Solubility: Definition, Henry’s Law, Factors Affecting, Types, Examples & FAQs

Solubility is a fundamental concept in chemistry that describes the ability of a substance to dissolve in a particular solvent under specific conditions to form a solution. A fluid may or may not dissolve completely in a fluid. Understanding the concept of solubility is essential in many fields of science, including pharmaceuticals, environmental science, and materials science.

What is Solubility?

Solubility Definition

Solubility refers to the greatest amount of solute that can dissolve in a known quantity of solvent at a given temperature.

In a solvent, a solution is a homogeneous mixture of one or more solutes. A common example of a solution is sugar cubes added to a cup of tea or coffee. Solubility is the property that allows sugar molecules to dissolve. As a result, solubility can be defined as the ability of a material (solute) to dissolve in a specific solvent. Any substance dissolved in a solvent, whether solid, liquid, or gas, is referred to as a solute.

Solubility Effects on Reactions

If we dissolve any solute in a solvent then there are three possible result that are as follows :

Dilute Solution: If a solvent has less solute dissolve in forming the solution then this solution is called the Dilute Solution.

Saturated Solution: If a solvent has maximum solute(that can be dissolved without changing the temperature) dissolve in forming the solution then this solution is called the Saturated Solution.

Precipitate Solution: If a solvent we add excess solute then its saturation limit then it forms the solution in which precipitate is formed also called precipitate solution.

Solubility Product

“Solubility product” refers to salts that are only sparingly soluble. It is the maximal product of the molar concentration of the ions produced by the dissociation of the molecule (raised to their proper powers).

The solubility product remains constant at a given temperature. The lower the value of the solubility product, the lower the solubility, and the higher the value of the solubility product, the greater the solubility. The elements that influence solubility vary depending on the condition of the solute:

  • Solubility of Liquids In Liquids
  • Solubility of Solids In Liquids
  • Solubility of Gases In Liquids

Now let’s learn about the same in detail.

Solubility of Liquids In Liquids 

Water is referred to as a universal solvent since it dissolves practically all solutes, with the exception of a few. A substance’s solubility can be influenced by a number of circumstances.

Solubility refers to the development of a new bond between the solute and solvent molecules. Solubility is the highest concentration of solute that dissolves in a known concentration of solvent at a particular temperature in terms of quantity. Solutes are classified as highly soluble, sparingly soluble, or insoluble based on the concentration at which they dissolve in a solvent. It is stated to be soluble if a concentration of 0.1 g or more of a solute can be dissolved in a 100 ml solvent. It is considered to be sparingly soluble when a concentration of less than 0.1 g is dissolved in the solvent. As a result, solubility is defined as a quantitative expression measured in grams per liter (g/L).

Different sorts of solutions can be obtained based on solubility. At a given temperature, a saturated solution is one in which a given amount of solute is entirely soluble in a solvent. A supersaturated solution, on the other hand, is one in which the solute begins to salt out or precipitate once a specific concentration is dissolved at the same temperature.

Solubility is a fundamental concept in chemistry that describes the ability of a substance to dissolve in a particular solvent under specific conditions to form a solution. A fluid may or may not dissolve completely in a fluid. Understanding the concept of solubility is essential in many fields of science, including pharmaceuticals, environmental science, and materials science.

Factors Affecting Solubility of Liquid in Liquid

The factors affecting the Solubility of Liquid in Liquid are discussed below,

Effect of Pressure

Pressure has a significantly greater impact on gases than it does on solids and liquids. When a gas’s partial pressure rises, so does the likelihood of its solubility. CO2 is bottled under high pressure in a soda bottle, for example.

Effect of Temperature

People can boost a solute’s solubility characteristic by adjusting the temperature. At 20° C or 100° C, water generally dissolves solutes. Increased temperature will totally dissolve sparingly soluble solid or liquid compounds. However, in the case of a gaseous substance, temperature affects solubility in the opposite direction, meaning that as the temperature rises, gases expand and escape from their solvent.

Solubility of Solids In Liquids 

Solid solubility has been observed to be dependent on both the composition of the solute and the solvent. People frequently see that some substances, such as sugar and common salt (NaCl), dissolve quickly in water whereas others, such as naphthalene, do not. Only polar solutes prefer to dissolve in polar solvents, while non-polar solvents dissolve only in non-polar solutes, according to different observations and experimental data. As a result, one of the most important elements impacting solubility is the composition of the solvent. The discovery that like dissolves like led to the conclusion that polar solvents dissolve polar solutes and non-polar solvents dissolve non-polar solutes.

Let’s take a closer look at how a solid dissolves in a solvent. Dissolution occurs when a solid solute is given to a solvent and the solute particles dissolve in the solvent. The process of crystallization occurs when solute particles in a solution clash with one another and some of the particles separate from the solution.

Between these two processes, a state of dynamic equilibrium is formed, at which point the number of solute molecules entering the solution equals the number of particles exiting the solution. As a result, at a given temperature and pressure, the concentration of the solute in the solution will remain constant.

A saturated solution is one in which no more solute can dissolve in the solvent at a given temperature and pressure, and it contains the maximum amount of solute. Solubility refers to the concentration of a solute in a solution at a certain temperature and pressure. An unsaturated solution is one in which more solute can be added to the solution.

Solubility is a fundamental concept in chemistry that describes the ability of a substance to dissolve in a particular solvent under specific conditions to form a solution. A fluid may or may not dissolve completely in a fluid. Understanding the concept of solubility is essential in many fields of science, including pharmaceuticals, environmental science, and materials science.

Factors Affecting Solubility of Solids In Liquids

The factors affecting the Solubility of Solids in Liquid are discussed below,

Effect of Temperature

If (∆solH > 0), the solubility of a nearly saturated solution increases as the temperature rises, and if (∆solH < 0), the solubility falls as the temperature rises.

Nature Solute and Solvent

Like disintegrates into like. Anthracene, for example, does not react with sodium chloride. Naphthalene and anthracene, on the other hand, dissolve quickly in benzene, whereas sodium chloride and sugar do not.

Effect of Pressure

Changes in pressure have little effect on solid solubility. This is owing to the fact that solids and liquids are highly incompressible and are essentially unaffected by pressure fluctuations.

Solubility of Gases In Liquids 

The topic of gas solubility in liquids is concerned with the idea of gas dissolving in a solvent. Let’s start with a definition of solubility. Solubility is the greatest amount of solute that may be dissolved in a given solvent at a given temperature for any substance. Our current interest is the solubility of gases in liquids. The gas solubility in liquids is greatly affected by temperature and pressure as well as the nature of the solute and the solvent.

Many gases dissolve quickly in water, while others do not under typical conditions. Oxygen is only slightly soluble in water, whereas HCl or ammonia dissolves quickly.

Solubility is a fundamental concept in chemistry that describes the ability of a substance to dissolve in a particular solvent under specific conditions to form a solution. A fluid may or may not dissolve completely in a fluid. Understanding the concept of solubility is essential in many fields of science, including pharmaceuticals, environmental science, and materials science.

Factors Affecting Solubility of Gases In Liquids

The factors affecting the Solubility of gas in Liquid are discussed below,

Effect of Pressure

It has been discovered that as pressure rises, so does the solubility of a gas in liquids. Consider a system of a gas solution in a solvent in a closed container in a state of dynamic equilibrium to better understand the effect of pressure on gas solubility. Because the solution is now in equilibrium, the rate of gaseous molecules entering it is equal to the rate of gaseous molecules leaving it. As a result, the number of gas molecules in the solution increases until a new equilibrium point is reached. As a result, the solubility of gases increases as the pressure of a gas above the solution rises.

Effect of Temperature

With increasing temperature, gas solubility in liquids decreases. Dissolution is the process by which gas molecules in a liquid dissolve. Heat is emitted throughout the process. When a system’s equilibrium is disturbed, the system readjusts itself in such a way that the effect that caused the change in equilibrium is offset, according to Le Chatelier’s Principle. Because dissolution is an exothermic process, solubility should decrease as the temperature rises, proving Le Chatelier’s Principle.

Henry’s Law

Here, KH is Henry’s Law constant

Applications of Henry’s Law

Henry’s Law is one of the most important laws used in solutions and its various applications are,

  • In the manufacture of carbonated drinks.
  • Climbers and those who live at high altitudes will benefit from Henry’s Law
  • During a deep-water dive a diver uses Henry’s Law to use proper oxygen.

Raoult’s Law (Special Case of Henry’s Law)

According to Raoult’s law, “solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid”. Mathematically it can be written as

One of the components of a gas in a liquid solution is so volatile that it exists as a gas. According to Henry’s law, it is soluble in water.

As a result, Raoult’s law is a specific case of Henry’s law, in which KH equals pi0be dissolved

Examples on Solubility

Example 1: At 313 K, benzene and toluene form perfect solutions A and B. 4 moles of toluene and 1 mole of C6H6 makeup Solution A. Toluene and benzene are equal amounts in Solution B. In each scenario, calculate the total pressure. At 313 K, C6H6 and toluene have vapor pressures of 160 and 60 mm, respectively.

Solution:

PM = PB + PT = (P0B × XB) + (P0T × XT)

PM = 160 × (1/1+4) + 60 × (4/1+4)

PM = 32 + 48

PM = 80 mm

PM = 160 × (92/170) + 60 × (78/170)

PM = 86.588 + 27.529

PM = 114.117 mm

Example 2: Heptane and octane form an ideal solution at 373 K, the vapor pressures of the pure liquids at this temperature are 105.2 kPa and 46.8 kPa respectively. If the solution contains 25g of heptane and 28.5g of octane, calculate the vapor pressure exerted by heptane.

Solution:

Given,

  • Po(C7H16) = 105.2 kPa
  • Po(C8H18) = 46.8 kPa
  • M(C7H16) = 100g mol-1
  • M(C8H18) = 114g mol-1

X{C7H16} = n(C7H16) / {n(C7H16) + n(C8H18)}

X{C7H16}= (25/100) / ((25/100) + (28.5/114))

X{C7H16}= 0.25/0.25 + 0.25

X{C7H16} = 0.5

X{C8H18} = 1 – 0.5 = 0.5

P{C7H16} = 105.2 × 0.5 = 52.60 kPa

FAQs on Solubility

1. What is Solubility in Chemistry?

Solubility is the ability of a substance (solute) to dissolve in a solvent to form a homogenous solution.

2. What Factors Affect Solubility?

The factor that affect the solubility are, Temperature, Pressure, and Chemical Nature.

3. How does Temperature Affect Solubility?

Solubility of solids in liquids increases with temperature, while the solubility of gases in liquids decreases with temperature.

4. How does Pressure Affect Solubility?

Solubility of gases in liquids increases with pressure, while the solubility of solids in liquids is generally unaffected by pressure.

5. What is Solubility Product Constant?

Solubility product constant (Ksp) is a measure of the maximum amount of a solute that can dissolve in a given solvent at a particular temperature and pressure.

6. What is the Difference between an Unsaturated, Saturated, and Supersaturated Solution?

 An unsaturated solution is a solution that contains less than the maximum amount of solute that can dissolve in a solvent. A saturated solution is a solution that contains the maximum amount of solute that can dissolve in a solvent. A supersaturated solution is a solution that contains more solute than is normally possible at a given temperature and pressure.

7. What is “Like Dissolves Like”?

This means that substances with similar polarities or intermolecular forces are more likely to dissolve in each other.

8. What are Effects of Temperature and Pressure on Solubility?

An increase in pressure and temperature contributes to higher solubility in this process. An rise in pressure causes more gas particles to enter the liquid, lowering the partial pressure. As a result, the solubility will rise.

9. What is Solubility Product Constant?

Solubility Constant denoted by Ksp is the equilibrium constant that represents the extent to which a solid solute dissolves in a solution.

Er. Neeraj K.Anand is a freelance mentor and writer who specializes in Engineering & Science subjects. Neeraj Anand received a B.Tech degree in Electronics and Communication Engineering from N.I.T Warangal & M.Tech Post Graduation from IETE, New Delhi. He has over 30 years of teaching experience and serves as the Head of Department of ANAND CLASSES. He concentrated all his energy and experiences in academics and subsequently grew up as one of the best mentors in the country for students aspiring for success in competitive examinations. In parallel, he started a Technical Publication "ANAND TECHNICAL PUBLISHERS" in 2002 and Educational Newspaper "NATIONAL EDUCATION NEWS" in 2014 at Jalandhar. Now he is a Director of leading publication "ANAND TECHNICAL PUBLISHERS", "ANAND CLASSES" and "NATIONAL EDUCATION NEWS". He has published more than hundred books in the field of Physics, Mathematics, Computers and Information Technology. Besides this he has written many books to help students prepare for IIT-JEE and AIPMT entrance exams. He is an executive member of the IEEE (Institute of Electrical & Electronics Engineers. USA) and honorary member of many Indian scientific societies such as Institution of Electronics & Telecommunication Engineers, Aeronautical Society of India, Bioinformatics Institute of India, Institution of Engineers. He has got award from American Biographical Institute Board of International Research in the year 2005.

CBSE Class 12 Chemistry Syllabus Download PDF

Below is the CBSE Class 12 Syllabus along with the marking scheme and time duration of the Chemistry exam.

S.NoTitleNo. of PeriodsMarks
1Solutions107
2Electrochemistry129
3Chemical Kinetics107
4d -and f -Block Elements127
5Coordination Compounds127
6Haloalkanes and Haloarenes106
7Alcohols, Phenols and Ethers106
8Aldehydes, Ketones and Carboxylic Acids108
9Amines106
10Biomolecules127
Total70

CBSE Class 12 Chemistry Practical Syllabus along with Marking Scheme

The following is a breakdown of the marks for practical, project work, class records, and viva. The total number of marks for all parts is 15. The marks for both terms are provided in the table below.

Evaluation Scheme for ExaminationMarks
Volumetric Analysis08
Salt Analysis08
Content-Based Experiment06
Project Work and Viva04
Class record and Viva04
Total30

CBSE Class 12 Chemistry Syllabus (Chapter-wise)

Unit -1: Solutions

  • Raoult's law.
  • Colligative properties - relative lowering of vapour pressure, elevation of boiling point, depression of freezing point, osmotic pressure, determination of molecular masses using colligative properties, abnormal molecular mass.
  • Solutions, Types of solutions, expression of concentration of solutions of solids in liquids, solubility of gases in liquids, solid solutions.
  • Van't Hoff factor.

Unit -2: Electrochemistry

  • Redox reactions, EMF of a cell, standard electrode potential
  • Nernst equation and its application to chemical cells
  • Relation between Gibbs energy change and EMF of a cell
  • Kohlrausch's Law
  • Electrolysis and law of electrolysis (elementary idea)
  • Dry cell-electrolytic cells and Galvanic cells
  • Conductance in electrolytic solutions, specific and molar conductivity, variations of conductivity with concentration.
  • Lead accumulator
  • Fuel cells

Unit -3: Chemical Kinetics

  • Rate of a reaction (Average and instantaneous)
  • Rate law and specific rate constant
  • Integrated rate equations and half-life (only for zerfirst-order order reactions)
  • Concept of collision theory (elementary idea, no mathematical treatment)
  • Factors affecting rate of reaction: concentration, temperature, catalyst;
  • Order and molecularity of a reaction
  • Activation energy
  • Arrhenius equation

Unit -4: d and f Block Elements  

  • Lanthanoids- Electronic configuration, oxidation states, chemical reactivity and lanthanoid contraction and its consequences.
  • Actinoids- Electronic configuration, oxidation states and comparison with lanthanoids.
  • General introduction, electronic configuration, occurrence and characteristics of transition metals, general trends in properties of the first-row transition metals – metallic character, ionization enthalpy, oxidation states, ionic radii, color, catalytic property, magnetic properties, interstitial compounds, alloy formation, preparation and properties of K2Cr2O7 and KMnO4.

Unit -5: Coordination Compounds  

  • Coordination compounds - Introduction, ligands, coordination number, color, magnetic properties and shapes
  • The importance of coordination compounds (in qualitative analysis, extraction of metals and biological system).
  • IUPAC nomenclature of mononuclear coordination compounds.
  • Bonding
  • Werner's theory, VBT, and CFT; structure and stereoisomerism

Unit -6: Haloalkanes and Haloarenes  

  • Haloarenes: Nature of C–X bond, substitution reactions (Directive influence of halogen in monosubstituted compounds only). Uses and environmental effects of - dichloromethane, trichloro methane, tetrachloromethane, iodoform, freons, DDT.
  • Haloalkanes: Nomenclature, nature of C–X bond, physical and chemical properties, optical rotation mechanism of substitution reactions.

Unit -7: Alcohols, Phenols and Ethers   

  • Phenols: Nomenclature, methods of preparation, physical and chemical properties, acidic nature of phenol, electrophilic substitution reactions, uses of phenols.
  • Ethers: Nomenclature, methods of preparation, physical and chemical properties, uses.
  • Alcohols: Nomenclature, methods of preparation, physical and chemical properties (of primary alcohols only), identification of primary, secondary and tertiary alcohols, mechanism of dehydration, and uses with special reference to methanol and ethanol.

Unit -8: Aldehydes, Ketones and Carboxylic Acids   

  • Carboxylic Acids: Nomenclature, acidic nature, methods of preparation, physical and chemical properties; uses.
  • Aldehydes and Ketones: Nomenclature, nature of carbonyl group, methods of preparation, physical and chemical properties, mechanism of nucleophilic addition, the reactivity of alpha hydrogen in aldehydes, uses.

Unit -9: Amines    

  • Diazonium salts: Preparation, chemical reactions and importance in synthetic organic chemistry.
  • Amines: Nomenclature, classification, structure, methods of preparation, physical and chemical properties, uses, and identification of primary, secondary and tertiary amines.

Unit -10: Biomolecules     

  • Proteins -Elementary idea of - amino acids, peptide bond, polypeptides, proteins, structure of proteins - primary, secondary, tertiary structure and quaternary structures (qualitative idea only), denaturation of proteins; enzymes. Hormones - Elementary idea excluding structure.
  • Vitamins - Classification and functions.
  • Carbohydrates - Classification (aldoses and ketoses), monosaccharides (glucose and fructose), D-L configuration oligosaccharides (sucrose, lactose, maltose), polysaccharides (starch, cellulose, glycogen); Importance of carbohydrates.
  • Nucleic Acids: DNA and RNA.

The syllabus is divided into three parts: Part A, Part B, and Part C. Part A consist of Basic Concepts of Chemistry, which covers topics such as atomic structure, chemical bonding, states of matter, and thermochemistry. Part B consists of Topics in Physical Chemistry, which includes topics such as chemical kinetics, equilibrium, and electrochemistry. Part C consists of Topics in Organic Chemistry, which covers topics such as alkanes, alkenes, alkynes, and aromatic compounds.

Basic Concepts of Chemistry:

  • Atomic structure: This section covers the fundamental concepts of atomic structure, including the electronic configuration of atoms, the Bohr model of the atom, and the wave nature of matter.
  • Chemical bonding: This section covers the different types of chemical bonds, including ionic, covalent, and metallic bonds, as well as the concept of hybridization.
  • States of the matter: This section covers the three states of matter - solid, liquid, and gas - and the factors that influence their properties.
  • Thermochemistry: This section covers the principles of thermochemistry, including the laws of thermodynamics and the concept of enthalpy.

Chapters in Physical Chemistry:

  • Chemical kinetics: This section covers the study of the rate of chemical reactions and the factors that influence it, including the concentration of reactants, temperature, and the presence of catalysts.
  • Equilibrium: This section covers the principles of chemical equilibrium, including the concept of Le Chatelier's principle and the equilibrium constant.
  • Electrochemistry: This section covers the principles of electrochemistry, including the concept of half-cell reactions, galvanic cells, and electrolysis.

Chapters in Organic Chemistry:

  • Alkanes: This section covers the properties and reactions of alkanes, including their structure, isomerism, and combustion.
  • Alkenes: This section covers the properties and reactions of alkenes, including their structure, isomerism, and addition reactions.
  • Alkynes: This section covers the properties and reactions of alkynes, including their structure, isomerism, and addition reactions.
  • Aromatic compounds: This section covers the properties and reactions of aromatic compounds, including their structure, isomerism, and electrophilic substitution reactions.

In addition to the topics covered in the syllabus, the CBSE Class 12 Chemistry exam also tests students on their analytical and problem-solving skills, as well as their ability to apply the concepts learned in the classroom to real-world situations.

Students can also check out the Tips for the Class 12 Chemistry Exam. They can easily access the Class 12 study material in one place by visiting the CBSE Class 12 page at ANAND CLASSES (A School Of Competitions). Moreover, to get interactive lessons and study videos, download the ANAND CLASSES (A School Of Competitions) App.

Frequently Asked Questions on CBSE Class 12 Chemistry Syllabus

Q1

How many chapters are there in the CBSE Class 12 Chemistry as per the syllabus?

There are 10 chapters in the CBSE Class 12 Chemistry as per Syllabus. Students can learn all these chapters efficiently using the study materials provided at ANAND CLASSES (A School Of Competitions).

Q2

What is the marking scheme for CBSE Class 12 Chemistry practical exam according to the syllabus?

The marking scheme for CBSE Class 12 Chemistry practical exam, according to the syllabus, is 8 marks for volumetric analysis, 8 marks for salt analysis, 6 marks for the content-based experiment, 4 marks for the project and viva and 4 marks for class record and viva.

Q3

Which is the scoring chapter in Chemistry as per CBSE Class 12 syllabus?

The chapter Electrochemistry in Chemistry is the scoring chapter as per CBSE Class 12 syllabus.