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Ch.13 - Properties of Solutions
All textbooksBrown 14th EditionCh.13 - Properties of SolutionsProblem 24
Chapter 13, Problem 24

The solubility of MnSO4 · H2O in water at 20 °C is 70 g per 100 mL of water. (b) Given a solution of MnSO4 · H2O of unknown concentration, what experiment could you perform to determine whether the new solution is saturated, supersaturated, or unsaturated?

Verified step by step guidance
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Step 1: Understand the definitions of saturated, unsaturated, and supersaturated solutions. A saturated solution contains the maximum amount of solute that can dissolve at a given temperature. An unsaturated solution can dissolve more solute, while a supersaturated solution contains more solute than can typically dissolve at that temperature.
Step 2: Prepare a sample of the unknown MnSO4 · H2O solution. Ensure that the solution is at the same temperature as the given solubility data, which is 20 °C.
Step 3: Add a small amount of solid MnSO4 · H2O to the solution. Observe whether the added solute dissolves, remains undissolved, or causes crystallization.
Step 4: Analyze the observations: If the added solute dissolves, the solution is unsaturated. If the added solute does not dissolve, the solution is saturated. If crystallization occurs, the solution is supersaturated.
Step 5: Optionally, filter and dry any undissolved or crystallized MnSO4 · H2O to confirm the amount of solute present, comparing it to the known solubility to further verify the solution's status.
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?

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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.

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Open Question
The solubility of Cr1NO323 # 9 H2O in water is 208 g per 100 g of water at 15 °C. A solution of Cr1NO323 # 9 H2O in water at 35 °C is formed by dissolving 324 g in 100 g of water. When this solution is slowly cooled to 15 °C, no precipitate forms. (b) You take a metal spatula and scratch the side of the glass vessel that contains this cooled solution, and crystals start to appear. What has just happened?
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:(c) K2Cr2O7

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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.

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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,

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