Vitamin Solubility

Molecular Basis for Water Solubility and Fat Solubility

The solubility of organic molecule is often summarized through the phrase, "like disappear like." This way that molecules with many polar groups are much more soluble in polar solvents, and also molecules with couple of or no polar teams (i.e., nonpolar molecules) are an ext soluble in nonpolar solvents. (You encountered these concepts in the "Membranes and also Proteins" experiment and the connected tutorial, "Maintaining the Body"s betterworld2016.org: Dialysis in the Kidneys".) Hence, vitamins are either water-soluble or fat-soluble (soluble in lipids and also nonpolar compounds), depending on their molecule structures. Water-soluble vitamin have numerous polar groups and are for this reason soluble in polar solvents such as water. Fat-soluble vitamin are primarily nonpolar and also hence room soluble in nonpolar solvents such together the fatty (nonpolar) tissue of the body.

You are watching: What is the rule when using polar and nonpolar solvents

What provides polar vitamins dissolve in polar solvents and also nonpolar vitamins soluble in nonpolar solvents? The answer to this question lies in the species of interactions that occur in between the molecule in a solution. Solubility is a complicated phenomenon that depends on the change in cost-free energy (ΔG) of the process. Because that a procedure (in this case, a vitamin dissolving in a solvent) to it is in spontaneous, the adjust in complimentary energy have to be an unfavorable (i.e., ΔG

Thermodynamics of resolution (Solubilization)

The resolution of a substance (solute) can be separated into three steps:
The solute particles should separate native one another. The solvent particles should separate sufficient to make an are for the solute molecules to come in between them. The solute and also solvent corpuscle must communicate to kind the solution.
The free energy (G) explains both the energetics (i.e., the enthalpy H) and the randomness or probability (i.e., the entropy S) the a process ( ΔG=ΔH-TΔS, whereby T is the pure temperature). The enthalpy and also entropy alters that happen in the dissolution process are displayed in figure 2, below. In the dissolved process, steps 1 and 2 (listed above) require energy because interactions in between the particles (solute or solvent) are being broken. Action 3 usually release energy because solute-solvent interactions are being formed. Therefore, the change in enthalpy (ΔH) because that the dissolution procedure (steps 1 v 3) deserve to be either positive or negative, relying on the quantity of power released in action 3 relative to the lot of power required in procedures 1 and 2. In terms of the change in entropy (ΔS) the the dissolved process, many dissolution processes bring about a greater randomness (and therefore rise in entropy). In fact, for a big number of dissolved reactions, the entropic result (the change in randomness) is an ext important 보다 the enthalpic result (the readjust in energy) in identify the spontaneity that the process.


Figure 2

The number on the left schematically shows the enthalpy changes accompanying the three procedures that must happen in order for a solution to form: (1) separation that solute molecules, (2) separation that solvent molecules, and (3) communication of solute and also solvent molecules. The as whole enthalpy change, ΔHsoln, is the sum of the enthalpy alters for each step. In the example shown, ΔHsoln is contempt positive, although it can be positive or an adverse in other cases.

The number on the best schematically shows the large, confident entropy change, ΔSsoln, that occurs when a equipment is formed. (Although ΔSsoln is normally positive, this value could be negative in certain situations entailing the dissolved of strong ions.)

In general, if the solute and solvent interactions space of similar strength (i.e., both polar or both nonpolar), climate the energetics of measures 1 and 2 are comparable to the energetics of step 3. Therefore, the increase in entropy determines spontaneity in the process. However, if the solute and also solvent interactions space of differing toughness (i.e., polar through nonpolar), climate the energetics of procedures 1 and also 2 space much higher than the energetics of action 3. Hence, the rise in entropy the can take place is not enough to get rid of the large increase in enthalpy; thus, the dissolution procedure is nonspontaneous.

To highlight the prominence of ΔH and ΔS in identify the spontaneity the dissolution, let us take into consideration three possible cases:
The polar solute molecule are hosted together by solid dipole-dipole interactions and hydrogen bonds between the polar groups. Hence, the enthalpy change to break these interactions (step 1) is large and hopeful (ΔH1>0). The polar solvent molecule are additionally held together by solid dipole-dipole interactions and also hydrogen bonds, therefore the enthalpy adjust for action 2 is also huge and hopeful (ΔH2>0). The polar teams of the solute molecules can connect favorably v the polar solvent molecules, causing a large, an unfavorable enthalpy readjust for action 3 (ΔH31+ΔH2+ΔH3) is small. The tiny enthalpy adjust (ΔH),together v the optimistic entropy adjust for the process (ΔS), an outcome in a negative totally free energy readjust (ΔG=ΔH-TΔS) for the process; hence, the dissolution wake up spontaneously.

The resolution of a nonpolar solute in a polar solvent.

The nonpolar solute molecule are held together only by weak van der Waals interactions. Hence, the enthalpy readjust to break this interactions (step 1) is small. The polar solvent molecules are held together by strong dipole-dipole interactions and also hydrogen bonds together in example (a), therefore the enthalpy adjust for step 2 is large and confident (ΔH2>0). The nonpolar solute molecules carry out not type strong interactions v the polar solvent molecules; therefore, the negative enthalpy change for action 3 is small and cannot compensate because that the large, confident enthalpy change of step 2. Hence, the all at once enthalpy adjust (ΔH1+ΔH2+ΔH3) is huge and positive. The entropy readjust for the process (ΔS) is not large enough to overcome the enthalpic effect, and so the overall complimentary energy change (ΔG=ΔH-TΔS) is positive. Therefore, the dissolution does not take place spontaneously.

The nonpolar solute molecule are hosted together only by weak van der Waals interactions. Hence, the enthalpy readjust to break these interactions (step 1) is small. The nonpolar solvent molecules are likewise held with each other only by weak van der Waals interactions, therefore the enthalpy readjust for action 2 is likewise small. Even though the solute and solvent particles will likewise not form strong interactions through each other (only valve der Waals interactions, therefore ΔH3 is additionally small), there is very little energy required for procedures 1 and also 2 that should be get over in action 3. Hence, the all at once enthalpy readjust (ΔH1+ΔH2+ΔH3) is small. The small enthalpy change (ΔH), together with the confident entropy readjust for the process (ΔS), an outcome in a negative complimentary energy readjust (ΔG=ΔH-TΔS) for the process; hence, the dissolution wake up spontaneously.

See more: Wait, So What Cheese Can You Eat Manchego When Pregnant ? Manchego, A Great Cheese To Eat When Pregnant

The values outlined in the eco-friendly box above explain why the interactions between molecules favor services of polar vitamins in water and nonpolar vitamin in lipids. The polar vitamins, and also the polar water molecules, have solid intermolecular forces that need to be get over in order because that a equipment to it is in formed, requiring energy. As soon as these polar molecules communicate with each various other (i.e., as soon as the polar vitamin are dissolved in water), solid interactions room formed, publication energy. Hence, the overall enthalpy change (energetics) is small. The small enthalpy change, coupled with a far-reaching increase in randomness (entropy change) as soon as the equipment is formed, allow this solution to type spontaneously. Nonpolar vitamins and nonpolar solvents both have weak intermolecular interactions, for this reason the as whole enthalpy adjust (energetics) is again small. Hence, in the case of nonpolar vitamin dissolving in nonpolar (lipid) solvents, the small enthalpy change, coupled v a far-ranging increase in randomness (entropy change) as soon as the systems is formed, allow this solution to form spontaneously together well. Because that a nonpolar vitamin to dissolve in water, or for a polar vitamin to dissolve in fat, the energy required to get over the early intermolecular forces (i.e., in between the polar vitamin molecules or in between the water molecules) is big and is not counter by the power released as soon as the molecules connect in systems (because there is no solid interaction in between polar and also nonpolar molecules). Hence, in this cases, the enthalpy readjust (energetics) is unfavorable to dissolution, and also the size of this unfavorable enthalpy adjust is too huge to be balance out by the rise in randomness that the solution. Therefore, these services will not type spontaneously. (There are exceptions to the principle "like disappear like," e.g., as soon as the entropy decreases once a equipment is formed; however, this exceptions will not be debated in this tutorial.)

In general, it is feasible to predict whether a vitamin is fat-soluble or water-soluble by analyzing its framework to determine whether polar teams or nonpolar groups predominate. In the structure of calciferol (Vitamin D2), shown in number 3 below, we discover an –OH group attached to a bulky arrangement of hydrocarbon rings and chains. This one polar group is not sufficient to compensate for the much larger nonpolar region. Therefore, calciferol is classified together a fat-soluble vitamin.


Figure 3

This is a 2D ChemDraw depiction of the structure of calciferol, Vitamin D2. Back the molecule has actually one polar hydroxyl group, that is thought about a nonpolar (fat-soluble) vitamin since of the advantage of the nonpolar hydrocarbon region.