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

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Concept explainers

Solutions

Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to as solute. Solution chemistry plays an important role in chemistry since it supports many commercial applications of solutions.

Question

Part A
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.
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*---NO3, which acts like one "particle" instead of two, thereby reducing the van't Hoff factor.
Freezing-point depression is only valid for dilute solutions, so your colleague should throw out the data for concentrated solutions.
The nitrate anion is reacting with water, so the number of ions in solution is actually decreasing at high concentrations.
Your colleague should just round 1.5 to 2.
O O O

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