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Chapter 4: Problem 10

Can a solid ever be a solvent? Explain.

Short Answer

Expert verified
Answer: Yes, although it is rare, a solid can act as a solvent in specific situations, such as the formation of solid alloys. In these cases, a solid substance breaks down other solids and forms new bonds with them. However, solids generally have lower kinetic energy, which makes it more challenging for them to act as solvents compared to liquids and gases.

Step by step solution

01

Understand Solvents and Solutes

In a solution, the substance that dissolves another substance is called the solvent, while the substance being dissolved is called the solute. Generally, solvents are liquids, and solutes can be in any state (solid, liquid, or gas).
02

Understand the Dissolving Process

The process of dissolving involves breaking the bonds between the molecules or ions in the solute and forming new bonds with the molecules of the solvent. For this to happen, the solvent particles must have enough kinetic energy to overcome the forces holding the solute particles together.
03

Determine if Solids Can Be Solvents

In general, solids have lower kinetic energy compared to liquids and gases due to their tightly packed particles. This low kinetic energy makes it hard for solid particles to overcome the forces holding solute particles together and form new bonds with them. However, there are some exceptions, where specific solid substances can act as solvents. One example is when a solid alloy is formed by mixing two or more metals together. In this case, the metal with a lower melting point acts as a solvent, dissolving the metal with a higher melting point to create a homogenous mixture.
04

Conclusion

Despite solids typically having low kinetic energy, making it more challenging for them to act as solvents, there are specific situations where they can. In certain cases, such as the formation of solid alloys, solid substances can indeed function as solvents, breaking down other solids and forming new bonds. However, these cases are not common and are largely limited to unique situations.

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Key Concepts

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

Solute
In any solution, there is a dynamic dance between two main components: the solute and the solvent. The solute is the substance that gets dissolved. It can exist in three forms: solid, liquid, or gas. Imagine stirring sugar (a solid solute) into water (a liquid solvent); the sugar becomes uniformly dispersed and no longer visibly distinct from the water.
One fascinating aspect of solute behavior is its ability to change states. For instance:
  • Solid solute: Sugar in tea is a perfect example, where the sugar dissolves to form a sweet solution.
  • Liquid solute: Vinegar mixing into oil is a trickier combination due to limited solubility.
  • Gaseous solute: Think of carbon dioxide dissolved in soda, which gives it fizz.
These examples illustrate that though we most often see liquid solvents, solutes are incredibly versatile, existing and dissolving in varied states of matter.
Dissolving Process
The art of dissolving is a remarkable process of transformation. It requires energy and affinity between the solute and solvent. In the act of dissolving, solute particles must overcome intermolecular forces that hold them together, facilitated by the solvent. A pivotal factor here is kinetic energy, which is vital for breaking these intermolecular bonds of the solute.
During dissolving, several factors come into play:
  • Kinetic energy: Solvent particles with high kinetic energy, such as those in a liquid, can effectively break solute bonds.
  • Temperature: Elevated temperatures often increase kinetic energy, enhancing dissolution.
  • Mixing and agitation: Stirring aids in dispersing solute particles, hastening the dissolving process.
When everything aligns correctly, the solute integrates into the solvent, forming a homogenous solution, ready to display new characteristics different from its separate components.
Solid Alloys
Solid alloys are an exceptional example of solids acting as solvents. They're mixtures of two or more metals blended to form a new metallic entity with distinct properties. In a solid alloy, typically, a metal with a lower melting point serves the role of a solvent, while the metal with higher melting point dissolves into it.
These unique alloys are created under specific conditions where:
  • Thermal energy: Applying heat reduces the energy disparity between the metals, aiding the solute metal to dissolve.
  • Homogeneity: The resulting alloy displays uniformity, retaining its metallic nature yet embodying various combined attributes.
Solid alloys revolutionize industries by offering enhanced strength, corrosion resistance, or electrical conductivity. This process illustrates how solids, contrary to their usual nature, can sometimes serve as solvents, expanding the boundaries of material science.

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Most popular questions from this chapter

(a) Use the solubility rules to write the balanced net ionic equation for each of the following "molecular" reactions. If there is no net reaction, write "NR." (b) Which of these three reactions give clear visual evidence of the ion exchange process? 1\. \(\mathrm{BaCl}_{2}(a q)+\mathrm{Na}_{2} \mathrm{CO}_{3}(a q) \rightarrow \mathrm{BaCO}_{3}(s)+\mathrm{NaCl}(a q)\) 2\. \(\mathrm{NaCl}(a q)+\mathrm{KOH}(a q) \rightarrow \mathrm{NaOH}(a q)+\mathrm{KCl}(a q)\) 3\. \(\mathrm{Na}_{3} \mathrm{PO}_{4}(a q)+\mathrm{CaCl}_{2}(a q) \rightarrow \mathrm{Ca}_{3}\left(\mathrm{PO}_{4}\right)_{2}(s)+\mathrm{NaCl}(a q)\)

Give the oxidation number of nitrogen in each of the following: (a) elemental nitrogen \(\left(\mathrm{N}_{2}\right) ;\) (b) hydrazine \(\left(\mathrm{N}_{2} \mathrm{H}_{4}\right) ;(\mathrm{c})\) ammonium ion \(\left(\mathrm{NH}_{4}^{+}\right)\)

The solubility of magnesium hydroxide, \(\mathrm{Mg}(\mathrm{OH})_{2},\) in water is \(9.0 \times 10^{-4} \mathrm{g} / 100.0 \mathrm{mL} .\) What volume of \(0.00100 M \mathrm{HNO}_{3}\) is required to neutralize \(1.00 \mathrm{L}\) of saturated \(\mathrm{Mg}(\mathrm{OH})_{2}\) solution?

A precipitate may appear when two completely clear aqueous solutions are mixed. What circumstances are responsible for this event?

How are the gains or losses of electrons related to changes in oxidation numbers?
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