Solute vs Solvent- Definition, 9 Major Differences, Examples

Solute Definition

A solute is a substance that is added to a solvent to form a solution.

• The solute can exist in all three forms of matter as solid, liquid, or gas.
• In a homogenous mixture, the solute completely dissolves in another substance, and the solute is uniformly distributed throughout the solution.
• In a heterogeneous mixture, the solute is not distributed uniformly, and its concentration is different in different parts of the solution.
• The amount of solute in a solution is measured in terms of its concentration. The concentration of solute in a solution is determined by the ratio of the amount of the solute and the total volume of the solution.
• The property of solute particles to dissolve within the solvent is termed as solubility. The solubility of a solute depends on a number of factors.
• In solids and gases, temperature directly affects the solubility of the solute. Pressure, however, only affects the solubility of gases.
• Besides, the ability of solid particles to dissolve in a solvent is dependent on their own chemical structure. Polar solute dissolves in a polar solvent and vice versa.
• The molecular size of the solute is also essential in the solution as the solvent breaks down the solute particles and distributes it throughout the solution.
• In almost all types of solutions, the amount or volume of solute is less than that of the solvent.
• Solute particles tend to have a higher boiling point than solvents.
• Examples of solute include salt in seawater, protons in the cytosol, sugar in tea, etc.

Solvent Definition

A solvent is a substance that dissolves the solute particles during the formation of a solution.

• Most solvents are in a liquid state, but some solvents might be in a gas or solid-state.
• The solvent breaks down the larger solute particle into smaller particles that can then be dispersed throughout the solution.
• Solvent forms the medium of the solution that makes up most of the volume of the solution.
• The amount of solute that can be dispersed in the solvent depends on the temperature of the medium.
• A solution is a homogenous mixture where the solute particles are uniformly distributed throughout the solvent. Thus, each volume of solvent in the solution has the same concentration of solute.
• The solvent and solute in a solution exist in the single-phase forming solute-solvent complexes, also known as solvates.
• During the formation of a solution, multiple solvent particles surround the solute particle where heat energy is transferred from solvent to the solute, creating a more thermodynamically stable condition.
• The polarity of the solvent particle is crucial to determine the solubility of any solute in the solvent.
• Water is a polar compound that is also considered as a universal solvent that dissolves a large number of solute particles.
• Most solvents are classified into two categories as polar and non-polar solvents. Mercury forms a particular type of solvent called amalgams.
• The boiling point of the solvent is lower than that of the solute.
• Examples of the solvent include water, hydrocarbons, alcohols, esters, etc.

Key Differences (Solute vs Solvent)

Examples of Solutes

Salt in seawater

• Salt is the solute, and water is the solvent in seawater.
• The salt, NaCl, is an ionic compound where the negatively charged chloride ion is attracted by the slightly positively charged hydrogen atom of water. A similar attraction occurs between sodium and oxygen atoms.
• This attraction causes the breakdown of NaCl into smaller particles which are then dispersed throughout the water.
• The range of solubility and time period depends on the surface area of the solute particle.
• Thus, coarse salts dissolve to a lesser extent than finer salts with a larger surface area.
• Once all the salt is dissolved, no salt crystals will be visible in the solution.

Read Also: Lewis Acids and Bases

Protons in the cytosol

• Protons or H⁺ are present in the cytoplasm of a cell that helps to maintain the pH of the solution.
• These protons are attracted by the oxygen atom of water molecules and thus play an essential role in the transmembrane transport of molecules.
• The membranes are permeable to water but not to the protons. As a result water molecules can freely across the membrane.
• Due to the attraction between the water molecules and protons, a proton motive force is created.
• The proton motive force can then be used for the transport of a variety of substances across the membrane.

Examples of Solvents

Water

• Water is considered a universal solvent as it dissolves a wide variety of solute particles.
• Water forms the basis of many biological solutions that carries important particles and moves them throughout the body.
• Water is a polar solvent where the oxygen atom carries a partial negative charge, and the hydrogen atom carries a partial positive charge.
• The polarity of water molecules makes it very compatible with several solutes molecules.
• One of the most important examples of water as a solvent is seawater. Seawater carries large quantities of salt dissolved in water.

Oil

• Oil also acts as a solvent in cooking where it prevents the sticking of polar and on polar solutes to the pan.
• The hot oil creates a solution where other foods can be cooked.
• The oil carries some solute which can then be added to the food being cooked.
• Oil is an organic compound and an example of a non-polar solvent, that allows the dispersal of non-polar solute molecules throughout the solution.
• When compared to other petroleum solvents, vegetable oil is considered a non-volatile organic compound (VOC) that have high dissolving power and flash point, together with low toxicity and less environmental impact.

Video Animation: Solute and Solvent (By Stile Education)

Reference

Yara-Varón, E., Li, Y., Balcells, M., Canela-Garayoa, R., Fabiano-Tixier, A. S., & Chemat, F. (2017). Vegetable Oils as Alternative Solvents for Green Oleo-Extraction, Purification, and Formulation of Food and Natural Products. Molecules (Basel, Switzerland), 22(9), 1474. https://doi.org/10.3390/molecules22091474.

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