You and a colleague are performing freezing-point depression experiments with standard concentrated and dilute solutions of KNO3 in water. If you assume i = 2 for the ionic compound, all your data makes sense for dilute solutions. But when your colleague measures data for a concentrated solution, she concludes that i = 1.5. Suggest an explanation. O Your colleague must be doing something wrong; i is always an integer. O At high concentrations, it is possible that ion pairs form in solution, such as K*---NO, which acts like one "particle" instead of two, thereby reducing the van't Hoff factor. O Freezing-point depression is only valid for dilute solutions, so your colleague should throw out the data for concentrated solutions. O The nitrate anion is reacting with water, so the number of ions in solution is actually decreasing at high concentrations. O Your colleague should just round 1.5 to 2.

You and a colleague are performing freezing-point depression experiments with standard concentrated and dilute solutions of KNO3 in water. If you assume i = 2 for the ionic compound, all your data makes sense for dilute solutions. But when your colleague measures data for a concentrated solution, she concludes that i = 1.5. Suggest an explanation. O Your colleague must be doing something wrong; i is always an integer. O At high concentrations, it is possible that ion pairs form in solution, such as K*---NO, which acts like one "particle" instead of two, thereby reducing the van't Hoff factor. O Freezing-point depression is only valid for dilute solutions, so your colleague should throw out the data for concentrated solutions. O The nitrate anion is reacting with water, so the number of ions in solution is actually decreasing at high concentrations. O Your colleague should just round 1.5 to 2.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter13: The Chemistry Of Solutes And Solutions

Section: Chapter Questions

Problem 76QRT: A 1.00 mol/kg aqueous sulfuric acid solution, H2SO4,freezes at 4.04 C. Calculate i, the vant Hoff...

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