Solution Properties Concentration - Characteristics, Types, FAQs

Edited By Team Careers360 | Updated on Jul 02, 2025 04:41 PM IST

What is a solution in science and give solution examples?

A solution is a homogenous mixture of two or more substances with particle sizes ranging from 0.1nm to 1 nm. The term "homogeneous" refers to a mixture's components forming a single phase. All the components of a solution appear as a single phase. There is particle homogeneity or a uniform distribution of particles.

This Story also Contains

What is a solution in science and give solution examples?
Characteristics of a solution properties concentration
Different types of solution properties concentration
The Concentration of a solution
Solubility

Spoon Sugar Solution with Glass

A liquid solution is made up of a solid, liquid, or gas that has been dissolved in a liquid solvent. Similarly, a solid solution is made up of a solid, liquid, or gas dissolved in a solid solvent.

Also read -

Characteristics of a solution properties concentration

What is a solute?

Solution definition chemistry and Solution meaning: A solute is a solid, liquid, or gas which is dissolved to make solution. A solute is dissolved in a solvent to make a solution

What is a solvent?

A solvent is the component of a solution in which a solute is dissolved. It is more abundant in solution chemistry than the solute.

What are the properties of the solution?

The following are some of the properties of solutions:

It is a completely homogeneous mixture.
Its particles are too small, with a diameter of less than 1 nm.
The particles cannot be seen with the naked eye.
A beam of light moving through particles does not scatter, therefore the path of the light is not visible.
Filtration cannot separate the constituents of a combination.

Different types of solution properties concentration

1. Based on solute and solvent

The most common type of solution is a liquid, such as sugar in water, but there are also solutions that are gases or solids. During the formation of a solution, any state of matter (solid, liquid, or gas) can act as both a solute and a solvent. As a result, we may divide solutions into nine categories based on the physical states of the solute and solvent.

Sl. No	Types of solution	Examples	Solute	Solvent
1	Solid in solid solution example	Alloys like bonze and brass	Solid	Solid
2	Solid in liquid solution example	The solution of salt and sugar in water.	Solid	Liquid
3	Solid in gas solution example	Sublimation of iodine, camphor in air	Solid	Gas
4	Liquid in solid solution example	Amalgams (mercury in silver )	Liquid	Solid
5	Liquid in liquid solution example	Alcohol in water, benzene in toluene	Liquid	Liquid
6	Liquid in gas solution example	Aerosol	Liquid	Gas
7	Gas in solid solution example	Hydrogen absorbed in palladium	Gas	Solid
8	Gas in liquid solution example	Aerated drinks	Gas	Liquid
9	Gas in gas solution example	Mixture of gases	Gas	Gas

Related Topics Link,

NEET Highest Scoring Chapters & Topics

This ebook serves as a valuable study guide for NEET exams, specifically designed to assist students in light of recent changes and the removal of certain topics from the NEET exam.

Download EBook

Based on quantity of solute in solution

Unsaturated Solution - An unsaturated solution is one in which we can add more solute at given temperature.
Supersaturated Solution - A supersaturated solution is a saturated solution to which more solute is added by increasing the temperature or pressure. Generally, crystals begin to form in these solutions.
Saturated Solution - A saturated solution is one in which no more solute can be dissolved in the solvent at given temperature.

The Concentration of a solution

Concentration meaning in chemistry: The concentration of a solution refers to the amount of solute in a specific solution. In solutions, the proportions of solute and solvent are not equal. A solution can be one of the following, depending on the percentage of solute:

Diluted
Concentrated
Saturated

Concentration of solution = Amount of solute / Amount of solution

A solution's concentration can be expressed both quantitatively and qualitatively. It can be described qualitatively as a dilute solution for or a concentrated solution. It can be stated quantitatively in terms of mass percentage, volume percentage, parts per million, and so on.

Mass Percentage (w/w) = Mass of solute / Total mass of solution × 100
Volume Percentage (v/v) = Volume of solute / Total volume of solution × 100
Mass by volume Percentage (w/v) = Mass of solute(g) / Volume of solution(ml) × 100
Parts per million (ppm) = Number of parts of the component / Total number of parts of all the components of the solution × 10⁶
Mole fraction of solute = Moles of solute / Moles of solute + moles of solvent
Molarity = Moles of solute / Volume of solvent in litre
Molality =Mass of solute / Mass of solvent in kg

Also Read:

Solubility

A solubility of a substance refers to the greatest amount of solvent that may be dissolved in a given amount of solvent at a given temperature.

The Solubility of a Substance is affected by the Following Factors –

Nature of the Solute
The nature of the solvent
Temperature
Pressure

What is a mixture?

Mixtures are compounds made up of two or more different kinds of materials. Mixtures include things like air, earth, blood, and so on. Mixtures are classified as homogeneous or heterogeneous based on the nature of the components and their distribution. A homogeneous mixture is one in which the constituents are evenly distributed. The mixture is called a heterogeneous mixture if the distribution is not uniform. A solution is a mixture of two or more components that is homogeneous.

Also check-

NCERT Chemistry Notes:

Frequently Asked Questions (FAQs)

1. What is the difference between a solute and a solution?

A simple solution is made up of two components that are uniformly mixed together. The solute is one, while the solvent is the other. A dissolving material is referred to as a solute (sugar) and the one who dissolves it is the solvent (water).

2. What exactly is a universal solvent?

A common solvent is a substance in which most compounds dissolve. Because water dissolves more chemicals than any other solvent, it is referred to as the common solvent.

3. Give an example of a saturated solution?

Carbonated water is the example for saturated solution.

4. Give examples of some solutions used in our daily life?

A solution is a mixture in which all of the components have entirely dissolved into each other.

The following are five examples of solutions that we employ in our daily lives:

Sugar & Milk.
Water and Ink
Water with Oxygen.
Salt in Water.
Lemon juice in a glass of water

5. What is the difference between saturated and unsaturated solutions?

A saturated solution occurs when a solution dissolves as much solute as possible at a given temperature. In simpler terms, a saturated solution is one in which no more solute can dissolve itself in the solution at a given temperature. An unsaturated solution is one in which the amount of solute is not equal to, but less than, the saturation level.

6. What is the difference between saturated and unsaturated solutions?

A saturated solution contains the maximum amount of solute that can be dissolved in a given amount of solvent at a specific temperature. No more solute can be dissolved without changing conditions. An unsaturated solution contains less solute than it is capable of dissolving under the given conditions, meaning more solute can still be dissolved.

7. Is air a solution?

Our air is a solution because it is a homogeneous blend of many distinct gases. The solvent for this solution is nitrogen, which makes up around 78 percent of the atmosphere.

8. What is the difference between ideal and non-ideal solutions?

Ideal solutions are theoretical models where the interactions between all particles (solute-solute, solvent-solvent, and solute-solvent) are identical. Non-ideal solutions reflect real-world behavior. Key differences include:

9. How does the concept of partial molar properties help in understanding solution behavior?

Partial molar properties describe how an intensive property of a solution changes with the addition of a component while keeping temperature, pressure, and other component amounts constant. Key points:

10. What is the role of a buffer solution, and how does it maintain pH?

A buffer solution resists changes in pH when small amounts of acid or base are added. It typically consists of a weak acid and its conjugate base (or a weak base and its conjugate acid). Buffers maintain pH by:

11. How does ionic strength affect solution properties?

Ionic strength is a measure of the total ion concentration in a solution, accounting for both the concentration and charge of the ions. It affects solution properties by:

12. How does the presence of electrolytes affect the freezing point depression of a solution?

Electrolytes affect freezing point depression more than non-electrolytes because they dissociate into multiple ions in solution. The freezing point depression depends on the number of particles in solution, not their nature. Therefore:

13. How does the concept of activity coefficient relate to solution concentration?

The activity coefficient is a factor used to account for deviations from ideal behavior in solutions, especially at higher concentrations. It relates the actual behavior of an ion in solution to its behavior in an ideal, infinitely dilute solution. As concentration increases:

14. What is the significance of Raoult's law in solution chemistry?

Raoult's law describes the relationship between the vapor pressure of a solution and the mole fraction of the volatile component. It states that the partial vapor pressure of each component in an ideal solution is equal to the vapor pressure of the pure component multiplied by its mole fraction in the solution. Raoult's law is significant because:

15. How does temperature affect solubility?

Temperature generally affects solubility in the following ways:

16. Can a solution be supersaturated? How?

Yes, a solution can be supersaturated. This occurs when a solution contains more dissolved solute than it can theoretically hold under normal conditions. Supersaturated solutions are unstable and can be created by:

17. How does the nature of solute and solvent affect solubility?

The nature of solute and solvent affects solubility based on the principle "like dissolves like." This means:

18. What is Henry's law, and how does it relate to gas solubility?

Henry's law states that the amount of dissolved gas in a liquid is directly proportional to the partial pressure of the gas above the liquid, at constant temperature. Mathematically, it's expressed as C = kP, where C is the concentration of dissolved gas, k is Henry's constant, and P is the partial pressure of the gas. This law explains why carbonated drinks fizz when opened (reducing pressure) and why deep-sea divers must ascend slowly to avoid decompression sickness.

19. How does concentration relate to solution properties?

Concentration is a measure of how much solute is dissolved in a given amount of solvent or solution. It directly affects various properties of the solution, such as boiling point, freezing point, vapor pressure, and osmotic pressure. Higher concentrations generally lead to more pronounced changes in these properties.

20. What are the most common ways to express concentration?

The most common ways to express concentration are:

21. Why is molarity the most frequently used concentration unit?

Molarity is the most frequently used concentration unit because it's convenient for laboratory work. It relates the amount of solute to the volume of solution, which is easy to measure and manipulate in the lab. Additionally, molarity is directly proportional to the number of particles in solution, making it useful for calculations involving chemical reactions.

22. What is the difference between molarity and molality?

Molarity (M) is defined as moles of solute per liter of solution, while molality (m) is defined as moles of solute per kilogram of solvent. The key differences are:

23. How does the concentration of a solution affect its colligative properties?

Colligative properties are solution properties that depend on the number of dissolved particles, not their nature. As concentration increases:

24. What is a solution in chemistry?

A solution is a homogeneous mixture of two or more substances where one substance (the solute) is dissolved in another substance (the solvent). The particles of the solute are evenly distributed throughout the solvent, creating a uniform composition.

25. How does the concept of fugacity relate to the behavior of real gases in solution?

Fugacity is a measure of the tendency of a substance to escape from a phase, often used to describe real gases. In solutions:

26. How does the concept of preferential interaction coefficient relate to protein stability in solutions?

The preferential interaction coefficient quantifies the preference of a protein to interact with water or cosolvent molecules in a solution. Key points:

27. How does the Gibbs-Donnan effect influence the distribution of ions across semipermeable membranes?

The Gibbs-Donnan effect describes the uneven distribution of ions across a semipermeable membrane when one ion cannot pass through the membrane. Key points:

28. What is the significance of the Kirkwood-Buff theory in solution chemistry?

The Kirkwood-Buff theory provides a framework for relating macroscopic solution properties to microscopic interactions between molecules. Key aspects:

29. How does the concept of activity relate to concentration in non-ideal solutions?

Activity is a measure of the "effective concentration" of a species in a non-ideal solution. It's related to concentration by the activity coefficient (γ):

30. What is the significance of the common-ion effect in solution chemistry?

The common-ion effect occurs when a solute is added to a solution containing one of its ions, leading to a decrease in the solubility of the original solute. It's significant because:

31. How does the Debye-Hückel theory explain the behavior of electrolyte solutions?

The Debye-Hückel theory explains the non-ideal behavior of electrolyte solutions by considering the ionic atmosphere around each ion. Key points include:

32. What is the salting-out effect, and how does it impact solubility?

The salting-out effect is the decrease in solubility of a non-electrolyte in water when an electrolyte is added. It occurs because:

33. What is the Setschenow equation, and how is it used in solution chemistry?

The Setschenow equation describes the salting-out effect quantitatively. It relates the solubility of a non-electrolyte in an electrolyte solution to its solubility in pure water:

34. What is the Hofmeister series, and how does it affect solution properties?

The Hofmeister series is a ranking of ions based on their ability to salt out or salt in proteins and other macromolecules. Key aspects:

35. What is the role of the Pitzer equation in describing electrolyte solutions?

The Pitzer equation is a semi-empirical model for calculating activity coefficients in electrolyte solutions. Key aspects: