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11 Dec 2019

What is the concentration of Cu in a solution if a 25.00 mL aliquot reacted with an excess of KI that requires 15.64 mL of 39.94 mM Na2S2O3 solution to titrate the liberated iodine?

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Reid Wolff
Reid WolffLv2
13 Dec 2019

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Related questions

A standard iodate solution is prepared at 22.0 °C by dissolving 0.9123 g (uncorrected mass) of KIO3 with deionized water in a 499.92 mL volumetric flask. To standardize the Na2S2O3 solution, a 10.005 mL aliquot of the KIO3 solution is acidified, treated with excess KI, and titrated with Na2S2O3, requiring 22.05 mL to reach the end point. Finally, a 10.005 mL aliquot of unknown Cu solution is reduced with excess KI. The liberated iodine requires 31.46 mL of Na2S2O3 solution to reach the end point. Calculate the unknown Cu concentration in g/L.

These are what the correct step answers should be, just need to show how to do work:

[KIO3 standard (corrected to 20 °C): 8.53255 mM]

[S2O3 2− titrant: 23.2294 mM]

FINAL ANSWER: [Unknown: 4.64160 g/L Cu]

Help with some a prelab!

A 25 mL aliquot of 0.0104 M KIO3 solution is titrated to the stoichiometric point with 17.27 mL of sodium thiosulfate, Na2S2O3, solution. What is the molar concentration of Na2S2O3 solution?

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