablet: (i) Starch is used as an indicator: starch + I; → starch-I; complex (deep blue) (clear) (ii) Titrate ascorbic acid with I;: но он но но, + 31 + 211* + lj + H,0 HOl. HO, но ascorbic acid (FW 176.124) dehydroascorbic acid (FW 192,124) 1 mole ascorbic acid → 1 mole I; Standardization of Titrant Followed by Analysis of Unknown OStandardization: Suppose 29.41 mL of I;' solution is required to react with 0.1970 g of pure ascorbic acid, what is the Molarity of the I; solution? DAnalysis of Unknown: A vitamin C tablet containing ascorbic acid plus an inert binder was ground to a powder, and 0.4242g was titrated by 31.63 mL of I;. Find the weight percent of ascorbic acid in the tablet.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Practice5: Standard solution of Na2CO3 was prepared by dissolving 0.53 g in 100 ml of water. Then 10 ml of this solution requires 9 ml of HCl for titration. Later 10 ml of unknown NaOH solution require 8 ml of same HCl for titration. Calculate strength of unknown NaOH solution in g/lit.
None
Purpose Hypothesis Evidence Analysis Evaluation What is the mass of precipitate formed when 3.43g of barium hydroxide in solution reacts with an excess of sulphuric acid? Calculate the theoretical yield of barium sulphate • A white precipitate formed when the barium hydroxide solution was mixed with the sulphuric acid. • Mass of filter paper = 0.96 g• Mass of filter paper and precipitate = 5.25 g What is the mass of precipitate formed when 3.43g of barium hydroxide in solution reacts with an excess of sulphuric acid? What is the percentage yield of this reaction? What is your hypothesis, analysis, and evaluation section?
QUESTION 4 What is the Ksp for iron (II) sulfide if the iron (II) concentration in a saturated solution is 1.6863E-2 M?
Exercise 20.78 11 of 18 Constants Periodio. Table Part A For the hall-reaction Cr eCr", E. 0.424V. If excess Fe(s) is added to a solution in which Cr"] 1.00 M, what will be Fe] whon equilibrium is reached at 298 K? Fe (s) +2Cr Fet + 2Cr Express your answer to two significant figures and include the appropriate units. Fe*") = Value Units Submit Previous Answers Bequest Answer X Incorrect; Try Again; 5 attempts remaining
Question 8 What equation is used to relate AG rxn to K? What equation is used to relate AG to Q? Paragraph B V I UA Add a File Record Audio Record Video OR 0⁰ 8 + v www XX
Please explain, correct answer and typed answer only
Urgent
Question 5 of 15 The table shows the value of the activity coefficient of Na* Ionic strength Activity coefficient, YNa at different values of ionic strength. Interpolate the values in the table to find the activity coefficient of Na* at H = 0.025 M. (и, М) 0.001 0.964 0.005 0.928 0.01 0.902 0.05 0.82 YNa = 0.1 0.775
#9 #17
plz help asap
Give a clear handwritten answer with explanation....