Question

A sample of KIO3 primary standard solid weighing 0.1517 grams was added to a solution containing excess KI. The liberated I2 required 29.46 mL of sodium thiosulfate (Na2S2O3) solution to reach endpoint in a titration. Calculate the molarity of the "standardized thiosulfate solution", using the overall equation below. MW KIO3=214.0 g/mol IO3- + 6 H+ + 6 S2O32- -> 3 S4O62- + I- + 3 H2O

          A sample of KIO3 primary standard solid weighing 0.1517 grams was added to a solution containing excess KI. The liberated I2 required 29.46 mL of sodium thiosulfate (Na2S2O3) solution to reach endpoint in a titration. Calculate the molarity of the "standardized thiosulfate solution", using the overall equation below. MW KIO3=214.0 g/mol

IO3- + 6 H+ + 6 S2O32- -> 3 S4O62- + I- + 3 H2O

A sample of KIO3 primary standard solid weighing 0.1517 grams was added to a solution containing excess KI. The liberated I2 required 29.46 mL of sodium thiosulfate (Na2S2O3) solution to reach endpoint in a titration. Calculate the molarity of the "standardized thiosulfate solution", using the overall equation below. MW KIO3=214.0 g/mol

IO3- + 6 H+ + 6 S2O32- -> 3 S4O62- + I- + 3 H2O

Added by Lauren C.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert David Collins

06/04/2023

Step 1

First, we need to find the moles of KIO3 in the sample: moles of KIO3 = (mass of KIO3) / (molecular weight of KIO3) moles of KIO3 = (0.1517 g) / (214.0 g/mol) = 7.09 x 10^-4 mol Show more…

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A sample of KIO3 primary standard solid weighing 0.1517 grams was added to a solution containing excess KI. The liberated I2 required 29.46 mL of sodium thiosulfate (Na2S2O3) solution to reach endpoint in a titration. Calculate the molarity of the "standardized thiosulfate solution" using the overall equation below: MW KIO3 = 214.0 g/mol