What is the strength of the ionic interactions between an ion with 1 positive charges and an ion with 2 negative charges, when the distance between them is 32.3 nanometers and the solvent is water, at 25 oC with a dielectric constant of 78.5? Calculate answer to 7 decimal places. Do not specify units in the answer.

What is the strength of the ionic interactions between an ion with 1 positive charges and an ion with 2 negative charges, when the distance between them is 32.3 nanometers and the solvent is water, at 25 oC with a dielectric constant of 78.5? Calculate answer to 7 decimal places. Do not specify units in the answer.

General, Organic, and Biological Chemistry

7th Edition

ISBN:9781285853918

Author:H. Stephen Stoker

Publisher:H. Stephen Stoker

Chapter8: Solutions

Section: Chapter Questions

Problem 8.9EP: A solution is made by dissolving 34.0 g of NaCl in 100 g of H2O at 0C. Based on the data in Table...

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A solution is made by dissolving 34.0 g of NaCl in 100 g of H2O at 0C. Based on the data in Table 8-1, should this solution be characterized as a. saturated or unsaturated b. dilute or concentrated
What is the strength of the ionic interactions between an ion with 1 positive charges and an ion with 2 negative charges, when the distance between them is 32.3 nanometers and the solvent is water, at 25 °C with a dielectric constant of 78.5? Calculate answer to 7 decimal places. Do not specify units in the answer.
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In performing an experiment on freezing point depression, the solution was prepared by dissolving2.25 g of salt in 20.00 mL distilled water (density = 0.997 g mL-1; Tf = 0 °C; kf = 1.86 °C m-1). We determined thefreezing point of the solution to be -3.48 °C. We later found out that the salt we used was sodium chloride that wascontaminated with potassium chloride. Calculate ΔTf for the experiment.
In performing an experiment on freezing point depression, the solution was prepared by dissolving2.25 g of salt in 20.00 mL distilled water (density = 0.997 g mL-1; Tf = 0 °C; kf = 1.86 °C m-1). We determined thefreezing point of the solution to be -3.48 °C. We later found out that the salt we used was sodium chloride that wascontaminated with potassium chloride.1. Calculate ΔTf for the experiment.2. Calculate the molality of the solution.3. Calculate the mass of potassium nitrate present in the salt sample.
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