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Chapter 7: Problem 46

Solubility of sodium hydroxide increases with increase in temperature.

Short Answer

Expert verified
Sodium hydroxide becomes more soluble in water as temperature increases.

Step by step solution

01

Understanding Solubility and Temperature Relationship

Solubility is the maximum amount of solute that can dissolve in a given amount of solvent at a specific temperature. For most solids like sodium hydroxide, solubility increases as temperature increases because higher temperatures provide more kinetic energy to molecules, allowing more of the solute to dissolve.
02

Apply this Concept to Sodium Hydroxide

Sodium hydroxide (NaOH) is a solid that dissolves in water. As the temperature of the water increases, the kinetic energy of water molecules also increases. This leads to more frequent and energetic collisions between solute and solvent particles, causing more NaOH to dissolve.
03

Considerations for Practical Application

In industrial or laboratory settings, increasing the temperature of the solvent can help in achieving a higher concentration of sodium hydroxide in solution. This property is leveraged when preparing solutions requiring higher NaOH concentrations at elevated temperatures.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Sodium Hydroxide
Sodium Hydroxide, commonly known as NaOH, is a white, highly caustic substance that is used extensively in various industries. It is a strong base and is essential in the production of soap, paper, and textiles. NaOH is also utilized in water treatment and as a cleaning agent.

When sodium hydroxide dissolves in water, it dissociates into sodium ions (Na鈦�) and hydroxide ions (OH鈦�). This dissociation is essential for the compound's strong alkaline nature, making solutions of NaOH very effective in breaking down acids and organic materials.

The solubility of sodium hydroxide in water makes it a versatile component in chemical reactions, helping to adjust pH levels and participate in neutralization processes. Its ability to dissolve enhances its applicability in both household cleaning products and complex industrial syntheses.
Temperature and Solubility Relationship
The principle of temperature influencing solubility is straightforward yet fundamental. Solubility refers to how much solute can dissolve in a solvent at a specific temperature. In the case of most solids, including sodium hydroxide, solubility typically increases with temperature.

As temperature rises, the solvent molecules move more energetically, providing the necessary conditions for solute particles to break away from their solid structure. This means that at higher temperatures, more NaOH can dissolve in water, resulting in a more concentrated solution.

In practical terms, this relationship allows for control and manipulation of solubility in various chemical and industrial processes. For example, a manufacturer looking to create a concentrated NaOH solution would increase the temperature of the solvent, ensuring maximum dissolution.
Kinetic Energy in Solutions
Kinetic energy plays a pivotal role in the process of dissolution. In a solution, both solvent and solute molecules are in constant motion. As the temperature of a solution increases, the kinetic energy of its particles also increases.

For sodium hydroxide, when the water's temperature rises, its molecules move faster, creating more frequent collisions with NaOH particles. These collisions provide the energy necessary to overcome the attractive forces within the solid NaOH, encouraging more of it to dissolve.

This concept explains why heating a solution can dramatically increase the dissolving rate of many solutes. Not only does this enhance their solubility, but it also accelerates chemical reactions, making kinetic energy an essential consideration in both laboratory and industrial settings.

By understanding the role of kinetic energy, one can predict and control how different substances behave in various conditions, leading to optimal efficiency and outcomes in chemical processes.

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Most popular questions from this chapter

Calculate the \(\mathrm{pH}\) of an aqueous solution of \(1.0 \mathrm{M}\) ammonium formate assuming complete dissociation. (p \(K_{a}\) of formic acid \(=3.8\) and \(\mathrm{p} K_{b}\) of ammonia \(=4.8\).)

The following acids have been arranged in the order of decreasing acid strength. Identify the correct order. \(\mathrm{ClOH}\) (I), \(\mathrm{BrOH}(\mathrm{II}), \mathrm{IOH}(\mathrm{III})\) (a) \(\mathrm{I}>\mathrm{II}>\mathrm{III}\) (b) \(\mathrm{II}>\mathrm{I}>\mathrm{III}\) (c) \(\mathrm{III}>\mathrm{II}>\mathrm{I}\) (d) \(\mathrm{I}>\mathrm{III}>\mathrm{II}\)

When equal volumes of the following solutions are mixed, precipitation of \(\mathrm{AgCl}\left(\mathrm{K}_{\mathrm{sp}}=1.8 \times 10^{-10}\right)\) will occur only with (a) \(10^{-4} \mathrm{M}\left(\mathrm{Ag}^{+}\right)\)and \(10^{-4} \mathrm{M}\left(\mathrm{Cl}^{-}\right)\) (b) \(10^{-5} \mathrm{M}\left(\mathrm{Ag}^{+}\right)\)and \(10^{-5} \mathrm{M}\left(\mathrm{Cl}^{-}\right)\) (c) \(10^{-6} \mathrm{M}\left(\mathrm{Ag}^{+}\right)\)and \(10^{-6} \mathrm{M}\left(\mathrm{Cl}^{-}\right)\) (d) \(10^{-10} \mathrm{M}\left(\mathrm{Ag}^{+}\right)\)and \(10^{-10} \mathrm{M}\left(\mathrm{Cl}^{-}\right)\)

In reaction \(\mathrm{A}+2 \mathrm{~B} \rightleftharpoons 2 \mathrm{C}+\mathrm{D}\), initial concentration of \(\mathrm{B}\) was \(1.5\) times of \([\mathrm{A}]\), but at equilibrium the concentrations of \(\mathrm{A}\) and \(\mathrm{B}\) became equal. The equilibrium constant for the reaction is: (a) 8 (b) 4 (c) 12 (d) 6

The \(\mathrm{pH}\) of a \(0.02 \mathrm{M} \mathrm{NH}_{4} \mathrm{Cl}\) solution will be [given \(\mathrm{K}_{\mathrm{b}}\left(\mathrm{NH}_{4} \mathrm{OH}\right)=10^{-5}\) and \(\log 2=0.301]\) (a) \(2.65\) (b) \(4.35\) (c) \(4.65\) (d) \(5.35\)
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