Use the following table for problems 9.25 to 9.28: A solution containing 80. g of KCl in 200. g of H₂O at 50 °C is cooled to 20 °C.a. How many grams of KCl remain in solution at 20 °C?

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Identify the solubility of KCl at 50 °C and 20 °C using the provided table.

Determine how much KCl can dissolve in 200 g of H₂O at 20 °C based on the solubility data.

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Calculate the difference between the initial amount of KCl (80 g) and the amount that can remain dissolved at 20 °C.

The difference will indicate how much KCl will precipitate out of the solution as it cools from 50 °C to 20 °C.

Subtract the precipitated amount from the initial 80 g to find the grams of KCl remaining in solution at 20 °C.

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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. For KCl in water, solubility changes with temperature; typically, as temperature decreases, solubility also decreases, leading to potential precipitation of the solute. Understanding the solubility curve for KCl is essential to determine how much remains dissolved when the solution is cooled.

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Saturation Point

The saturation point is the stage at which a solution can no longer dissolve additional solute at a specific temperature. When a solution is saturated, any excess solute will precipitate out. In this problem, knowing the saturation point of KCl at 20 °C is crucial to determine how much KCl remains in solution after cooling.

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Temperature Effects on Solubility

Temperature significantly affects the solubility of most solids in liquids. Generally, higher temperatures increase solubility, allowing more solute to dissolve. Conversely, cooling a solution can lead to decreased solubility, which may result in some solute crystallizing out of the solution. This concept is vital for predicting the behavior of KCl when the solution is cooled from 50 °C to 20 °C.

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Use the following table for problems 9.25 to 9.28:

A solution containing 80. g of NaNO₃ in 75 g of H₂O at 50 °C is cooled to 20 °C.b. How many grams of solid NaNO₃ crystallized after cooling?

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In a laboratory experiment, a 10.0-mL sample of NaCl solution is poured into an evaporating dish with a mass of 24.10 g. The combined mass of the evaporating dish and NaCl solution is 36.15 g. After heating, the evaporating dish and dry NaCl have a combined mass of 25.50 g. (9.4)a. What is the mass percent (m/m) of the NaCl solution?

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Textbook Question

Use the following table for problems 9.25 to 9.28:

A solution containing 80. g of NaNO₃ in 75 g of H₂O at 50 °C is cooled to 20 °C.b. How many grams of solid NaNO₃ crystallized after cooling?

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