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April 23, 2014

Homework Help: CHemistry Please Help..............LAB

Posted by Sara on Sunday, October 19, 2008 at 3:28pm.

Standardization of the Sodium Thiosulfate Solution

Make up a standard solution of potassium iodate by accurately “weighing by difference” about 0.1 g of KIO3 and placing it in your 100 mL volumetric flask. Fill the flask to mark with distilled water. Potassium iodate reacts with excess KI in acid solution according to the following reaction:

IO3- + 5I- + 6H^+ ----> 3I2 + 3H2O

RECALL:

2S2O3^2- + I2 ---> 2I- + S4O6^ 2-

To perform then standardized, first prepare the buret with the given solution of Na2S2O3. Then dispense 25 mL of KIO3 solution by pipet into a 250 mL Erlenmeyer flask, add 25 mL of 2% (v/v) KI solution and then add 10 mL of 1M HCL, and mix swirling. A deep brown colour should appear, indicating the presence of iodine. Titrate immediately with the Na2S2O3 solution in the buret until the brown fades to a pale yellow and then add 5 mL of starch indicator solution and continue the titration until the deep blue colour of the starch indicator disappears. Record the volume of the sodium thiosulafte solution used in the titration. Determine the stoichiometric ratio between the iodate and thiosulafte and use this to calculate the accurate concentration if the Na2S2O3 solution.

A.Standardization of Na2S2O3 ( Sodium thiosulfate)

Mass of KIO3 in 100 mL - 0.1255g

Find Molarity of potassium Iodate: (PLEASE CHECK IF CORRECT)

n= 0.1255/ 214 = 5.86*10^-4
100ml/1000= 0.1L

Molarity = 5.86*10^-4 /0.1
= 5.86*10^-3

Therefore, the concentration of KIO3 is: 5.86*10^-3

Titration:

Average Volume of Na2S2O3 = 27.15 mL

Concentration of Na2S2O3 _______________M.

I am not sure how to calculate this

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