A KNO 3 solution containing 45 g of KNO 3 per 100.0 g of water is cooled from 40 °C to 0 °C. What happens during cooling? (Use Figure 13.11.)

Hello everyone. So this problem being told by a solution was created by the solving 45 g of K C L. 03 and 100 g of water afterwards. The solution temperatures was lower 200 degrees Celsius to 10 degrees Celsius. So does K C L. 03 precipitate out of the solution. The ability of the K C L. 03 is given At 100°C as well as 10°C. Alright, so a substance eligibility is the amount of the substance that can be dissolved in a given volume of solvent at a particular temperature. So at 100 degrees Celsius, 45 g of the K C. L. 03 In 100 g of water is less than the scalability of KC. in water at this temperature. So we get from this information is that all The KCL. 03 will be dissolved Now at 0°C 45g of K. so 03 In 100 g of water is more is more valuable than that of the K. c. l. 03 In H 20. At this temperature. So we can get from this information is that excess? So I'll just you know that X. S. So access of the K. C. L. 03 will precipitate out. So again, the question here is does K. C. L three precipitate out of this solution? So the only thing that's precipitating out is the excess. So our answer then KCO. doesn't precipitate out of the solution. So this right here is going to be my final answer for this problem. Thank you all so much for watching.

Ch.13 - Solutions

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Tro 4th Edition

Ch.13 - Solutions

Problem 43

Chapter 13, Problem 43

A KNO₃ solution containing 45 g of KNO₃ per 100.0 g of water is cooled from 40 °C to 0 °C. What happens during cooling? (Use Figure 13.11.)

Verified step by step guidance

Identify the solubility of KNO3 at the initial and final temperatures using the solubility curve provided in Figure 13.11. Solubility is typically given in grams of solute per 100 grams of solvent.

Calculate the initial concentration of the solution in terms of grams of KNO3 per 100 grams of water at 40 °C.

Compare the initial concentration to the solubility of KNO3 at 40 °C. If the initial concentration exceeds the solubility, the solution is supersaturated. If it is less, it is unsaturated.

Determine the solubility of KNO3 at the final temperature of 0 °C using the same solubility curve.

Compare the initial concentration of KNO3 to the solubility at 0 °C. If the initial concentration exceeds the solubility at 0 °C, precipitation will occur until the concentration matches the solubility at this temperature.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Solubility

Solubility refers to the maximum amount of a solute that can dissolve in a solvent at a given temperature and pressure. In the case of KNO3, its solubility decreases as the temperature drops, meaning that less KNO3 can remain dissolved in water at lower temperatures. Understanding solubility is crucial for predicting whether a solution will remain saturated or if precipitation will occur when cooled.

Saturation and Precipitation

A saturated solution is one where the maximum amount of solute has been dissolved in the solvent at a specific temperature. When a saturated solution is cooled, it may exceed its solubility limit, leading to precipitation, where the excess solute forms solid crystals. This concept is essential for understanding the changes that occur in the KNO3 solution as it cools from 40 °C to 0 °C.

Cooling Effects on Solutions

Cooling a solution affects the kinetic energy of the molecules, which can lead to changes in solubility and the state of the solute. As temperature decreases, the solute's ability to remain dissolved diminishes, potentially resulting in crystallization. This principle is important for analyzing the behavior of the KNO3 solution as it transitions from a warmer to a cooler state.