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Solubility - Definition, Examples, Units, FAQs

Solubility - Definition, Examples, Units, FAQs

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

What is Solubility?

A solution may be a homogeneous mixture of 1 or more solutes during a solvent. Sugar cubes added to a cup of tea or coffee may be a common solubility examples of an answer . The property which helps sugar molecules to dissolve is understood as solubility.

Definition of Solubility

The term solubility is often defined as a property of a substance that is often used to dissolve during a given solvent. A solute is any substance which may be either solid or liquid or gas dissolved during a solvent.

Solubility units

Solubility is one of the measures of the amount of chemical substances that can be dissolved in water, usually at a certain temperature. The melting unit is usually mg / L (milligrams per liter) or ppm (parts per million).

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This Story also Contains
  1. What is Solubility?
  2. Sparingly soluble meaning
  3. Solubility Product
  4. 1. Solubility of Liquids In Liquids
  5. 2. Solubility of Solids In Liquids
  6. 3. Solubility of Gases In Liquids
  7. Solubility definition
  8. Examples of solvents

Sparingly soluble meaning

The less soluble substances are those, which reduce the melting. In other words, the material will melt slightly if the amount can be dissolved in 100ml ranges of between 1g and 3.3g.

Solubility Product

The term solubility product is usually applicable for sparingly soluble salts. it's the utmost product of the molarity of the ions (raised to their appropriate powers) which are produced ,thanks to dissociation of the compound. At the given temperature the solubility of a product is constant. Lesser the worth of solubility product indicates lower solubility and better value of solubility product indicates greater solubility.

On the idea of solubility, the factors affecting solubility vary on the state of the solute:

1.Liquids In Liquids

2.Solids In Liquids

3.Gases In Liquids

1. Solubility of Liquids In Liquids

Water is understood as alkahest because it dissolves almost every solute apart from a couple of .

There are certain factors that influence the solubility of a substance.

The concentration of solute always dissolves during a solvent whereas,solutes are categorized into

1.highly soluble,

2.sparingly soluble or insoluble

If a degree of 0.1 g or more of a solute is often dissolved during a 100ml solvent, it's said to be soluble. While a degree below 0.1 g is dissolved within the solvent it's said to be sparingly soluble. Thus, it can be said that solubility expression and is expressed by the unit gram/litre (g/L).

On the opposite hand, a supersaturated solution is those where the solute starts salting out or precipitates after a specific concentration is dissolved at an equivalent temperature.

Factors Affecting Solubility of Liquids in liquids

The solubility of a substance always depends upon the physical and chemical properties of the given substance. In addition to the present , there are a couple of conditions which may manipulate it. Temperature, pressure and therefore the sort of bond and forces between the particles are few among them.

Temperature:

By changing temperature we will increase soluble property of solute. The water dissolves solutes at 20°C or 100°C. Sparingly soluble even liquid substances are often dissolved completely with the help of increasing the temperature.

Pressure:

Gaseous substances are more influenced than solids as compared to liquids by pressure. When the partial pressure of gas increases, the prospect of its solubility is additionally increased. A pop bottle is an examples of soluble substances are where CO2 is bottled under high .

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2. Solubility of Solids In Liquids

It has been observed that solid solubility depends on the character of the solute also because of the solvent. We frequently see that substances like sugar, common salt (NaCl), etc readily dissolve in water soluble substances; while substances like naphthalene don't dissolve in water. From the varied observations and experimental results, it's been seen that only polar solutes tend to dissolve within the polar solvent and non-polar solvents dissolve only nonpolar solutes. Hence, the character of the solvent is often seen together with prominent factors affecting solubility.

Now allow us to understand the method by which a solid dissolves during a solvent. Once a solid solute is added to a solvent, the solute particles dissolve within the solvent and this process is understood as dissolution. Solute particles within the solution hit one another and a few of those particles get separated out of the answer , this process is named crystallization.

A state of dynamic equilibrium is established between these two processes and now , the amount of solute molecules entering the answer becomes adequate to the amount of particles leaving the answer . As a result, the concentration of the solute within the solution will remain constant at a given temperature and pressure. A solution during which no more solute can dissolve within the solvent at a given temperature and pressure is claimed to be a saturated solution because the solution contains the utmost amount of solute. The concentration of solute in such an answer is named its solubility at that temperature and pressure. If more solutes are often added to an answer then it's called an unsaturated solution.

Factors Affecting Solubility of Solid in Liquids

Effect of Temperature:

Apart from the character of solute as well as solvent, temperature also affects solid solubility considerably Le Chatelier's Principle. If the given dissolution process is exothermic then the solid solubility should decrease.

Effect of Pressure:

Solid solubility hardly suffers from changes in pressure. This is often thanks to the very fact that solids and liquids are highly incompressible and practically don't suffer from changes in pressure.

3. Solubility of Gases In Liquids

Gas solubility in liquids always deals with the concept of a gas dissolving during a solvent. allow us to first define solubility.

The gas solubility in liquids is greatly suffering from temperature and pressure also because of the nature of the solute and therefore the solvent.

Factors Affecting Solubility of Gases in Liquids

Effect of Pressure:

It is found that the gas solubility in liquids always increases with increase in pressure. to possess a far better understanding of the effect of pressure on gas solubility allow us to consider a system of a gas solution during a solvent during a closed container during a state of dynamic equilibrium. Now the answer is in equilibrium and hence the speed of gaseous molecules entering the answer is adequate to the speed of gaseous molecules leaving the answer .Since the amount of gas molecules presented above the answer has increased, the speed with which the gas molecules are going to be entering the answer also will increase. The top results arise within the number of gas molecules within the solution until a replacement equilibrium point is attained. Thus the solubility of gases increases with a rise within the pressure of a gas above the answer .

Additional information about The solubility of gases in liquids

Henry’s Law gives a magnitude relation between pressure and gas solubility during a liquid. It states that:

Solubility of a gas during a liquid is always directly proportional to the partial pressure of the gas that is present above the surface of liquid.

P = KHx

Here, p = The partial pressure of the gas

x = mole fraction of the gas in solution

KH = Henry’s law constant

Effect of Temperature:

Gas solubility of liquids is found to decrease with the increase in temperature. The gas molecules during a liquid are dissolved by the method of dissolution. During this process, heat evolves. consistent with Le Chatelier’s Principle which states that when equilibrium of a system is disturbed.

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Solubility definition

Moisture is the substance of a solid, liquid or gaseous substance called solute to dissolve in solid, liquid or gaseous solvents.

Solubility examples

Items such as salt, sugar and coffee will dissolve in water. They melt. They also dissolve faster and even better in warm water. Pepper and sand do not melt, they will not melt even in hot water.

Salt, ethanol and sugar are examples of solvents and oils, examples of chloride and mirrors of soluble substances.

Examples of solvents

Substances, like sugar, salt, alcohol and even other dishwashing materials are included under solvents

Soluble substances in water

Items such as salt, sugar and coffee will dissolve in water. They melt. They even dissolve better in warm water. Pepper and sand do not melt, they will not melt even in hot water. Other examples would be sugar, salt, ethanol, and soaps. In chemistry, dissolving a substance is a relative term that refers to the amount of soluble substances in a given solvent volume.

Solubility expression

Solubility is often portrayed as torture; for example, as g per solute per kg of solvent, g per dL (100 mL) of solvent, molarity, molality, mole fraction, etc.

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Frequently Asked Questions (FAQs)

1. 1.Why is the solubility test important?

The presence of fundamental and acidic functional groups are often inferred by solubility measures. The solubility of a compound in aqueous acid or base requires the compound’s ionisation and, thus, a reaction .

2. 2.What causes solubility?

Usually, the solubility of a given solute during a given solvent depends on temperature.They vibrate faster as water molecules heat up, and are better ready to communicate with and split the answer apart.

3. 3.Does pH affect solubility?

The solubility of the solute can affect the pH of a solution . If the solution’s pH is such that no net electrical charge is borne by a selected molecule, the answer also has minimal solubility and precipitates out of the answer.

4. 4.Does temperature affect solubility?

The solubility increases with temperature, surely solids that are dissolved in liquid water. the increase in higher temperature K.E. helps the solvent molecules to interrupt; solute molecules which are kept together by intermolecular attraction more effectively.

5. 5.How does temperature and pressure affect solubility?

In this reaction, an increase in pressure and a rise in temperature contributes to greater solubility. To decrease the partial pressure, a rise in pressure leads to more gas particles entering the liquid. The solubility will, therefore, increase.

6. How does the structure of organic molecules influence their solubility in water?
The solubility of organic molecules in water is influenced by their structure, particularly the presence of polar groups. Molecules with more polar groups (like -OH, -NH2, -COOH) tend to be more soluble in water, while those with long hydrocarbon chains are less soluble.
7. How do surfactants affect the solubility of substances?
Surfactants can increase the solubility of nonpolar substances in polar solvents (like water) by forming micelles. The hydrophobic parts of surfactant molecules surround the nonpolar substance, while their hydrophilic parts interact with water, effectively solubilizing the substance.
8. What is the role of co-solvents in pharmaceutical solubility enhancement?
Co-solvents are secondary solvents added to increase the solubility of a substance in the primary solvent. In pharmaceuticals, they're used to enhance the solubility of drugs that are poorly soluble in water. Common co-solvents include ethanol, propylene glycol, and glycerin.
9. How does the presence of multiple solutes affect the solubility of each other?
The presence of multiple solutes can affect each other's solubility through various mechanisms. They may compete for solvation, alter the solvent properties, or interact with each other. This can lead to either increased or decreased solubility compared to single-solute systems.
10. How does the concept of salting-in differ from salting-out?
While salting-out decreases solubility, salting-in increases it. Salting-in occurs when the addition of an electrolyte increases the solubility of a non-electrolyte. This can happen when the added ions interact more strongly with the solute than with water, effectively increasing the solute's affinity for the solution.
11. Can a solution become supersaturated? How?
Yes, a solution can become supersaturated by containing more dissolved solute than is normally possible under given conditions. This can occur by cooling a saturated solution slowly and carefully, or by removing solvent from a saturated solution without disturbing it.
12. How does the size of solute particles affect solubility?
Generally, smaller solute particles have higher solubility than larger ones. This is because smaller particles have a higher surface area-to-volume ratio, allowing more effective interaction with solvent molecules and easier dissolution.
13. How do common ion effects influence solubility?
The common ion effect decreases the solubility of a sparingly soluble salt when another soluble compound with a common ion is added to the solution. This is due to Le Chatelier's principle, as the increased concentration of the common ion shifts the equilibrium towards the solid phase.
14. What is a solubility curve?
A solubility curve is a graph showing how the solubility of a substance changes with temperature. It typically shows temperature on the x-axis and solubility on the y-axis, allowing quick determination of solubility at different temperatures.
15. How does the concept of entropy relate to solubility?
Entropy, a measure of disorder in a system, often increases during dissolution as molecules become more randomly distributed. This increase in entropy can drive the dissolution process, especially for ionic compounds in water, contributing to their high solubility.
16. How does pressure affect the solubility of gases in liquids?
For gases dissolving in liquids, solubility generally increases with increasing pressure. This relationship is described by Henry's Law, which states that the amount of dissolved gas is proportional to its partial pressure above the liquid.
17. How does temperature affect solubility?
For most solid solutes in liquid solvents, solubility increases with temperature. This is because higher temperatures provide more energy for breaking intermolecular bonds. However, for gases in liquids, solubility typically decreases with increasing temperature.
18. What is the role of intermolecular forces in solubility?
Intermolecular forces play a crucial role in solubility. The solubility of a substance depends on the balance between the attractive forces between solute-solute, solvent-solvent, and solute-solvent molecules. Higher solute-solvent attraction generally leads to greater solubility.
19. What is meant by "salting out" in solubility?
"Salting out" refers to the decrease in solubility of a non-electrolyte in water when an electrolyte is added. The added ions attract water molecules, reducing the amount of water available to dissolve the non-electrolyte, effectively decreasing its solubility.
20. What is the role of solvation in the process of dissolution?
Solvation is the process where solvent molecules surround and interact with solute particles. It's crucial for dissolution as it helps overcome the attractive forces between solute particles. The energy released during solvation can offset the energy required to break solute-solute interactions.
21. What is meant by "like dissolves like" in solubility?
"Like dissolves like" is a general rule in chemistry stating that substances with similar polarity tend to dissolve in each other. For example, polar substances dissolve well in polar solvents, while nonpolar substances dissolve better in nonpolar solvents.
22. How does polarity of the solvent affect solubility?
The polarity of the solvent greatly affects solubility. Polar solvents like water dissolve polar and ionic compounds well, while nonpolar solvents like hexane dissolve nonpolar compounds better. This is due to the "like dissolves like" principle.
23. How does solubility relate to the concept of hydrophobicity and hydrophilicity?
Hydrophilic substances, which are "water-loving" and often polar, tend to have high solubility in water. Hydrophobic substances, which are "water-fearing" and usually nonpolar, have low solubility in water but may be soluble in nonpolar solvents.
24. What is the relationship between solubility and the colligative properties of solutions?
Solubility affects colligative properties like boiling point elevation and freezing point depression. More soluble substances create solutions with a higher concentration of particles, leading to greater changes in these properties compared to the pure solvent.
25. How does the concept of hard and soft acids and bases (HSAB) relate to solubility?
The HSAB concept helps predict solubility trends. Hard acids tend to form stronger bonds with hard bases, while soft acids bond more strongly with soft bases. This principle can be used to predict the solubility of various compounds in different solvents.
26. What is the solubility product (Ksp)?
The solubility product (Ksp) is the equilibrium constant for a solid substance dissolving in an aqueous solution. It represents the product of the concentrations of the ions in a saturated solution raised to the power of their stoichiometric coefficients.
27. What is the significance of the solubility product in precipitation reactions?
The solubility product (Ksp) is crucial in predicting whether a precipitate will form when solutions are mixed. If the ion product exceeds the Ksp, precipitation occurs. This concept is important in qualitative analysis and in understanding natural water chemistry.
28. How does the concept of dynamic equilibrium apply to solubility?
In a saturated solution, there's a dynamic equilibrium between the dissolution and crystallization processes. The rate at which solute particles enter the solution equals the rate at which they return to the solid phase, maintaining a constant concentration of dissolved solute.
29. What is the relationship between solubility and crystal lattice energy?
There's an inverse relationship between solubility and crystal lattice energy. Compounds with high lattice energies tend to have lower solubilities because more energy is required to break the strong intermolecular forces in the crystal structure.
30. How does pH affect the solubility of weak acids and bases?
The pH of a solution can significantly affect the solubility of weak acids and bases. Generally, acids are more soluble in basic solutions, while bases are more soluble in acidic solutions. This is due to the formation of salt and shifts in equilibrium.
31. How is solubility different from dissolution?
Solubility is a property of a substance that describes its maximum ability to dissolve, while dissolution is the process of a substance dissolving. Solubility is quantitative and has a limit, whereas dissolution is the act of dissolving and can occur below the solubility limit.
32. What is the difference between a saturated and an unsaturated solution?
A saturated solution contains the maximum amount of dissolved solute possible at a given temperature and pressure. An unsaturated solution contains less than the maximum amount of solute and can dissolve more if added.
33. What is the difference between solubility and miscibility?
Solubility refers to the maximum amount of solute that can dissolve in a solvent, typically for solid-liquid or gas-liquid systems. Miscibility describes the ability of two liquids to mix in all proportions, forming a homogeneous solution.
34. What are the common units used to express solubility?
Solubility is often expressed in grams of solute per 100 grams of solvent (g/100g), grams per liter (g/L), moles per liter (mol/L), or parts per million (ppm). The choice of unit depends on the context and the concentration of the solution.
35. What is the difference between intrinsic and apparent solubility?
Intrinsic solubility is the solubility of the neutral form of a compound, while apparent solubility includes all species of the compound (ionized and un-ionized) present in solution. For ionizable compounds, apparent solubility can be much higher than intrinsic solubility, especially at certain pH values.
36. How does solubility relate to the concept of solubility equilibrium?
Solubility equilibrium refers to the dynamic balance between the dissolved and undissolved solute in a saturated solution. The solubility product constant (Ksp) quantifies this equilibrium, helping predict whether precipitation will occur under given conditions.
37. What is the significance of the common ion effect in environmental chemistry?
The common ion effect is significant in environmental chemistry, particularly in water systems. It can influence the solubility of minerals in natural waters, affect the bioavailability of nutrients and pollutants, and play a role in the formation of scale in pipes and industrial equipment.
38. How does solubility relate to the concept of partition coefficient in drug absorption?
The partition coefficient, often expressed as log P, measures a compound's differential solubility in two immiscible phases (usually octanol and water). It's crucial in predicting drug absorption, as it indicates how easily a drug can cross biological membranes. Compounds with optimal log P values tend to have better absorption.
39. What is the significance of retrograde solubility?
Retrograde solubility refers to the unusual behavior where a substance's solubility decreases as temperature increases. This is important in various industrial processes, particularly in the formation of scale in boilers and heat exchangers, where compounds like calcium sulfate become less soluble at higher temperatures.
40. How does solubility relate to the concept of fractional crystallization?
Fractional crystallization exploits differences in solubility to separate and purify compounds. As a solution cools or evaporates, compounds with lower solubility crystallize first. By carefully controlling conditions, mixtures can be separated based on their differing solubilities at various temperatures.
41. What is solubility?
Solubility is the maximum amount of a substance (solute) that can dissolve in a given amount of solvent at a specific temperature and pressure. It represents the point at which a solution becomes saturated and no more solute can dissolve.
42. What is the relationship between solubility and the Gibbs free energy of solvation?
The Gibbs free energy of solvation (ΔGsolv) is directly related to solubility. A negative ΔGsolv indicates a spontaneous dissolution process and higher solubility. The more negative the ΔGsolv, the more soluble the substance tends to be in that solvent.
43. How does the concept of solubility relate to the formation of inclusion compounds?
Inclusion compounds, such as cyclodextrins, can enhance the apparent solubility of poorly soluble compounds by forming host-guest complexes. The hydrophobic cavity of the host molecule can accommodate hydrophobic guest molecules, while the hydrophilic exterior allows the complex to dissolve in aqueous media.
44. How does solubility relate to the concept of supersaturation in crystal growth?
Supersaturation, where a solution contains more dissolved solute than its equilibrium solubility, is crucial for crystal growth. As the solution is supersaturated, solute molecules tend to come out of solution and form crystals. The degree of supersaturation affects the rate and nature of crystal formation.
45. What is the relationship between solubility and the concept of hydrotropy?
Hydrotropy is a solubilization phenomenon where the addition of a large amount of a second solute (hydrotrope) increases the aqueous solubility of a poorly soluble compound. Unlike micelle formation in surfactants, hydrotropes aggregate at higher concentrations and can enhance solubility through various mechanisms.
46. What is the significance of the heat of solution in solubility?
The heat of solution is the energy change when a substance dissolves. Exothermic dissolution processes (negative heat of solution) often lead to decreased solubility with increasing temperature, while endothermic processes typically show increased solubility with temperature.
47. What is the role of complexation in enhancing solubility?
Complexation can significantly enhance solubility, especially for metal ions. When a ligand forms a complex with a metal ion, it can make the ion more soluble in the solvent. This principle is used in various applications, including water treatment and metal extraction.
48. How does solubility relate to the concept of solvent extraction in analytical chemistry?
Solvent extraction in analytical chemistry relies on the differential solubility of compounds in two immiscible solvents. By choosing appropriate solvents, analysts can selectively extract and separate compounds based on their relative solubilities, which is crucial for purification and analysis techniques.
49. What is the significance of the Hofmeister series in solubility?
The Hofmeister series ranks ions based on their ability to salt out or salt in proteins and other macromolecules. It's significant in understanding how different ions affect the solubility and stability of proteins, with implications in biochemistry, pharmaceuticals, and colloid science.
50. What is the role of solubility in the formation of solid solutions?
Solid solutions form when one substance dissolves in another in the solid state. The solubility of one component in the crystal lattice of another determines the extent of solid solution formation. This concept is crucial in materials science, particularly in the development of alloys and doped semiconductors.
51. How does the concept of solubility apply to gas chromatography?
In gas chromatography, solubility plays a role in the partitioning of analytes between the mobile gas phase and the stationary liquid phase. Compounds with higher solubility in the stationary phase will be retained longer, affecting their retention times and separation from other analytes.
52. What is the significance of solubility in the context of drug polymorphism?
Different polymorphs of a drug can have varying solubilities, which can significantly affect bioavailability and efficacy. Understanding and controlling polymorphism is crucial in pharmaceutical development, as the most soluble polymorph is often desired for optimal drug performance.
53. How does solubility relate to the concept of critical solution temperature?
The critical solution temperature is the temperature at which two liquids become completely miscible. Below (or above) this temperature, the liquids have limited solubility in each other. This concept is important in understanding phase behavior of liquid mixtures and in industrial separation processes.
54. What is the role of solubility in the formation of aerosols and atmospheric chemistry?
Solubility plays a crucial role in aerosol formation and atmospheric chemistry. The solubility of gases in water droplets affects cloud formation and acid rain. Additionally, the solubility of particulate matter in atmospheric moisture influences air quality and the transport of pollutants.
55. How does the concept of solubility apply to the phenomenon of osmosis?
Solubility is fundamental to osmosis, as it determines the concentration of solutes in solutions. Differences in solute concentration (and thus solubility) between two solutions separated by a semipermeable membrane drive the osmotic flow of solvent. This principle is crucial in biological systems and various industrial applications like desalination.

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Questions related to

Have a question related to ?

Question : Which chemical law proposes that "soft drinks and soda bottles are sealed under high pressure to increase the solubility of CO2?"

Option 1: Dalton’s Law

Option 2: Henry's Law

Option 3: Ohm's Law

Option 4: Raoult’s Law

Correct Answer: Henry's Law


Solution : The correct answer is Henry's Law.

Henry's Law is one of the gas laws formulated by the British chemist William Henry in 1803.

According to Henry's Law, the solubility of a gas in a liquid is directly proportional to the pressure of the gas. So, to increase the solubility of CO2 in soft drinks, the bottle is sealed under high pressure.

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Team Careers360 25 January,2024

Question : Solubility of gases in liquids ______ with a decrease in temperature.

Option 1: remains constant

Option 2: first decreases and then increases

Option 3: increases

Option 4: decreases

Correct Answer: increases


Solution : The correct answer is increases.

The partial pressure of a gas above the liquid or solution's surface determines how soluble the gas is in the liquid. The solution's temperature: as the temperature drops, gases become more soluble in liquids.

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Team Careers360 17 January,2024
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