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Hansen Solubility Parameters



Like, as we all know, attracts like. So if we have a formula for "like" we can judge the solubility of a polymer in a solvent or the compatibility of a polymer and plasticiser or the stability of a nanoparticle in a solvent dispersion by how alike they are. It starts with evaporation It takes energy (enthalpy of vapourisation) to evaporate a solvent. You get all that energy back when you condense it. If you evaporate a portion of a solvent and then condense in an equal volume of a different solvent, if the two solvents are alike then the energy cost of doing this is minimal and the solvents are miscible. If they are very different then energy in and out don't balance and the miscibility is low. It's more precise to talk of the cohesive energy, E, of a solvent, i.e. how much energy is required to break it apart into gas molecules. If E is broken into 3 components of Dispersion, Polar and Hydrogen-bonding then we get: E = ED + EP + EH We are generally not familiar with cohesive energy. Instead we know the latent heat of vaporization Hv, R the universal gas constant, and T the absolute temperature . The relationship between them is: E = HV - RT Cohesive energy is not so useful on its own. Bigger molecules in a molecular series, not surprisingly, have bigger cohesive energies. To scale them so that molecules in a series are more comparable we need the cohesive energy density which is obtained by dividing by molar volume V: E/V = ED/V + EP/V + EH/V The cohesive energy density is more conveniently handled in terms of the solubility parameter δ where δ=E/V. This gives us the classic formula for Hansen Solubility Parameters where the total parameter, δ, is broken into δD, δP and δH for Dispersion, Polar and Hydrogen-bonding: δ = δD + δP + δH The units of solubility parameters are MPa. Older references use (cal/cc) which are a factor of 2.0455 smaller. The measure of "like" The HSP Distance between two molecules, conventionally called Ra, is the measure of how alike they are. The smaller Ra, the more likely they are to be compatible. The famous formula, used for nearly 50 years is:Ra = 4(δD1-δD2) + (δP1-δP2) + (δH1-δH2) The factor of 4 in front of the ΔδD term has aroused controversy for decades but plausible theoretical reasons and overwhelming experimental evidence show that it is valid. Conveniently it makes HSP plots into nice spheres. If from measurements of "good" and "bad" solvents you can define a sphere of radius Ro which contains all the good solvents, then you can define a Relative Energy Difference, RED, which tells you where you are in solubility space:RED = Ra/R0 Hansen Solubility Parameters in Practice If you know the HSP of your solvents, polymers, plasticisers, pigments, nanoparticles, bio-system... then it is very easy to use the Distance formula to understand solubility, swellability, dispersability, permeation and so forth. You can find plenty of published HSP values on the internet. If there is no solvent with the right balance of HSP, cost, safety, odour etc. (and these days it is very hard to find such solvents) you can create your own by mixing solvents, using the rule that the HSP of the mix is the volume-weighted average of the HSP of the components. And Hansen's method of measuring HSP of unknowns via simple good/bad tests with a range of solvents and fitting to a Sphere is not hard to do. The Excel spreadsheet, improved in 2019 by Dr Manuel Díaz de los Ríos, Director of Derivatives Division, ICIDCA (acknowledged with many thanks!) HSP_Calculations.xlsx allows you to try out many of the basics.




Hansen Solubility Parameters




This page provides a crash course in how "solubility" parameters have a big impact on "adhesion". There is a much fuller explanation about HSP within Practical-Solubility, but use this page to get a quick overview of why you really need to know more about them.


  • The ability of two polymers to intermingle or entangle depends, to a large extent, on how "like" they are. So all we need is an objective measure of likeness - or its opposite, the "distance" between two polymers. There is one scheme that does a good job at this and is described on this page. More details can be found on the Hansen Solubility site. 3 Parameters Rather than rely on simplistic ideas of "hydrophilic/lipophilic" or "polar/non-polar" which are ill-defined terms, HSP use 3 parameters. δD is the "Dispersion" parameter which correlates with the polarisability of a molecule, which in turn correlates with refractive index and van der Waals forces. Molecules like methanol have few polarizable electrons so δD is low but aromatics like toluene have more polarizability and δD is higher. Similarly chlorinated solvents have a high δD because of the polarizable halogen electrons.

  • δP is the "Polar" parameter and correlates with our intuitions about polar groups such as -OH or -C=O. Methanol, and acetone therefore have a relatively high δP and toluene a low value.

  • δH is the "Hydrogen bonding" parameter and is obvious in terms of molecules such as methanol. However, molecules such acetone have a modest δH because the C=O is an acceptor for hydrogen donors.

Every solvent and polymer can be assigned its HSP. If the HSP values are similar then the solvent(s) and polymer(s) are compatible, if they are dissimilar then they are non-compatible. This encapsulates the intuition that "like attracts like". We can easily calculate how alike two molecules, 1 and 2, are from their HSP Distance defined as: Distance2=4(δD1-δD2)2+(δP1-δP2)2+(δH1-δH2)2 Clearly if all 3 parameters for 1 and 2 are very close, then Distance is small and mutual solubility/compatibility is high. If one or more values differ greatly then the Distance is large and mutual solubility is low. For those who are used to the Flory-Huggins χ parameter for thinking about polymer solubility, it is calculated via: χ=MVol*Distance2/4RT where MVol is the molar volume and RT is the usual gas constant times temperature term. For polymer-polymer intermingling (rather than complete mutual solubility which is hard to achieve) the χ parameter can be used to calculate the distance two polymers can reach across the interface, with a lower χ value giving a greater possibility of intermingling. In other words, the HSP Distance is a good guide to polymer intermingling even if (for those who know Painter-Coleman) they are a less good guide to polymer miscibility. Applying HSP The app lets you calculate some HSP distances between common polymers polymers. Simply select a pair and the HSP distance is calculated. Although it is well-known that most polymers (at high MWt) are immiscible, at an interface between them the distance that the polymer chains can intermingle can be significant - even for polymers that aren't very close. This makes the "diffusion" theory of adhesion much more likely (and, in fact, provable). The intermingle distance d is based on the "statistical bond length" (Kuhn length) which for simplicity here can be taken to be equivalent to 5 C-C bond lengths, i.e. 0.7nm. and is given by the Helfand formula: d=b/(6χ)0.5. The transformation of χ from Distance uses a value of 50000 for MVol of the polymers.


A blend of two solvents can often have better solubility properties (lower HSP Distance) than either of the individual solvents which might even be non-solvents for the target materials. With this app you can try out these ideas. Choose a target polymer, then various pairs of solvents and vary their ratio till you get the best match (lowest HSP Distance or Ra): HSP Solvent Blends Acetone [15.5, 10.4, 7]Acetonitrile [15.3, 18, 6.1]Benzyl Alcohol [18.4, 6.3, 13.7]1-Butanol [16, 5.7, 15.8]2-Butanol [15.8, 5.7, 14.5]n-Butyl Acetate [15.8, 3.7, 6.3]Cyclohexane [16.8, 0, 0.2]Cyclohexanol [17.4, 4.1, 13.5]Cyclohexanone [17.8, 8.4, 5.1]Diacetone Alcohol [15.8, 8.2, 10.8]N,N-Dimethyl Acetamide [16.8, 11.5, 10.2]N,N-Dimethyl Formamide (DMF) [17.4, 13.7, 11.3]Dimethyl Sulfoxide (DMSO) [18.4, 16.4, 10.2]1,4-Dioxane [17.5, 1.8, 9]Ethanol [15.8, 8.8, 19.4]Ethyl Acetate [15.8, 5.3, 7.2]Ethyl Benzene [17.8, 0.6, 1.4]Ethyl Lactate [16, 7.6, 12.5]Ethylene Carbonate [18, 21.7, 5.1]Ethylene Glycol [17, 11, 26]Ethylene Glycol Monobutyl Ether [16, 5.1, 12.3]Ethylene Glycol Monomethyl Ether [16, 8.2, 15]gamma-Butyrolactone (GBL) [18, 16.6, 7.4]Heptane [15.3, 0, 0]Hexane [14.9, 0, 0]Iso-Butanol [15.1, 5.7, 15.9]Iso-Propyl Acetate [14.9, 4.5, 8.2]Isophorone [17, 8, 5]d-Limonene [17.2, 1.8, 4.3]Methanol [14.7, 12.3, 22.3]Methyl Acetate [15.5, 7.2, 7.6]Methyl Ethyl Ketone (MEK) [16, 9, 5.1]N-Methyl-2-Pyrrolidone (NMP) [18, 12.3, 7.2]Methylene Chloride [17, 7.3, 7.1]1-Nitropropane [16.6, 12.3, 5.5]2-Propanol [15.8, 6.1, 16.4]1-Propanol [16, 6.8, 17.4]n-Propyl Acetate [15.3, 4.3, 7.6]Propylene Carbonate [20, 18, 4.1]PG Monobutyl Ether [15.3, 4.5, 9.2]PG Monoethyl Ether Acetate [15.6, 6.3, 7.7]PG Monomethyl Ether [15.6, 6.3, 11.6]PG Monomethyl Ether Acetate [15.6, 5.6, 9.8]Tetrahydrofuran (THF) [16.8, 5.7, 8]Toluene [18, 1.4, 2]Water [15.5, 16, 42.3]Xylene [17.6, 1, 3.1]Oxygen [14.7, 0, 0]Radon [17.2, 0, 0] Acetone [15.5, 10.4, 7]Acetonitrile [15.3, 18, 6.1]Benzyl Alcohol [18.4, 6.3, 13.7]1-Butanol [16, 5.7, 15.8]2-Butanol [15.8, 5.7, 14.5]n-Butyl Acetate [15.8, 3.7, 6.3]Cyclohexane [16.8, 0, 0.2]Cyclohexanol [17.4, 4.1, 13.5]Cyclohexanone [17.8, 8.4, 5.1]Diacetone Alcohol [15.8, 8.2, 10.8]N,N-Dimethyl Acetamide [16.8, 11.5, 10.2]N,N-Dimethyl Formamide (DMF) [17.4, 13.7, 11.3]Dimethyl Sulfoxide (DMSO) [18.4, 16.4, 10.2]1,4-Dioxane [17.5, 1.8, 9]Ethanol [15.8, 8.8, 19.4]Ethyl Acetate [15.8, 5.3, 7.2]Ethyl Benzene [17.8, 0.6, 1.4]Ethyl Lactate [16, 7.6, 12.5]Ethylene Carbonate [18, 21.7, 5.1]Ethylene Glycol [17, 11, 26]Ethylene Glycol Monobutyl Ether [16, 5.1, 12.3]Ethylene Glycol Monomethyl Ether [16, 8.2, 15]gamma-Butyrolactone (GBL) [18, 16.6, 7.4]Heptane [15.3, 0, 0]Hexane [14.9, 0, 0]Iso-Butanol [15.1, 5.7, 15.9]Iso-Propyl Acetate [14.9, 4.5, 8.2]Isophorone [17, 8, 5]d-Limonene [17.2, 1.8, 4.3]Methanol [14.7, 12.3, 22.3]Methyl Acetate [15.5, 7.2, 7.6]Methyl Ethyl Ketone (MEK) [16, 9, 5.1]N-Methyl-2-Pyrrolidone (NMP) [18, 12.3, 7.2]Methylene Chloride [17, 7.3, 7.1]1-Nitropropane [16.6, 12.3, 5.5]2-Propanol [15.8, 6.1, 16.4]1-Propanol [16, 6.8, 17.4]n-Propyl Acetate [15.3, 4.3, 7.6]Propylene Carbonate [20, 18, 4.1]PG Monobutyl Ether [15.3, 4.5, 9.2]PG Monoethyl Ether Acetate [15.6, 6.3, 7.7]PG Monomethyl Ether [15.6, 6.3, 11.6]PG Monomethyl Ether Acetate [15.6, 5.6, 9.8]Tetrahydrofuran (THF) [16.8, 5.7, 8]Toluene [18, 1.4, 2]Water [15.5, 16, 42.3]Xylene [17.6, 1, 3.1]Oxygen [14.7, 0, 0]Radon [17.2, 0, 0] Polyethylene (PE) [16.9, 0.8, 2.8]Polypropylene (PP) [18, 0, 1]Polystyrene (PS) [18.5, 4.5, 2.9]Polyvinylchloride (PVC) [19.2, 7.9, 3.4]Polyacrylonitrile (PAN) [22.4, 14.1, 9.1]Polymethylmethacrylate (PMMA) [18.6, 10.5, 5.1]Polyethylmethacrylate (PEMA) [17.6, 9.7, 4]Polycarbonate (PC) [18.2, 5.9, 6.9]Polycaprolactone [17.7, 5, 8.4]Polyvinylacetate (PVA) [17.6, 2.2, 4]Nylon 66 [17.4, 9.9, 14.6]PET [18.2, 6.4, 6.6]Epoxy [17.4, 10.5, 9]Polyvinylbutyral [18.6, 4.4, 13]Polyvinylidenefluoride (PVF) [17, 12.1, 10.2]Polyphenyleneoxide (PPO) [17.9, 3.1, 8.5]Polyurethane (PU) [18.1, 9.3, 4.5]Polysulphone [16, 6, 6.6]Polysilicone [17.2, 3, 3]Polyethersulfone [19, 11, 8]Polyoxymethylene (PON) [17.2, 9.2, 9.8]Polyvinylpyrrolidone (PVP) [17.5, 8, 15]CyclicOlefinCopolymer (COC) [18, 3, 2]Polyethylene oxide (PEO, PEG) [17, 10, 5]Polypropylene oxide (PPO, PPG) [16.5, 9, 7]Polyvinylalcohol (PVOH) [15, 17.2, 17.8]Ethylene-vinylalcohol (EVOH) [15.5, 13, 13]Polylactic acid (PLA) [18.6, 9.9, 6] Solvent 1% Mix HSP Mix Ra When Charles first came up with his HSP scheme he saw that it made a surprising prediction. That two bad solvents (the blue dots in the image) on opposite sides of the HSP Sphere should produce an excellent solvent (green dot in the middle) when mixed 50:50. If his HSP ideas were wrong then mixing two bad solvents would create another bad solvent. When he did the test his ideas were confirmed - you really can make a good solvent from a mixture of bad ones. This is probably the single most useful idea in the whole of HSP. It allows formulators amazing freedom to combine solvents that are attractive in terms of cost, safety, odour, volatility etc. but which are poor solvents for the specific system and create an excellent solvent blend. By being smart with the relative volatilities of the solvents it's possible to make mixes that deliberately crash out the solutes when evaporation starts (the best solvent is more volatile) or crash out one solute component (its best solvent is more volatile) or, alternatively, to make a super-smooth coating by ensuring that the best solvent for the critical component is the least volatile so keeps it in solution up to the last moment. Sticking Together: The Science of Adhesion This 'popular science' book gets to the heart of adhesion science in a gentle and friendly manner. It even has its own YouTube channel!


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