Redox Reaction
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Redox titration determines the concentration of an analyte containing either an oxidizing or a reducing agent.
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Redox titration determines the concentration of an unknown solution (analyte) that contains an oxidizing or reducing agent.
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Calculate the concentration of an unknown analyte.
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EXAMPLE:
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1. 0.2640 g of sodium oxalate is dissolved in a flask and requires 30.74 mL of potassium permanganate (from a buret) to titrate it and cause it to turn pink (the end point).
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How many moles of sodium oxalate are present in the flask?
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How many moles of potassium permanganate have been titrated into the flask to reach the end point?
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What is the molarity of the potassium permanganate?
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2. Potassium dichromate is used to titrate a sample containing an unknown percentage of iron. The sample is dissolved in H3PO4/H2SO4 mixture to reduce all of the iron to Fe ions. The solution is then titrated with 0.01625 M K2Cr2O7, producing Fe and Cr ions in acidic solution. The titration requires 32.26 mL of K2Cr2O7 for 1.2765 g of the sample.
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Determine the percent iron in the sample.
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3. The iodine produce when an excess of KI was added to a solution containing of K2Cr2O7 (0.1518 g) required a 46.13 ml titration with Na2S2O3. Calculate the molar concentration of the thiosulfate solution.
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4. A 0.1017 g of sample KBrO3 was dissolved in dilute HCl and treated with an unmeasured excess of KI. The liberated Iodine required 39.75 ml of Na2S2O3 solution. Calculate the molarity of Na2S2O3.
References and Sources:
http://www.chemteam.info/Redox/WS-redox-titration-problems.html
http://www.ausetute.com.au/redoxtitr.html
Advance Chemistry Notebook
Written By: Terry Maine Dela Pieza
