and in4) To adjust the thiosulfate (S2O32) solution to be used as a titrant in thecopper determination, excess KI was added to exactly 25.0 mL of 5.68 x103 M KIO3 solution to liberate iodine (12) and 16.4 mL of thiosulfatesolution is being consumed in the titration of I2. In this standardizationprocess, the concentration of the thiosulfate solution is calculated.ー1852x10- 0, OSZM103 +51 (excess)+ 6H*→ 3lz+ 3H2O142x10-616.4 xdo3426x 10-6Iz+ 2S,032> S.O6²+21 -426 185x10-6Then, for copper determination 25.0 mL of 250 mL copper-aliquots istaken and treated with excess KI.Cu?++ 21(excess)→ Cul + % l2The liberated 2 was titrated with the 8.2 mL of adjusted thiosulfatesolution (S2O32).し032×82こ25×MI212+ 2S2032→ S4O,²+21-Mエ2こ0.04 とでと034MWCalcylate, how many milligrams of copper is found in the sample? (Cu:63.5 g/ mol)O. Og x6]5 =0.52970.034 9O085mde

Answered: Image /qna-images/answer/828d6bbf-b4f5-478c-a9cc-4e98fc6def04.jpg

and in 4) To adjust the thiosulfate (S2O32) solution to be used as a titrant in the copper determination, excess KI was added to exactly 25.0 mL of 5.68 x 103 M KIO3 solution to liberate iodine (l2) and 16.4 mL of thiosulfate solution is being consumed in the titration of I2. In this standardization process, the concentration of the thiosulfate solution is calculated. 852x10 - 0, OSZM 103 +51 (excess)+ 6H*→ 3lz+ 3H2O 142x10-6 16.4 xlo3 426x 10-6 Iz+ 2S,032> S.O6²+21 - 1852x10-6 Then, for copper determination 25.0 mL of 250 mL copper-aliquots is 426 taken and treated with excess KI. Cu**+ 21(excess)→ Cul + % l2 The liberated 2 was titrated with the 8.2 mL of adjusted thiosulfate solution (S2O32). し032×82こ25×MI2 I2+ 2S2032→ S4O,²÷+21- Mエ2こ0.04 とでと034MW Calcylate, how many milligrams of copper is found in the sample? (Cu: 63.5 g/ mol) O. Ogs x6]5 =0.5297 v.034 O.085mde

and in 4) To adjust the thiosulfate (S2O32) solution to be used as a titrant in the copper determination, excess KI was added to exactly 25.0 mL of 5.68 x 103 M KIO3 solution to liberate iodine (l2) and 16.4 mL of thiosulfate solution is being consumed in the titration of I2. In this standardization process, the concentration of the thiosulfate solution is calculated. 852x10 - 0, OSZM 103 +51 (excess)+ 6H*→ 3lz+ 3H2O 142x10-6 16.4 xlo3 426x 10-6 Iz+ 2S,032> S.O6²+21 - 1852x10-6 Then, for copper determination 25.0 mL of 250 mL copper-aliquots is 426 taken and treated with excess KI. Cu**+ 21(excess)→ Cul + % l2 The liberated 2 was titrated with the 8.2 mL of adjusted thiosulfate solution (S2O32). し032×82こ25×MI2 I2+ 2S2032→ S4O,²÷+21- Mエ2こ0.04 とでと034MW Calcylate, how many milligrams of copper is found in the sample? (Cu: 63.5 g/ mol) O. Ogs x6]5 =0.5297 v.034 O.085mde

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

Consider the reaction of Potassium Phosphate and Nickel (II) Bromide, where 15.00 ml of 0.7000M K3PO4 is mixed with 15.00ml of 0.2000M NiBr2 (and the final volume is 30.00 ml, that is there is no change in volume upon mixing). Your answer has to include all of the following: What is the limiting reagent? What is the identity and mass of precipitate formed? What is the concentration of the alkali metal that is a spectator ion? What is the concentration of the excess phosphate?
A sample consisting of Na2CO3 (105.96), NaOH (39.99) and inert matter weighs 1.179 g. It is titrated with 0.300 N HCI with phenolphthalein as the indicator, and the solution becomes colorless after the addition of 48.16 ml. Methyl orange is then added and 24.08 ml more of the acid are needed for the color change. What is the percentage of NaOH and N22CO3? *
(a) You are about to prepare three solutions of 0.5 M KI, 0.01 M K2S2O8, and 0.01 M Na2S2O3*5H2O in 250 mL volumetric flasks. - Describe how you will go about this, i,e, explain all steps of weighing of solutes, volumetric measurements (filling up with deionised water) ect. Calculate what mass of solute you will need in each of solutions mentioned above that you need to prepare. Show all calculations steps. (b) You are also tasked to fill burettes with the above-mentioned solutions, however, after filling up the solutions, you realised that there is a bubble towards the bottom tip inside the burette. Is it wise to continue with the experiment, while there is a bubble, if NOT explain why. (c) According to the manual's Experimental procedure, one conical flask (flask 1) contains a mixture of 20 mL of the KI solution plus 10 mL of the Na2S2O3 solution, while in the second flask (flask 2) there is 20 mL of the K2S2O8 solution with added five drops of starch solution. Why can't you add…
Analytical chemistry
A sample of unknown iron ore weighs 0.35 g. It is digested using dilute HCl. An SnCl2 solution is added to turn the solution yellow. Zimmermann–Reinhardt reagent is added, and the solution is diluted to 150mL. It is then titrated with 31.30 mL of 0.045 M potassium permanganate. a) How many moles of MnO4- were used to titrate the iron in the sample? b) How many moles of Fe2+ were in the sample? c) What is the mass of iron in the sample? d) What is the % w/w of Fe in the sample?
The gravimetric determination of Ni: Ni (58.7 g/mol) was precipitated as Ni(DMG) 2 (288.7 g/mol). The volume of unknown solution in the sample =30.00 mL. The mass of empty crucible = 30.107 g, the mass of empty crucible and precipitate = 30.300 g. Calculate the concentration of NiT in the unknown in sample solution (in mg/L) is: 1. O2.62X103 2. O1.31X 103 3. 25.3X 104 4. 00.5X 10 Previous Next hp
1.50 mL of 0.15M Fe2(SO4)3 is diluted with deionized water to 25.00 mL in a volumetric flask. What is the concentration (molarity) of iron (not Fe2(SO4)3) in the diluted sample?
A solid sample containing some Fe2+ion had a total mass of .9791 g. It required 18.2 ml of 0.02304 M KMnO4 to titrate the Fe2+ in the dissolved sample to a pink endpoint. How many moles of Fe2+ were in the the sample? How many grams of irion were present in the sample and what was the mass percent iron in the sample?