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Microcalorimetry Techniques for Studying Interactions at Solid-Liquid Interface: A Review

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19 February 2024

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20 February 2024

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Abstract
Solid-liquid interfacial phenomena play an essential role in our everyday lives and are often regarded as the outcome of interactions at the solid-liquid interface. However, the intricately intrinsic mechanism underlying interfacial interactions renders in-situ simulations and direct measurements challenging. As an effective analytic method for studying solid-liquid interfacial interactions, Microcalorimetry can provide the most basic thermodynamic information (including changes in enthalpy, entropy, and Gibbs free energy during solid-liquid binding/separation processes), which is extremely crucial for understanding interaction directionality and limitation. This review is dedicated to highlighting the pivotal role of microcalorimetry in studying solid-liquid immersion and adsorption processes. Specifically, we provide an overview of the commonly employed microcalorimetric methods, delve into the influence factors of enthalpy change, and finally discuss the specific applications of microcalorimetry in studying various solid-liquid binding processes. There remains a vast expanse of thermodynamic information regarding solid-liquid interactions that await exploration via calorimetry.
Keywords: 
Subject: Chemistry and Materials Science  -   Physical Chemistry

1. Introduction

The solid-liquid interfacial phenomena are common occurrence in nature and human activities. For example, agglomerated water droplets on a lotus leaf, rain wetting the road surface, and the paint is required to spread evenly on the wall without falling off or forming bubbles. Fundamentally speaking, the interfacial phenomenon is resulted from the intermolecular interactions (covalent interaction or noncovalent interaction) at solid-liquid interface. Great progress has been achieved in the characterization techniques for studying solid-liquid interfacial interaction since 1900s. Macroscopic analytic methods include the contact angle of the liquid on the solid surface, the zeta potential of the solid, and the interfacial tension between solid and liquid, et al. Microscopic interaction information such as surface images, intermolecular forces, molecular orientations and vibration frequencies can be obtained through atomic force microscopy (AFM) [1,2,3], scanning tunneling microscopy (STM) [4,5], sum frequency generation spectroscopy (SFG) [6,7], infrared spectroscopy (IR) [8,9], and magnetic resonance imaging (MRI) [10]. Calorimetry is an experimental technique and serves as an essential means to probe solid-liquid interactions from a thermodynamic perspective. It enables the interaction process to be tracked and quantified through directly measuring the associated enthalpy change. Most binding processes at the solid-liquid interface involve intermolecular interactions dominated by non-covalent forces, such as hydrogen bonding and van der Waals interactions, representing a distinctive type of process. Based on the heat partitioning measured by calorimetry, prevalent techniques include Isothermal Titration Calorimetry (ITC), Differential Scanning Calorimetry (DSC) [11], and Immersion Calorimetry (IM). These calorimetric methods allow us to gather heat information during various solid-liquid interface interactions. Immersion enthalpy stands out as the most pivotal parameter in the solid-liquid immersion process, exclusively measured by the heat emitted or absorbed during solid-liquid binding via titration calorimetry and immersion calorimetry. This then allows the determination of changes in enthalpy, entropy, and Gibbs free energy. However, these two calorimetric methods still face two inherent challenges. The first pertains to the fact that the heat obtained from these microcalorimetric tests represents the total heat of the entire process, lacking differentiation for specifics, such as the diffusion process or particular binding sites, which leads to the second issue concerning the theoretical validity of these thermodynamic concepts owing to that minute errors can become amplified during derivations using thermodynamics. Thus, it is imperative to select appropriate materials for various experiments when utilizing calorimetry to investigate the interactions between solids and liquids at their interface, which aids in distinguishing the distinct impacts of dissolution, diffusion, and adsorption processes on the overall heat. Furthermore, it is essential to consider any potential experimental inaccuracies to attain more precise when determining thermodynamic values.

2. Fundamental Principles of ITC and DSC

The heat obtained via calorimetry is a process function, implying that the heat in a given process will depend on the constraints of the study in question. Both ITC and IM measure processes carried out at constant temperature (T) using a thermostat and constant pressure (P) using a pressure stabilizer. Under these constraints, the process is isothermal and isobaric, meaning the associated heat will be equivalent to the change in enthalpy (ΔH) of the system. The Gibbs energy (G) is the thermodynamic potential controlling system equilibrium, and its change (ΔG) determines the feasibility or spontaneity of a given process under constant temperature and pressure. The equilibrium constant (Ke) ascertains the system’s composition at equilibrium and quantifies the tendency to form the final products. ΔG0 is associated with the standard Gibbs energy of the process.
Δ G 0 =   – RT   ln K e  
The affinity of a given interaction can be quantified using the equilibrium binding constant (Ka), equilibrium dissociation constant (Kd), and the Gibbs free energy of binding. A more negative Gibbs free energy indicates a higher affinity between the solid and liquid and better intermolecular binding stability at the solid-liquid interface. Microcalorimetric methods refer to calorimetric techniques capable of detecting extremely minute heat changes during a process. From this perspective, DSC, ITC, and IM can all be termed microcalorimetric methods. With technological advancements, calorimetry is no longer a technique confined to specialized labs using custom-built instruments and all available devices offer automated titrations in computer-controlled experiments, running in parallel with automated data collection. Sample loading and instrument cleaning can be accomplished manually, but some newer models possess semi-automatic maintenance kits and scripts, enabling automatic cleaning and minimizing operator intervention to the greatest extent possible.
The sample and reference cells of the ITC are enclosed within an insulating jacket, isolating them from the surrounding environment and maintaining a constant temperature (Figure 1) [12]. A stepping motor within the syringe holder controls the plunger of the airtight syringe, introducing the titrant into the sample cell. In addition, stirring ensures rapid mixing with the sample after each titrant addition. The temperature difference between the sample and reference cells is transformed into a voltage signal by thermocouples, which are then converted into a heat power signal. During an ITC measurement, titration is performed under constant temperature and pressure, gradually mixing one reactant into another while simultaneously measuring the heat associated with the binding reaction [13]. ITC is currently mainly used in the biological field for measuring interactions between proteins [14], proteins and nucleic acids [15], and proteins and lipids [16]. Some studies have also employed ITC for investigating the binding of solid substances such as activated carbon [17], Metal Organic Frameworks (MOFs) materials [18,19,20], and rare earth [21] with liquids. Considering the general solid-liquid binding process, it might be accompanied by equilibriums of numerous different solid surface sites with liquid molecules. If an experiment is conducted under a single set of conditions, then all binding parameters estimated and used to characterize the interaction must be considered as apparent binding parameters. On account of ITC measures the total heat change encompassing all processes involved in the interaction, no further binding information can be inferred without additional experiments to clarify the contributions of different processes to the total heat. For instance, supposing activated carbon surface possesses both hydroxyl and carboxyl groups, these active sites would have different heat release contributions when binding with water. Typically, the binding process is described using total enthalpy and total entropy, wherein such a description seems overly simplistic and it’s controversial over the general validity and usefulness of the interpretation of binding parameters [22,23,24]. Additionally, IM method, similar to ITC, measures the heat released when a certain amount of solid is fully immersed in a liquid under isothermal and isobaric conditions.
DSC is a technique to measure the relationship of temperature/time with input energy difference between the sample and the reference material wherein temperature is programmatically controlled within a specified range, exactly as the ICTAC Nomenclature Committee defines DSC as “a technique measuring the difference in heat flow between the sample and a reference material” [26]. In simpler terms, DSC measures the heat released or absorbed by a substance during its heating or cooling process. DSC has been extensively employed in characterizing and studying pharmaceuticals [27], graphite [28], and polymers [29] and so on. Heat flux DSC is the most commonly used method, in which the heat flows the reference and sample simultaneously through an electrically heated Constantine thermoelectric disk (Figure 2). Commonly recorded data includes the glass transition temperature (Tg), melting temperature (Tm), and crystallization temperature (Tc). Furthermore, physical and chemical changes detected by DSC might encompass phase transitions, glass transitions, denaturation, melting, crystallization, and other characteristics like polymer transformations, oxidations, decompositions (either oxidatively or otherwise), thermal curing, and annealing. All these above transitions can be both qualitatively and quantitatively detected through DSC measurement. Such insights hold significance for the synthesis and development of new products [30], as well as for exploring the viability of applications ranging from food and drugs to novel materials. César Leyva Porras et al. [31] elucidated how DSC is employed for investigating intricate solid/solid and liquid/liquid interactions in food and medicines. There are also pertinent studies [32] highlighting the use of DSC in the characterization of graphene-based materials and understanding of solid-surface state at the molecular scale. Due to its own inherent characteristics, DSC predominantly focuses on the characterization of solid materials and its application in studying solid-liquid interface interactions is comparatively rare. For certain solids that adsorb liquids, immersion calorimetry can measure the heat changes during the adsorption and desorption processes of the solid onto the liquid. The binding or adsorption behaviors occurred during the solid-liquid immersion process are mainly explored through Isothermal Titration Calorimetry and immersion calorimetry.

3. Calorimetric Insights into Enthalpy Changes during Solid-Liquid Immersion Processes

The process of solid-liquid immersion refers to the transformation of the gas-solid interface into a liquid-solid interface. Typically, if we assume the immersion area to be a unit surface area, the reduction in Gibbs function of the system during this process equates to the difference between the solid-liquid interfacial tension and the solid surface tension under isothermal and isobaric conditions, which also represents the immersion capacity countering the contraction of the liquid surface. The heat released during immersion under constant pressure, is termed immersion enthalpy. So, what does the magnitude of the immersion enthalpy signify, and what insights regarding the solid-liquid interface can be deduced from the immersion enthalpy? Addressing these questions necessitate a discussion on the factors influencing immersion enthalpy. Rouquerol et al. [33] proposed that when a solid surface is degassed under a vacuum prior to measurement, the immersion enthalpy predominantly depends on the following parameters: (1) The accessible surface area of the solid. For a given solid-liquid system, immersion enthalpy increases with the augmentation of the available surface area. (2) The chemical nature of the liquid and the solid surface. Specific interaction between the solid surface and the liquid can enhances the immersion enthalpy. (3) The porous structure of the solid. Enhanced interactions can lead to an increase in immersion enthalpy when the molecular size of the liquid is proximate to the pore size. Additionally, the congruence between the shape of the liquid molecules and the pores must be considered.
In this review, two primary factors influencing immersion enthalpy were emphasized. The first is the surface area of the solid interface molecules accessible to the liquid molecules, which is related to the kinetic diameter of liquid molecules, and the structural features of solid like pore size, pore architecture, and porosity. The second determinant is the binding process dictated by chemical characteristics of the liquid molecules and the solid interface molecules. Herein our emphasis leans more towards the noncovalent interaction relying on intermolecular forces, rarely involving the strong chemical bonds such as new covalent or ionic bonds between solid interface molecules and liquid molecules. It is recognized that bond formation is an exothermic process while bond breaking is endothermic. For solid-liquid immersion, liquid molecules replace the gas molecules on the solid surface, which is accompanied by the binding of solid interface molecules with liquid molecules, and the detachment of solid interface molecules from gas molecules. Consequently, if the immersion process is exothermic, it suggests that the heat released due to the binding of solid interface molecules and liquid molecules exceeds the heat absorbed during their detachment from gas molecules. The stronger and more intimate interaction between the solid interface molecules and the liquid molecules, the more heat is released during binding.

3.1. The influence of noncovalent interactions between liquid molecules and solid interface molecules on immersion enthalpy

Noncovalent interactions between solid interface molecules and liquid molecules can be specifically categorized as hydrogen bonding, hydrophobic interactions, and van der Waals forces. In certain compounds, a hydrogen atom can bond simultaneously with two highly electronegative and smaller atomic radius atoms (e.g., O, F, N). Hydrogen bonds influence water’s boiling point and the structure of proteins and DNA. In this article, hydrogen bonding refers to the connection between an X-H bond of one molecule and a Y atom of another. The genesis of hydrogen bonding is a result of various attractive and repulsive forces, with electrostatic interactions being paramount. Silanol groups Si-OH on zeolite or quartz surfaces can form hydrogen bonds with water molecules. Van der Waals forces mainly encompass induced forces (polar molecules with non-polar molecules), dispersion forces, and electrostatic forces (attraction between polar molecular dipoles).
Román-Leshkov group [34] reported that cyclohexanone, in the presence of 2-butanol as a solvent, exhibits distinct adsorption behaviors in hydrophobic zeolites versus hydrophilic zeolites. Within hydrophilic zeolites, cyclohexanone interacts with a greater number of 2-butanol molecules, leading to a more ordered hydrogen-bonding network, which accelerates transfer hydrogenation turnover rates (Figure 3). Liliana Giraldo et al. [35] measured the immersion enthalpy of different types of activated carbon in benzene, cyclohexane, water, and phenol. For most activated carbons, the absolute adsorption enthalpy in benzene was higher than in cyclohexane, and slightly higher in phenol solutions than in water. However, immersion enthalpy in cyclohexane and phenol solutions varied based on the type of activated carbon. Similarly, D.A. Blanco-Martínez et al. [36] examined the relationship between the adsorption of phenol in activated carbon solutions at a pH of 7 and immersion enthalpy, finding that immersion enthalpy increased with adsorption. Blanco D and colleagues [37] studied the adsorption of catechol by modified activated carbon in water and the related changes in immersion enthalpy. They found the immersion enthalpy values increased with increasing adsorption. Giraldo L et al. [38] chemically prepared activated carbon and investigated its immersion enthalpy in tetrachloromethane, water, HCl, and NaOH. For most of the prepared activated carbon, immersion enthalpy was highest in tetrachloromethane, followed by acid or base, and least in water. Direct correlations were observed between immersion enthalpy in HCL and NaOH and the total acidity and alkalinity of the activated carbon. Giraldo L and co-researchers [39] determined the immersion enthalpy of modified activated carbon in dichloromethane and tetrachloromethane, noting higher values in dichloromethane due to its smaller molecule size and lesser diffusion limitations. Giraldo et al. [40] applied immersion calorimetry to study interactions between benzene/cyclohexane and toluene/cyclohexane binary mixtures with three activated carbons of varying physicochemical properties. They found that immersion heat in aromatic compounds was higher than in cyclohexane. By selecting activated carbons with stable interfaces for the study and measuring their immersion enthalpy in different liquids, it was deduced that the binding strength between activated carbon interface molecules and benzene molecules was stronger than with cyclohexane. This could be attributed to the differences in bond formation between benzene and cyclohexane molecules, which subsequently affected their bonding with activated carbon surface molecules.
From another perspective, functional groups on the solid surface primarily dictate the binding sites of liquid molecules on the solid interface. Consequently, these functional groups contribute significantly to immersion enthalpy. The relationship between the amount of functional groups and immersion heat can be understood from the standpoint of chemical properties and affinity. For carbon-based material, functional groups (e.g., carboxyl, phenolic, lactonic) determine the chemical properties and surface activity. These functional groups can interact with molecules in immersion liquids through noncovalent forces such as hydrogen bonding and van der Waals forces. Some even form covalent bonds, releasing a considerable amount of heat, as observed in the interaction between the carboxyl groups on the surface of activated carbon and sodium hydroxide.
In order to elucidate how the functional groups on the surface of activated carbon influence its bonding with liquid molecules and consequent immersion enthalpy, numerous researchers have treated the surface of activated carbon and altered its functional groups. Bernal et al. [41] thermally and chemically treated a commercial activated carbon to modify its surface oxidation groups and further assessed the impact on the adsorption of paracetamol. They found that immersion enthalpy increased with a rise in overall alkalinity, indicating that π electrons have a low affinity for water. Conversely, the immersion enthalpy decreased as the total alkalinity reduced in acidic mediums (Figure 4). Rodríguez-Reinoso et al. [42] studied the influence of surface oxygen groups on immersion heat in activated carbon prepared from steam activation of olive stone and further oxidized with nitric acid. When measuring immersion enthalpy as a function of degassing temperature, they observed similar trends in both systems and the immersion heat in non-polar benzene was virtually unaffected by the removal of surface groups during thermal treatment. Acevedo et al. [43] chemically activated African palm shells to produce activated carbon and introduced the concept of a “hydrophobic factor,” which is defined as the ratio of the immersion enthalpy in benzene to that in water. It was observed that the immersion enthalpies of the activated carbon in benzene and dichloromethane were significantly higher than those in water, which indicates a strong hydrophobic character of the produced activated carbon. This underscores the general principle that a higher solid-liquid immersion enthalpy suggests stronger non-covalent interactions between the solid and the liquid. This concept has been widely accepted and acknowledged by many researchers. Bogeat et al. [44] immersed activated carbon in solutions with various ions to prepare samples coated with metal oxides and found the number and type of hydrophilic groups (functional groups containing oxygen on the activated carbon surface (like hydroxyl, carboxyl, and ketone groups) and coordinating groups and polarized bonds, such as metal-oxygen bonds in metal oxides) in the samples affected their affinity for water. Samples with more hydrophilic groups showed a stronger affinity for water, implying that activated carbon with more hydrophilic groups has higher immersion enthalpies in water. Diana et al. [45] discovered that when the oxygen-containing functional group content on the surface of activated carbon samples is reduced, there is a stronger interaction with toluene, resulting in an increased immersion enthalpy. This enhancement in interaction arises from the amplified non-covalent forces between the π electrons on the activated carbon surface and the electrons in the aromatic ring of toluene.
The emphasis of our discussion lies in these augmented non-covalent interactions. It is evident that due to the orders of magnitude difference between covalent and non-covalent interactions, one can readily differentiate between covalent and non-covalent interactions in their manifestations. Given that non-covalent forces are generally weaker in nature, the immersion enthalpy derived from immersion processes dominated by non-covalent interactions typically ranges from 5 J/g to 150 J/g. Similarly, Carvajal-Bernal et al. [46] pointed out that the interaction with water molecules can be intensified when there are more oxygen-containing groups on the surface of activated carbon. For the adsorption of phenol, water must first be displaced from its surface. This suggests that as the number of oxygen-containing groups on activated carbon increases, the enthalpy values obtained during phenol adsorption will decrease. Giraldo L et al. [47] modified activated carbon using nitric acid solutions to increase the content of acidic functional groups on its surface. They measured the immersion enthalpy of different activated carbons with lead nitrate and found that as the amount of acidic functional groups on the active surface increased, both the immersion enthalpy and the adsorption quantity of lead ions also rose.
Castillejos et al. [48] attributed the differences in immersion enthalpies of toluene between carbon nanotubes and graphite to the variations in the strength of non-covalent intermolecular interactions. Specifically, the π-π interactions of toluene with carbon nanotubes were found to be stronger. To discern which particular non-covalent interaction primarily contributes to the immersion enthalpies, it is essential to consider the molecular properties in the analysis. This highlights the influence of surface functional groups on immersion enthalpy, which is consistent with conclusions drawn from studies on activated carbon. Barton and colleagues [49] undertook studies on immersion calorimetry using various butyl derivatives of differing polarities, namely n-butanol, n-butyric acid, n-butyl chloride, n-butanal, n-butyronitrile, and n-butylamine. For non-polar liquids, such as n-hexane, the immersion heat values for both oxidized and non-oxidized graphite were similar, suggesting that surface polarity has minimal impact on their interactions. However, the butyl derivatives presented a range of values with large differences, which can be attributed to the interplay between the electrostatic field on the graphite surface and the dipole moments of the liquid molecules. Additionally, Barton et al. [50] investigated the impact of different oxygen functional groups on the graphite surface concerning the immersion heat of various polar liquids, including benzene, water, and methanol. Stoeckli et al. [51] measured the immersion enthalpies of two non-porous illites in benzene and water. The per unit area immersion enthalpy for both illites in benzene was found to be comparable, approximately 73 mJ·m-2. However, in water, there was a significant disparity, registering at 371 mJ·m-2 and 782 mJ·m-2 respectively. Bernal et al. [52] employed immersion calorimetry to study the effect of sodium chloride solution concentration on the adsorption of acetaminophen and salicylic acid by activated carbon (Figure 5). With increasing ion concentration, the adsorption capacity of activated carbon for both acetaminophen and salicylic acid decreased, as reflected by the corresponding immersion enthalpies. This decrease was ascribed to the fact that the conjugation effects between π electrons and sodium ions diminished the adsorption affinity of activated carbon for acetaminophen and salicylic acid. Bursh et al. [53] established a correlation between the silica surface property and the immersion calorimetric data concerning the interaction between silica and water and further obtained evidence of potential variations in the surface bond characteristics across different silica samples. They found the content of hydroxyl groups on the silica surface is not directly related to immersion heat, even though typically, a silica surface with a high proportion of hydroxyl groups exhibited greater immersion heat.

3.2. Influence of Liquid-Accessible Surface Area on the Immersion Enthalpy at Solid Surfaces

A paramount concept in solid-liquid interface interaction is the total surface area of the solid that is accessible to the liquid molecules. This accessible surface area is primarily dictated by the pore structure, porosity, surface morphology of the solid, and the kinetic diameter and shape of the liquid molecules. Calorimetric methods can be employed to evaluate the pore size distribution of porous solids. For this, one needs to select probe molecules with varying kinetic diameters and measure their immersion enthalpy with the porous substrate. The pore size distribution acquired from calorimetry can then be compared relatively to results obtained from other methods, such as the determination of specific surface area through gas adsorption using the BET method.
Atkins et al. [54] investigated the immersion heat of a microporous activated carbon in an array of organic liquids and found that immersion enthalpy depends on the volume of the immersion liquid molecules that can enter the porous structure. This observation opened the possibility of utilizing calorimetric methods as tools for determining pore size distribution of microporous carbon. Stoeckli and Kraehenbuehl [55] proposed a method to analyze immersion enthalpy data based on the Dubinin pore volume filling model. They established a mathematical relation describing the correlation between immersion enthalpy in liquid for microporous solids and the parameters from vapor adsorption based on the Dubinin-Radushkevich (DR) equation, where the immersion enthalpy is primarily governed by the micropore volume and the characteristic energy of the system. This equation suggests that the immersion enthalpy of microporous solids in a specific liquid is a function of the micropore network, in which characteristic energy is associated with the average pore diameter and is influenced not just by the micropore volume. The characteristic energy (E0) is a parameter describing the interaction strength between solid adsorbents, like activated carbon, and adsorbates (gaseous or liquid molecules), which is related to the microporous structure (including pore size and shape) of the adsorbent and surface functional groups (e.g., oxides or other chemical groups) affecting the interaction of adsorbate molecules with the solid surface. Moreover, the characteristic energy is also influenced by properties of the adsorbate molecule, such as molecular polarity and size. A higher E0 value indicates a stronger adsorbent-adsorbate interaction, which may lead to an enhanced adsorption capacity and selectivity.
Water is extensively used as a probe molecule for characterizing zeolites in terms of pore size distribution [56]. Water adsorption on hydrophilic zeolites has been utilized to measure its pore volume, indicating that the quantity of water adsorbed by zeolites is a linear function of its aluminum content [57]. Concurrently, in co-adsorption experiments, the relationship between hydrocarbons (e.g., toluene) and the weight of adsorbed water has been employed to define the hydrophobicity index (HI) of zeolites [58], which can be determined from the ratio of the weight of hydrocarbons to that of adsorbed water. Reinoso et al. [59] found that immersing carbonaceous materials (like microporous activated carbon and carbon molecular sieves) in nonpolar or low-polarity liquids with different molecular sizes can estimate micropore size distribution and immersing in liquids of similar polarity (such as water or methanol) can characterize the hydrophilicity of the surface. Vargas et al. [60] prepared granular activated carbon by chemically activating African palm kernel and measured its immersion enthalpy with benzene. They found a relationship between immersion heat in benzene and accessible surface area, in which the immersion heat increased as the accessible surface area increased. Pendleton et al. [61] utilized microcalorimetry to measure the immersion enthalpies of baseline and reference carbons in various liquids at 30 °C with aim to determine the specific surface area and pore size distribution of microporous polyvinyl alcohol-based activated carbon by conducting controlled and repetitive immersion calorimetry experiments. They discovered that the specific surface area obtained through immersion calorimetry closely resembled the pore size distribution and specific surface area derived from nitrogen gas adsorption (Figure 6). Giraldo et al. [62] investigated the pore size distribution and surface chemical properties of oxidized graphene via immersion calorimetry. They selected ten different probe molecules (including water, benzene, hexane, ethanol, and propanol) and conducted experiments on a laboratory-made calorimeter. They observed that molecules with smaller diameters exhibited larger immersion enthalpies with both graphite and oxidized graphene through plotting the relationship between the kinetic diameter of the liquid molecules and the immersion enthalpy of graphite and graphene. They also compared the pore size distribution results obtained from calorimetry with those derived using other methods. In conclusion, the use of calorimetry to study the specific surface area and pore size distribution of solid porous materials such as activated carbon, zeolites, and graphene has found considerable application. Moreover, this method shows promise for expansion to a wider range of porous materials.

4. Application of Calorimetry in the Study of Specific Solid-Liquid Interaction Processes

This section delves into the use of calorimetry for examining specific solid-liquid interface interaction processes, structured around two primary subsections.

4.1. Calorimetry in Investigating Adhesion and Adsorption Behavior during Solid-Liquid Immersion

Omar R. Harvey and colleagues [63] employed a flow adsorption microcalorimeter to probe the structural adsorption relationships between plant biochar with varying Lewis acidities and two metal ions. Zineb Fritah et al. [64] used mixed solution calorimetry to explore the impact of water molecules on the interactions of epoxyamines with metals ions. They found that the presence of water might significantly influence epoxyamine-based systems. Roth et al. [65] found that the mixing enthalpy of montmorillonite suspensions with LiCl, NaCl, and KCl correlates with the electrolyte solution concentration. They further pointed out that the enthalpy change is related to the collapse of montmorillonite layers, especially at specific interlayer spacings. Another observation was that the enthalpy change for LiCl with montmorillonite suspension was endothermic, while that for NaCl and KCl was exothermic. They speculated that the diffusion of ions to montmorillonite particles, ion penetration (adsorption) into the montmorillonite layers and a restructuring of interlayered montmorillonite occurred during the mixing process of montmorillonite with the electrolyte solutions.
Douillard and colleagues [66] employed three distinct methods to analyze the enthalpy produced during the immersion of calcium ions or sodium ions saturated montmorillonite in water. In all cases, it was discerned that the interaction of calcium-ion saturated montmorillonite with water molecules was stronger than its sodium-ion counterpart. Sharma et al. [67] utilized immersion calorimetry at room temperature to determine the enthalpy of pseudo-clay Ti3C2Tx absorbing different cations (Li+, Na+, K+). They also examined the ion-exchange enthalpy and ascertained the insertion and release behavior of ions combined with pH measurements and ICP-MS analysis.
Drout and co-researchers [68] studied the adsorption of pesticides toxins onto MOFs materials using isothermal titration calorimetry (Figure 7). They deduced the changes in enthalpy, entropy, and Gibbs free energy during the adsorption process. Bernal et al. [69] gauged the immersion enthalpy of activated carbon in phenol, salicylic acid, and paracetamol and deliberated on the relationship between adsorption rates and enthalpy values. Additionally, the adsorption of organic toxins onto MOF materials investigated using isothermal titration calorimetry showed that the integrated heat data, aligned with the single-point model (depicted by the red line), validates that the adsorption processes for both toxins on MOFs are exothermic in nature (Figure 8) [20].

4.2. Immersion Calorimetry as a Quantitative Method for Assessing Solid Particle Wettability

Wettability typically refers to the ability of a liquid to spread across a solid surface. The wettability of solid particles plays a pivotal role in areas such as mineral flotation [70], pharmaceutical engineering [71], catalysis [72], and petroleum extraction [73] and so on. Contact angle method is the most direct and conventional method to evaluate the wettability between a solid and a liquid. However, utilizing the contact angle to describe wettability has several limitations. For instance, it requires the solid surface to be impeccably clean, and the reproducibility and precision of the obtained results need to be improved. Theoretically, one can deduce the solid-liquid immersion heat from the contact angle and vice versa. Indeed, immersion heat can provide a broader application scope than contact angle if wettability is defined as the affinity between the solid and the liquid.

4.2.1. Theoretical Derivation of the Contact Angle and Immersion Heat

According to the definition of the contact angle, when a droplet is placed on a uniform and smooth solid surface and achieves a stable form, the three interfacial angles between solid-liquid, solid-gas, and liquid-gas remain constant. At this point, the interfacial tensions between the three phases (solid, liquid and gas) achieve equilibrium, and the forces at the trijunction comply with Young’s equation [74]:
γ g - s = γ l - s + γ g - l   cos θ
Under constant temperature and pressure, the immersion process gives:
Δ G imm = γ l - s -   γ g - s  
dH = TdS + dG  
Δ imm H = Δ G imm - T ( d ( Δ G imm ) dT )  
Equation (5) can be reformulated as:
Δ imm H = - γ g - l cos θ + T ( d ( γ g - l cos θ ) dT ) P  
Theoretically, the immersion enthalpy of a solid-liquid system is determined by the liquid surface tension and the solid-liquid contact angle. From equation (6), it can be deduced that:
Δ imm H = γ l - s - γ g - s + T ( d ( γ l - s ) dT - d ( γ g - s ) dT ) P
Δ imm H = - γ g - l cos θ + T ( d ( γ l - s ) dT - d ( γ g - s ) dT ) P
Let   T ( d ( γ l - s ) dT - d ( γ g - s ) dT ) P be denoted as K.
  • the relation becomes:
cos θ = Δ imm H - KT γ g - l
The term K represents the change in interfacial tensions of solid-liquid and the solid surface with temperature under constant temperature and pressure conditions. According to Young’s equation, one only needs to measure the other three variables to calculate the surface energy   γ g - s   of the solid. Contact angle θ and liquid surface tension γ l can be directly measured using instruments. However, since the solid-liquid interfacial tension γ l - s is difficult to be directly measured, several scholars have developed methods to solve for surface free energy based on the aforementioned rationale. Fowke and others [75,76] posited that the liquid surface tension and the solid surface tension consist of dispersive component γ d and polar component γ p , that is:
γ = γ d + γ p
Where γ d   is the molecular interaction produced by London forces, called dispersive interactions, which usually involve non-polar molecular interactions influenced by density. γ p encompasses the molecular interactions produced by non-London forces, which include dipoles and hydrogen bonding, with its value influenced by surface polarity.
When only considering dispersive interactions between solid and liquid, it follows:
γ 12 = γ 1 + γ 2 - 2 γ 1 d   γ 2 d
Combined with equation (1), it becomes:
γ g - l cos θ = - γ g - l + 2 γ l d   γ s d
Where γ l d is the dispersive component of the liquid, and γ s d   is the dispersive component of the solid. By equation (12), measuring the angle θ between a known liquid with γ g - l   and γ l d   and the tested solid will yield the dispersive component γ s d   of the solid surface free energy. Aside from Fowke, other researchers [77,78,79,80,81,82,83,84,85,86,87,88,89] have also proposed methods to solve for solid surface free energy by considering molecular forces beyond dispersive forces. Overall, using immersion calorimetry to solve for the solid-liquid contact angle is theoretically feasible, but it proves complex in practical applications.

4.2.2. Practical Examples of Quantifying Solid Particle Wettability Using Immersion Calorimetry

Weston et al. [90] assessed the wettability of nano-silica utilized immersion calorimetry (Figure 9). Yan et al. [91] obtained immersion enthalpy data for water/nano-silica and toluene/silica systems through employing calorimetric techniques, in which the contact angles was derived by evaluating these data. Starting from the first principles of hydrophobic powders, Spagnolo et al. [72] established a relationship between immersion heat and contact angle. They also calculated the contact angle of pure water and fluorocarbon using the immersion enthalpy of pure water in fluorocarbon. Xu [92] measured the immersion enthalpies of three particles with varying wettability under different temperatures. Combined with accurate measurements of the interfacial tension as a function of temperature, they deduced the contact angle values from the immersion heat data. Taguta et al. [93] employed the obtained immersion enthalpy data as an indicator for evaluating the hydrophobicity of clay minerals and further used this data in their study on mineral flotation.

4. Conclusion and Outlook

Calorimetry serves as an effective tool for probing solid-liquid interfacial interactions. It has been widely applied in studying the interactions between liquids such as water, organic solvents, and electrolyte solutions, and solids like activated carbon, zeolites, clay minerals, and silica. The immersion enthalpy values obtained through calorimetry are influenced both by the intensity of the solid-liquid interaction and by the accessible surface area of the solid to the liquid. Calorimetry offers thermodynamic insights into the solid-liquid binding process. Furthermore, the immersion enthalpy obtained from calorimetry can be employed as data for quantifying the wettability of solid-liquid systems, which is feasible both theoretically and practically. We anticipate that calorimetry will play an even more significant role in the research of solid-liquid interfacial interactions in fields such as petroleum extraction, mineral flotation, pharmaceuticals, and catalysis.

Acknowledgements

This project was funded by the PetroChina Company Limited projects including Critical Technical Research of Functional Water Flooding Technology (2021DJ1302) and New Mechanism and New Method Research of Greatly Improving Oil Recovery in Low Permeability/Tight Reservoir (2023ZZ0404), and the Natural Science Foundation of Shaanxi Province (2021JQ-014).

Conflicts of Interest

The authors declare that they have no known competing financial interests or personal relationships that could have appeared to influence the work reported in this paper.

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Figure 1. The graphic illustration of a simplified ITC instrument [12].
Figure 1. The graphic illustration of a simplified ITC instrument [12].
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Figure 2. Schematic diagram of the heat flux DSC principle [32].
Figure 2. Schematic diagram of the heat flux DSC principle [32].
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Figure 3. Adsorption of Cyclohexanone within the 2-Butanol Filled Pores of (a) Hydrophobic zeolite and (b) Hydrophilic zeolite [34].
Figure 3. Adsorption of Cyclohexanone within the 2-Butanol Filled Pores of (a) Hydrophobic zeolite and (b) Hydrophilic zeolite [34].
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Figure 4. (a) The immersion enthalpy of activated carbon in paracetamol solutions of varying concentrations; (b) The interaction between activated carbon and paracetamol in an acidic medium [41].
Figure 4. (a) The immersion enthalpy of activated carbon in paracetamol solutions of varying concentrations; (b) The interaction between activated carbon and paracetamol in an acidic medium [41].
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Figure 5. The adsorption enthalpy of activated carbon for acetaminophen or salicylic acid in sodium chloride solutions of varying concentrations [52].
Figure 5. The adsorption enthalpy of activated carbon for acetaminophen or salicylic acid in sodium chloride solutions of varying concentrations [52].
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Figure 6. The illustration of molecular optimal packing paradigm upon adsorption within the micropores [61].
Figure 6. The illustration of molecular optimal packing paradigm upon adsorption within the micropores [61].
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Figure 7. Isothermal Titration Calorimetry Investigation of Organophosphorus Pesticide Adsorption onto MOF Materials [68].
Figure 7. Isothermal Titration Calorimetry Investigation of Organophosphorus Pesticide Adsorption onto MOF Materials [68].
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Figure 8. Adsorption of p-CS potassium and potassium indoxyl sulfate on NU-1000 (A and C). The corresponding combined heat data (B and D) were fitted to the unit point model (red line) [20].
Figure 8. Adsorption of p-CS potassium and potassium indoxyl sulfate on NU-1000 (A and C). The corresponding combined heat data (B and D) were fitted to the unit point model (red line) [20].
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