Consider that the determination of potassium iodide (MM-166.00 g/mol) from a food supplement was performed by the Volhard method. For this, a 0.5240g sample of the supplement was dissolved and treated with 10.00 ml. of a 0.1035 mol/l. AgNO3 solution. The excess silver ions were then titrated with 8.25 ml. of a 0.0550 mol/l. KSCN solution using ammoniacal ferrie sulfate solution as an indicator a)Write down the three balanced chemical reactions that are involved in this method and briefly explain how it is determined the end point of this titration. b)What is the percentage of potassium iodide in the supplement?
Consider that the determination of potassium iodide (MM-166.00 g/mol) from a food supplement was performed by the Volhard method. For this, a 0.5240g sample of the supplement was dissolved and treated with 10.00 ml. of a 0.1035 mol/l. AgNO3 solution. The excess silver ions were then titrated with 8.25 ml. of a 0.0550 mol/l. KSCN solution using ammoniacal ferrie sulfate solution as an indicator a)Write down the three balanced chemical reactions that are involved in this method and briefly explain how it is determined the end point of this titration. b)What is the percentage of potassium iodide in the supplement?
Chapter16: Applications Of Neutralization Titrations
Section: Chapter Questions
Problem 16.40QAP
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Consider that the determination of potassium iodide (MM-166.00 g/mol) from a food supplement was performed by the Volhard method. For this, a 0.5240g sample of the supplement was dissolved and treated with 10.00 ml. of a 0.1035 mol/l. AgNO3 solution. The excess silver ions were then titrated with 8.25 ml. of a 0.0550 mol/l. KSCN solution using ammoniacal ferrie sulfate solution as an indicator
a)Write down the three balanced chemical reactions that are involved in this method and briefly explain how it is determined the end point of this titration.
b)What is the percentage of potassium iodide in the supplement?
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