Scholarly article on topic 'Technical crystallization for application in pharmaceutical material engineering: Review article'

Technical crystallization for application in pharmaceutical material engineering: Review article Academic research paper on "Materials engineering"

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Abstract of research paper on Materials engineering, author of scientific article — Abdul Khaliq El-Zhry El-Yafi, Hind El-Zein

Abstract In recent years, engineering the total morphology of pharmaceutical materials particles to desirable shape, size and surface area has long been actively increased because it has many advantages especially for improving physicochemical properties of Active Pharmaceutical Ingredients (APIs). This article therefore considers the potential utility of crystal engineering as a tool for controlling and designing properties of pharmaceutical solid particles in purpose to developing efficacious performance of solid dosage form, fundamentals of crystallization process, applications. In addition, understanding the relationship between molecular recognition, thermodynamic, and kinetics which controls the crystallization process so that it benefits in designing successful experiments to have desirable crystal habit for materials.

Academic research paper on topic "Technical crystallization for application in pharmaceutical material engineering: Review article"

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Review

Technical crystallization for application in ^

pharmaceutical material engineering: Review

article

Abdul Khaliq El-Zhry El-Yafi*, Hind El-Zein

Department of Pharmaceutical Technology, Faculty of Pharmacy, Damascus University, Damascus, Syria

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ARTICLE INFO

ABSTRACT

Article history: Received 11 October 2014 Received in revised form 15 February 2015 Accepted 25 March 2015 Available online 4 April 2015

Keywords:

Crystallization

Nucleation

Crystal growth dispersion Thermodynamic

In recent years, engineering the total morphology of pharmaceutical materials particles to desirable shape, size and surface area has long been actively increased because it has many advantages especially for improving physicochemical properties of Active Pharmaceutical Ingredients (APIs). This article therefore considers the potential utility of crystal engineering as a tool for controlling and designing properties of pharmaceutical solid particles in purpose to developing efficacious performance of solid dosage form, fundamentals of crystallization process, applications. In addition, understanding the relationship between molecular recognition, thermodynamic, and kinetics which controls the crystallization process so that it benefits in designing successful experiments to have desirable crystal habit for materials.

© 2015 Shenyang Pharmaceutical University. Production and hosting by Elsevier B.V. This is an open access article under the CC BY-NC-ND license (http://creativecommons.org/

licenses/by-nc-nd/4.0/).

1. Introduction

Drug molecules with limited micromeritic properties & aqueous solubility (about 90% of new API's having low solubility in water) [1] are becoming increasingly prevalent in the research and development of new drugs [2]. Nowadays, increasing energy prices and the inefficient manufacturing have made pharmaceutical companies face cost pressures. Therefore, the primary aim of pharmaceutical material engineering is to improve designed particles of solid pharmaceutical dosage forms which results in improving the efficiency of the manufacturing processes and giving a high degree of

functionality to the drug or excipient particles (especially of pharmaceutical materials for direct compression) [3] in pharmaceutical products. Materials in the solid state depending on the internal packing of their molecules can be found in either crystalline, polymorphism or amorphous (or a combination of both). It has been shown that they can be packed in a defined order (crystalline), have no long-range three dimensional (3-D) order (amorphous) have different repeating packing arrangements (polymorphic crystals) or have solvent included (solvates and hydrates). Each of these changes in internal packing of a solid will give rise to changes in bulk properties such as physiochemical, mechanical, etc. [4]. For the crystal form, it is possible to change the external

* Corresponding author. Department of Pharmaceutical Technology, Faculty of Pharmacy, Damascus University, Damascus, Syria. E-mail addresses: telyafi@gmail.com (A.K. El-Zhry El-Yafi), hindalzen@yahoo.com (H. El-Zein). Peer review under responsibility of Shenyang Pharmaceutical University. http://dx.doi.org/10.1016/j.ajps.2015.03.003

1818-0876/© 2015 Shenyang Pharmaceutical University. Production and hosting by Elsevier B.V. This is an open access article under the CC BY-NC-ND license (http://creativecommons.org/licenses/by-nc-nd/4.0/).

shape of a crystal and this is called the crystal habit which is the consequence of the rate at which different faces grow. Changes in internal packing usually (but not always) give an easily distinguishable change in the crystal habit. With any crystalline material, the largest face is always the slowest growing and some crystal faces may have more exposed polar groups and others may be relatively non-polar that are depend on the packing geometry of the molecules into the lattice. In other words, the growth on different faces will depend on the relative affinities of the solute for the solvent and the growing faces of the crystal. It is technically possible to engineer changes in crystal habit by deliberately manipulating the rate of growth of different faces of the crystal [5]. Crystallization, particularly crystallization from solutions, is the vitally important operation in the production of pharmaceutical solid particles because most of drug particles (<90%) are delivered in crystalline form [1] and it benefits in determining the purity (chemical and structure) and the physical properties of a material which are summarized in Table 1.

However, changes in crystallization conditions can significantly alter their previous properties followed by thermody-namic and mechanical properties [6].

Powder technology is the base of dosage form design with effective drug delivery. Any particles of pharmaceutical solid materials may be produced by two ways:

• Constructive methods: include crystallization, spray-drying, lyophilization, and supercritical fluid techniques.

• Destructive methods: include milling and grinding.

In general, crystallization is the most common method of particle production [7].

2. Crystal engineering in properties design of pharmaceutical materials

2.1. The role of thermodynamic in the crystallization process

The phase change with stability associated with crystallization processes can be explained by rules of physical chemistry and thermodynamic principles. When a substances is transformed from one phase to another, the change in the molar Gibbs free energy (DG) of the transformation, at constant pressure and temperature, is given by:

AG=(H2-Hl)

Solute in phase 1 Solute in phase 2

(Liquid form in solution) (Crystal + Liquid form in solution)

where m1 and m2 are the chemical potentials of phase 1 and phase 2, respectively. When DG < 0, the transition from phase 1 to 2 is spontaneous under specific conditions (in case of supersaturated solution). Alternatively, when DG > 0, this phase transformation is not thermodynamically possible (in case of unsaturated solution); whereas, DG = 0 defines a condition of thermodynamic equilibrium in the system, in

i—1 Î !—1

0) s rt

O M-H ^ &

^ S ^ S a ^

^ T3 rt G u rt

Us ^ it ^

s U <D O ia m M

w aj ^ a

01 u 43 Si U H

■y .u

43 Si U H

this situation, the free energy of two phases is the same [8] (in case of saturated solution) and the process can divided as follows [9]:

Crystalline Solute Pure Liquid Solvent

Supercooled Liquid Solute

Solvent-containing cavity

Supercooled liquid Solute Solvent-containing cavity

Saturated Solution

Crystalline Solute

Pure Liquid Solvent

Saturated Solution

A supersaturated solution can be achieved in general by under cooling if dCeq/dT > 0 or by evaporation the solution if dCeq/dT < 0. If T0 is the solute's saturation temperature for a given solvent system, then at some temperature T, DG can be demonstrated in terms of heat effects as:

ASdT = -AH

(T - To)

where AS is the molar entropy and AH is the enthalpy change for the phase transformation. The molar Gibbs free energy can also be expressed in terms of activity as:

DG = -RT = ~RT ln(S)

where R is the universal gas constant, T is the absolute temperature, a is the activity of the solute and o0 is the activity of the pure solute in equilibrium with a macroscopic crystal, S is the saturation ratio which is given by:

where C is the solute concentration and Ceq is the equilibrium solubility of the solute at the temperature and pressure of the system; from this, the supersaturation ratio can be defined as:

(C Ceq) /Ceq — S 1

These thermodynamic considerations describe a driving force for crystallization [10].

2.2. Crystallization process and factors affecting in crystal habit

2.2.1. The crystallization mechanism

Because of instability of many amorphous materials, most drugs are formulated in the crystalline state [4]. Crystals are produced by inducing a change from the liquid to the solid state. Crystallization from solution can be considered to be the result of relative rate of the three successive processes:

• Supersaturation of the solution.

• Formation of crystal nuclei.

• Crystal growth round the nuclei [10]. A Supersaturated Solution Step:

Supersaturated solution, a chemical potential and essential requirement for crystallization process, is the driving force for nucleation and crystal growth. It can be expressed as the concentration divided by the solubility (C/S). Supersaturation can be defined as any solution that contains more dissolved solid (solute) than that can be found in saturation conditions [11]. Supersaturated solutions are not thermodynamically stable; in these circumstances the system will adjust in order to move back to the true solubility and to do this the excess solute will precipitate [5]. This supersaturated solution maybe achieved by several methods including [8] and [10]:

1 Methods that produce supersaturation by increasing the solute

concentration: include:

a. Removing the solvent liquid by evaporation (this is the way sea salt is prepared): for systems (isothermal solution) in which the solubility is not a strong function of temperature.

b. Dissolution of a metastable solid phase like amorphous, anhydrous, more soluble, and salt which transformation to crystalline, hydrate, less soluble poly-morph, and free acid or base, respectively).

2 Methods that produce supersaturation by decreasing the solute

solubility: include:

a. Cooling the solution, as most materials become less soluble when the temperature is decreased: for systems in which solubility increases with temperature.

b. Adding another solvent which will mix with the solution, but in which the solute has a low solubility. This second solvent is often called an anti-solvent (i.e. water).

c. Adding precipitants or by a chemical reaction that change the nature of the solute.

d. pH changing.

The terms labile (unstable) and metastable zones can classify supersaturated solutions in which spontaneous nucleation would or would not occurs, respectively. These zones are presented in a solubility diagram as shown in Fig. 1.

Above the equilibrium line (solid line): the solution are at supersaturation. In the labile zone, nucleation can occur spontaneously which is called primary nucleation. In meta-stable zone, no nucleation occurs which means that supersaturation itself is insufficient to cause crystal formation. The crystal embryos must form by collision of molecules of solute in the solution or sometimes by the addition of breakage of the seed crystals or dust particles or even particles from container walls.

Deliberate seeding is often carried out in industrial processes, seeding crystals are not necessary to be of the substances concerned but may be isomorphous substances (i.e. of the same morphology) [11] and [12].

B Nucleation step:

Nucleation is the formation of a small mass on which a crystal can grow [5]. There are three types of nucleation that can occur in supersaturated solutions. These types are presented in nucleation situations diagram as shown in Fig. 2.

Fig. 1 - The solubility diagram representing the metastable zone [11].

1 Primary homogeneous nucleation:

This is spontaneous nucleation where the formation of the solid phase particle is not brought by the presence of any solid phase. It requires very high supersaturation conditions such as in the labile zone [8], [11], and [13].

2 Primary heterogeneous nucleation:

Is the most primary nucleation where the formation of new solid phase particle is catalysed by the presence of a foreign solid phase which has lower surface energy than that of a new solute particle. Therefore, it requires lower supersaturation than homogeneous nucleation [10] and [13]. However, homogeneous and heterogeneous can be presented in same the nucleation process as follow:

Shomo > Shetero

where S is a saturation ratio of solution [10].

3 Secondary heterogeneous nucleation:

It is the most common nucleation event in industrial crystallization and is the mechanism by which formation of the solid phase is initiated when solid phase of solute particle can be present or added to solution. Therefore, this type of nucleation can be found even in the metastable zone where the crystals seemingly only grow [10], [11], and [13].

In recent years, the theory of two step nucleation model has attracted attention, supported by various studies and observed especially in proteins and colloidal systems [14-18]. In this theory, nucleation proceeds through a dense liquid (amorphous) step before ordering into the growth structure to form a three-dimensional lattice structure [19].

The two steps progression from liquid to crystalline nuclei observed in colloid experiments can be seen in Fig. 3. As soon as stable nuclei are formed, they begin to grow into visible crystals [18]. The macromolecules nucleation such as colloi-dals, proteins and polymers can be observed by using techniques that are summarized in Table 2. Such as optical microscopy, small-angle neutron scattering and atomic force microscopy (AFM) [20-23]. which the effective technique to qualitatively study-surface morphology and crystal growth processes [24]. In order that there is more chances to control the rate of nucleation step which affects in morphology of crystal particles. As far small molecules, direct measurement and observation of nucleation of nuclei is impossible so crystal particles can be observed only after growth to larger size through growth step [23].

C Crystal growth step:

Crystal growth is the addition of more solute molecules to the nucleation site or crystal lattice to evolution macroscopic crystal form of defined size and shape [5]. In other words, Particle size distribution and morphologies produced are a result of the relative rates of reaction of nucleation, crystal growth [10].

Crystal growth is considered to be a reverse dissolution process and the diffusion theories of Noyes and Whitney, and of Nernst, consider that matter is deposited continuously on a crystal face at a rate proportional to the difference of concentration between the surface and the bulk solution. So an Equation (1.1) for crystallization can be proposed in the form:

f = AKm(Css - Cs)

Fig. 2 - The nucleation situations from solution [7].

where m is the mass of solid deposited in time t, A is the surface area of the crystal, Cs is the solute concentration at saturation and Css is the solute concentration at supersaturation. As km = D/5 (D being the diffusion coefficient of the solute and 5 the diffusion layer thickness), the degree of agitation of the system, which affects 5, also influences crystal growth. Crystals generally dissolve faster than they grow and depend on their initial size [12] and [25], so growth is not simply the reverse of dissolution. It has been suggested that there are two steps involved ingrowth in addition to those mentioned earlier [12].

However, crystal growth process consists of several stages through the growth unit. The growth unit in turn describes the critical elements of how a specific molecular species has assembled in a crystalline state in three dimensions, so that crystal growth depend on strength of the interactions (especially, if there is hydrogen bonding between functional group, Fig. 4) between molecules itself and also between growth layers in network structure which would change in overall morphology of the crystal [2]. These stages include [7], [23], [26], and [27]:

Fig. 3 - Two-step nucleation of colloidal particles. Image (a) shows the initial diluted liquid phase, (b) shows the amorphous dense droplets are first created from mother phase, followed by (c) the crystalline nuclei are created from the amorphous phase [18].

Table 2 - Physical approaches for studying macromolecular crystallization [24].

Method

Static/quasi-elastic light scattering

Michelson interferometry

Mach—Zehnder interferometry

Atomic force microscopy

Fluorescence polarization

Low angle neutron scattering

Osmometry

Light microscopy

Time lapse video microscopy

X-ray diffraction

Numerical simulation/modeling

Nucleation, phase transitions Growth kinetics

Concentration gradients in solutions

Growth mechanisms, kinetics, defect structure, defect density

Nucleation

Nucleation

Nucleation

Characterization of crystal

Growth kinetics

Characterization of crystal

Nucleation, growth kinetics, phase transitions.

1) Transport of a growth unit (a single molecules, atom, ion, or cluster) from or through the bulk solution to an impingement site on the crystal face by convention and diffusion, which is not necessarily the final growth site (i.e. site of incorporation into the crystal).

2) Adsorption of the growth unit at the impingement site.

3) Diffusion of the growth units from the impingement site to a growth site.

4) Incorporation into the crystal lattice.

5) The latent heat of crystallization is released and transported to the crystal and solution.

Desolvation of the growth unit may occur anywhere in steps 2—4, or the solvent may be adsorbed with the growth

unit. In general, three types of crystal surfaces (and thus growth sites created by these surfaces) can be observed when impingement site captured the arriving growth units: Kink, Step, and Flat faces, which provide three, two, and one surface bond(s), respectively Fig. 5 [28]. As well, any of these steps can be the rate-limiting step in the crystal growth process and which step is rate-limiting will depend on the solvent properties like viscosity [8]. When the diffusion of molecules from the bulk solution to the impingement site is the rate-limiting step, crystal growth is volume-diffusion controlled whereas if the incorporation of a growth unit into the lattice is the slowest process then crystal growth is surface-integration controlled [8], [11], and [29]. At last, the final shape of crystal is defined by the slowest growing flat faces.

Fig. 4 - Representative superior hydrogen bonding in supramolecular [2].

Fig. 5 - A three-dimensional crystal surface showing three type of growth sites [28].

Crystal growth studies are therefore concerned with the mechanisms by which these faces grow [5].

2.2.2. Factors affected of crystal habit

If the crystallization conditions are changed in any way. Therefore, it is possible that the molecules may start to form crystals with a different packing pattern and different tuning crystal facets from that which occurred when the original conditions were used. The change in some conditions could be change in the rate and mechanism of crystallization process in crystal growth step, specifically. Hence, the art of crystal facet engineering is determined by numerous factors that regarded in thermodynamic, kinetics, and molecular recognition. These factors are summarized in Fig. 6 [30].

In general, a knowledge of how crystal grow from the crystal nuclei and the effects of the various factors which may influence crystal growth is not studied from pharmaceutical

viewpoint in as much as chemical or physical viewpoints. So crystal growth for any pharmaceutical ingredients may be in general affected by two factors [31], [32], and [33]:

• Rate-controlling process for crystal growth:

The rate at which a crystal grows can be controlled by any of three factors: diffusion from the solution to the crystal nuclei as well as surface integration mechanisms, flow of latent heat away from the growing crystal surface (under cooling stage), and reactions at the crystal-solution interface.

• The stability of planar interfaces relative to cellular interfaces.

Moreover, new drugs are screened to see how many poly-morphs exist, and then to identify which one is the most stable. The screening process requires a lot of work in crystallizing from different solvent system, with variations in method and conditions, in order to try to cause different polymorphs to form. The products are then checked with spectroscopy (e.g. Raman) and X-ray diffraction to see if they have different internal packing [5].

2.2.3. Effect of crystal habit on the performance of a pharmaceutical powders

Changing in crystal habit to any solid state in crystal and powders of both drugs and pharmaceutical excipients are interested because it can be change in physicochemical properties for it like surface energy (which can be determined by gravimetric, calorimetric and chromatographic), density, flowability, compressibility, melting point, solubility, physical & chemical stability and biopharmaceutical behaviour (dissolution,

Fig. 6 - Schematic diagram showing the interplay between thermodynamic, kinetic, and molecular recognition phenomena that governs crystallization [30].

bioavailability) because these depend on the size and number of crystal faces in crystal habit which affect both the production of dosage forms and the performance of the finished product [5]. As mentioned above, many properties can be change when a material is in a different polymorphic form in specific micromeritic properties, such as flowability, and a good reproducible compressibility. At all events, the flow-ability of needle-shaped or plated-shaped crystals is very poor and these crystals are difficult to handle [34]. For example, Ibuprofen is usually crystallized from hexane as elongated needle-like crystals, which have been found to have poor flow properties that due to surface atomic arrangement and surface affinity for the solvent to each orientation is different which can affect in final shape of the crystal [23]; crystallization from methanol produces equi-dimensional crystals with better flow properties and compaction characteristics, making them more suitable for tableting, plate-like crystals of tolbutamide cause powder bridging in the hopper of the tablet machine and also capping problems during tableting [12]; crystallization by a temperature-cooling method [35] and by a solvent-change method [36] modified the size, shape of particles so it had improved the compressibility and had a higher dissolution rate of tolbutamide, respectively. Another consideration, crystallization process in aqueous solution at different pH values (1,7, and 11) affected the morphology and size of carbamazepine crystals, the shape of this crystals was changed from flaky or thin plate-like to needle shape which improve better compaction and higher dissolution rate than the original carbamazepine powder [37]. Paracetamol is a high-dose drug with poor compression properties, which can make it difficult to form into tablets, Consequently, researchers have tried to use different polymorphic forms of paracetamol to find one that is more compressible, for Nichols and Frampton are found this drug was exist in two polymorphic forms according to crystallization method used, a common crystal form is a form I (monoclinic) was described

as plate-shape (Thermodynamically stable at room temperature, the commercially used form, and not suitable for direct compression which leads to unstable tablets with high capping tendency) and form II (orthorhombic) was a prismatic crystal show better compression behaviour (have a plastic deformation upon compaction so it suggested to use in direct compression) [38], and [39]. The disadvantage of the orthorhombic form is the possible transition to form I [40].

In general there will be a correlation between the melting point of the different polymorphs and the rate of dissolution, because the one with the lowest melting point will most easily give up molecules to dissolve, whereas the most stable form (highest melting point) will not give up molecules to the solvent [5].

High melting point = strong lattice = hard to remove a molecule = low dissolution rate (and vice versa)

A classical example of the importance of polymorphism on bioavailability is that of chloramphenicol palmitate suspensions in the late 1960s. In Fig. 7 the blood serum level is plotted as a function of time after dosing. It can be seen that the stable a-polymorph (have low free energy) produces low serum levels, whereas the metastable b-polymorph (have high free energy so have greater solubility, absorption, and bio-avilability) yields much higher serum levels when the same dose is administered [2], [5], and [41].

Moreover, Norvir™, a semisolid capsules product which produced by Abbott company was failed in dissolution test after being in market that due to appearance of a new more stable crystalline polymorph of ritonavir (Form II) which held a lower thermodynamic solubility than the marketed (Form I)

[42]. The effect of a solvent or solvent mixture on the formation of erythromycin crystals was studied and the results illustrated that using solvent mixture of acetone and ethanol (3:1, v/v) induced the good shape and high purity crystals by comparison with other solvents such as isopropyl, 1 propanol

[43]. In addition, some anti-inflammatory drugs for pulmonary delivery such as bedomethasone, dipropionate, beta-methasone, prednisolone were micronized by controlled crystallization process without any milling process by using solvent change method which improves powder properties for inhalation [44],moreover, zinc-free insulin crystals can be prepared in the inhalation size range of 0.2-5 mm by using the solvent change (antisolvent precipitation) method [45]. On the other hand, synthesis, crystallization, separation and agglomeration can be incorporation in one step which defined as spherical crystallization; one must be mentioned, this technique can improve mechanical properties like compressibility, packability and flowability for API's powders such as naproxen, aminophylline, and salicylic acid crystals

[46-48].

Fig. 7 - Comparison of mean blood serum levels after the administration of chloramphenicol palmitate suspensions using varying ratios of the stable (a) and the metastable (ß) polymorphos. M, 100% a polymorph; N, 25:75 ß:a; O, 50:50 ß:a; P, 75:25 ß:a; L, 100% ß polymorph [41].

3. Growth rate dispersion & factors affected of it

Crystal growth rate dispersion (GRD) is a phenomenon, known as a great breadth and depth problem in the crystalline

Conclusion

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