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Ch.13 - Properties of Solutions
All textbooksBrown 15th EditionCh.13 - Properties of SolutionsProblem 25c
Chapter 13, Problem 25c

By referring to Figure 13.15, determine whether the addition of 40.0 g of each of the following ionic solids to 100 g of water at 40 °C will lead to a saturated solution:(c) K2Cr2O7

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1
Identify the solubility of K_2Cr_2O_7 in water at 40 °C from Figure 13.15. This will tell you how many grams of K_2Cr_2O_7 can dissolve in 100 g of water at this temperature.
Compare the given amount of K_2Cr_2O_7 (40.0 g) to the solubility value obtained from the figure.
If the solubility value is greater than or equal to 40.0 g, the solution will be unsaturated or just saturated, meaning all the K_2Cr_2O_7 can dissolve.
If the solubility value is less than 40.0 g, the solution will be saturated, and some of the K_2Cr_2O_7 will remain undissolved.
Conclude whether the addition of 40.0 g of K_2Cr_2O_7 to 100 g of water at 40 °C results in a saturated solution based on the comparison.

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Key Concepts

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

Solubility

Solubility is the maximum amount of a solute that can dissolve in a given quantity of solvent at a specific temperature. It is typically expressed in grams of solute per 100 grams of solvent. Understanding solubility is crucial for determining whether a solution can become saturated, meaning no more solute can dissolve in the solvent at that temperature.
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Saturated Solution

A saturated solution is one in which the maximum amount of solute has been dissolved in the solvent at a given temperature, resulting in an equilibrium between dissolved and undissolved solute. When additional solute is added to a saturated solution, it will not dissolve, indicating that the solubility limit has been reached.
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Ionic Compounds and Their Solubility

Ionic compounds, such as K<sub>2</sub>Cr<sub>2</sub>O<sub>7</sub>, dissociate into their constituent ions when dissolved in water. The solubility of these compounds varies widely depending on the specific ions involved and the temperature. Knowledge of the solubility rules helps predict whether a particular ionic solid will dissolve in water and to what extent.
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Related Practice
Textbook Question

Two nonpolar organic liquids, hexane (C6H14) and heptane (C7H16), are mixed. (b) Hexane and heptane are miscible with each other in all proportions. In making a solution of them, is the entropy of the system increased, decreased, or close to zero, compared to the separate pure liquids?

Textbook Question

KBr is relatively soluble in water, yet its enthalpy of solution is + 19.8 kJ/mol. Which of the following statements provides the best explanation for this behavior? (a) Potassium salts are always soluble in water. (b) The entropy of mixing must be unfavorable. (c) The enthalpy of mixing must be small compared to the enthalpies for breaking up water–water interactions and K–Br ionic interactions. (d) KBr has a high molar mass compared to other salts like NaCl.

Textbook Question

By referring to Figure 13.15, determine whether the addition of 40.0 g of each of the following ionic solids to 100 g of water at 40 °C will lead to a saturated solution: (d) Pb(NO3)2.

Textbook Question

By referring to Figure 13.15, determine the mass of each of the following salts required to form a saturated solution in 250 g of water at 30 °C: (b) Pb(NO3)2,

Textbook Question

By referring to Figure 13.15, determine the mass of each of the following salts required to form a saturated solution in 250 g of water at 30 °C: (c) Ce2(SO4)3.