# Polymorphic Forms of Lamivudine: Characterization, Estimation of Transition Temperature, and Stability Studies by Thermodynamic and Spectroscopic Studies

Authors: Renu Chadha; Poonam Arora; Swati Bhandari
Journal: ISRN Thermodynamics
 (2012)

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## Abstract

The present study is focused on estimation of transition temperature and stability of various forms of lamivudine. The forms were recrystallized from variety of solvents and preliminarily identification on the basis of SEM revealed existence of three forms (Forms I, II, III). DSC scans of Forms I and III show that these are metastable and undergo heat mediated transformation to Form IH and Form IIIH, respectively. Form II is phase pure with single sharp melting endotherm at 178.6°C. The thermal events are visually observed by hot stage microscopy. Enthalpy of solution of the forms is endothermic and magnitude varies in the order Form II > Form IL > Form IIIL  suggesting Form IIIL to be least crystalline which is well correlated with XRPD data. The transition temperature of the polymorphic pairs IL/IH and IIIL/IIIH derived from enthalpy of solution and solubility data revealed monotropy whereas enantiotropy exists in IIIH/II. The slurry experiments showed Form II to be thermodynamically most stable. Forms IL and IIIL though stable in water are converted to Form II in ethanol, acetonitrile, and propanol after 1 day. Form IIIL is converted to Form IL in water after 7 days and the observation is of importance as this instability can effect the pharmaceutical preparations whereas Form IL shows a balance between stability and solubility.


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## Body

## 1. Introduction

The increasing recognition of the importance of polymorphism to the pharmaceutical drug industry has generated a great deal of interest and the field has been evolving rapidly [1]. In fact, the systematic evaluation and characterization of the polymorphic forms of the drugs is essential and mandatory because important properties such as solubility and drug stability depend on the solid state structure [2, 3]. The thermodynamic relationships between polymorphic pairs classified as monotropic or enantiotropic, first developed by Berger and Ramberger, is of utmost importance and must be established carefully and accurately because as drug crystallizes from different solvents the kinetically favoured metastable polymorph appears first which can be isolated and characterized and can be formulated under certain conditions [4–6]. This metastable polymorph may undergo heat induced or solvent induced transformation to produce thermodynamically stable form at its own expense [6, 7]. Therefore, a precise knowledge of the stability of crystal forms and their interrelationship is critical for formulation development [8]. Thus, the objective of present work is to fully characterize the different polymorphic forms and to study the complex thermodynamic relationship between the polymorphic pairs of lamivudine.Lamivudine (Figure1), (2R, cis-4-amino-1-(2-hydroxymethyl-1, 3-oxathiolan-5-yl)-(1H)-pyrimidine-2-one, is a nucleoside reverse transcriptase inhibitor, used for the treatment of acquired immune deficiency syndrome (AIDS) [9]. Lamivudine in combination with other retroviral agents is indicated for the treatment of HIV-1 infection [10]. The solid state chemistry of this drug is of significant pharmaceutical interest as the drug is reported to exist in three crystalline forms. The two forms (Form I and II) reported in 1996 were again studied by Harris et al. in 1997 [11, 12]. Later in 2007, a new patent showing the existence of another polymorphic form III has appeared [13]. Unfortunately, all these studies lack in one or other aspect. The thermodynamic aspects of these polymorphs have not been taken into account and the transformation of one form to another has not been studied extensively. There are many lacunae in the reported literature which need to be filled for complete characterization of these polymorphs. Therefore, the purpose of the present work is to revisit these crystalline forms and the prime objective is to determine transition temperature of a polymorphic pairs and to interpret whether they are monotropically or enantiotropically related. The thermodynamic stability relationship of the polymorphic pair has also been determined from their melting temperature and enthalpy of solution data [14]. Besides this, the heat mediated and solvent mediated transformations are also emphasized in the present work.Figure 1
Chemical structure of lamivudine.


## 2. Materials and Methods

### 2.1. Materials

Lamivudine was obtained as a gift sample from Ranbaxy Laboratories Pvt. Ltd. (Poanta Sahib, India). Analytical grade solvents methanol, ethanol, ethyl acetate, chloroform, acetonitrile, hexane, heptane, 1-butanol, dimethylformamide (DMF), 1, 4-dioxane, and 2-propanol were used in this work.


### 2.2. Preparation of Polymorphs

The commercial sample of lamivudine was recrystallized from a variety of solvents and their mixtures to generate different crystal forms. Saturated solutions of lamivudine were prepared by heating in different solvents under constant stirring until most of lamivudine dissolved; the solutions were filtered and kept at room temperature until crystallization was complete (slow recrystallization). The further analysis of the recrystallized product by DSC and XRPD techniques showed that the crystallization ultimately resulted in only three polymorphic forms. Table1 summarizes the different solvent systems leading to the formation of the three distinct crystal forms of lamivudine.Table 1
Different solvent systems to prepare different crystal forms of lamivudine.
Solvent system
Form obtained
Shape
Water, Methanol,Toluene + ethanol, Ethanol, DMF + methanol, 1,4-dioxane
Form I
elongated needles
Ethyl acetate, Dry ethanol, Acetonitrile, 2-propanol, Toluene, Dry methanol,1,4-dioxane + methanol + water
Form II
prismatic crystals
Heptane + 1-butanolHexane + n-propanolChloroform
Form III
fine needles


### 2.3. Thermal Methods of Analysis

The DSC thermograms were obtained on DSC Q20, TA Instruments-Waters LLC, USA. The calorimeter was calibrated for temperature and heat flow accuracy using the melting of pure indium (mp 156.6°C and ΔH of 25.45 J g−1). A mass between 2 and 8 mg was taken into the aluminium pan, covered with lid and sealed. DSC curves were obtained under a nitrogen purge of 50 mL per minute at a heating rate of 10° per minute with the temperature range from 50 to 250°C.The TGA scans were obtained on TGA, TA Instruments-Waters LLC, USA. TGA traces were recorded at heating rates of 10° per minute under a nitrogen purge of 50 mL per minute. Samples with masses between 1 and 10 mg were analyzed using platinum pan. Mass loss (%) was calculated based on the mass of the original sample.


### 2.4. X-Ray Powder Diffraction Analysis

The powder diffraction patterns were recorded on an X-ray diffractometer (XPERT-PRO, PANalytical, Netherlands) with Cu as tube anode. The diffractograms were recorded under following conditions: voltage 40 kV, 35 mA, angular range 5, and fixed divergence slit. Approximately 200 mg of samples were loaded into the sample holder for analysis.


### 2.5. Scanning Electron Microscopy

A Jeol JSM-6100 scanning electron microscope was used to obtain photomicrographs of lamivudine and its polymorphs. Samples were mounted on a metal stub with an adhesive tape and coated under vacuum with gold.


### 2.6. Microcalorimetric Study

Calorimetric studies were performed on Microreaction calorimeter obtained from Thermal Hazards Technology, UK. Phosphate buffer (pH 7.0) was used to determine the enthalpy of solution and the measurements were performed at 25°C and 37°C. The size of sample used in this study ranged from 1 to 10 mg and was weighed (Sartorius Model CP225D) into a cylindrical glass tube covered with parafilm on one side. This cylindrical tube was submerged into the ampoule containing the solvent. A plunger with a cap was put from the open end of the tube. The same solvent was put into the reference ampoule. These were put into the sample and reference holes until both rest on the base of the holes. The parafilm was shattered mechanically by means of plunger.


### 2.7. Aqueous Solubility Measurement

MSW-275 (Macro scientific works, New Delhi) shaker was used for measuring aqueous solubility of different forms of lamivudine. Solubility studies were performed by adding 10 mg of sample in flask containing 10 mL of phosphate buffer pH 7.0 (50 mM). The mixture was shaken at 37°C for 24 h. The aliquots were filtered through 0.45μm membrane filter and analyzed spectrophotometrically at 270 nm. The standard plot of lamivudine was prepared by dissolving a weighed amount of sample in phosphate buffer pH 7.0, suitably diluted and absorbance taken at wavelength 270 nm on a spectrophotometer. E1%1cm was calculated.


### 2.8. Solvent Mediated Transformation Studies

The stability relationships and transformation between polymorphs were assessed at 25°C by slurry conversion method. Forms IL and IIIL and mixtures of these two forms prepared by mild blending of the solids in 1 : 1 ratio were suspended in water, ethanol, acetonitrile, and propanol and were maintained under constant shaking. To assess the conversion kinetics, the samples were withdrawn at 24 h and after 7 days. The suspensions were then filtered and analyzed by DSC and XRPD and compared with the starting material.


## 2.1. Materials

Lamivudine was obtained as a gift sample from Ranbaxy Laboratories Pvt. Ltd. (Poanta Sahib, India). Analytical grade solvents methanol, ethanol, ethyl acetate, chloroform, acetonitrile, hexane, heptane, 1-butanol, dimethylformamide (DMF), 1, 4-dioxane, and 2-propanol were used in this work.


## 2.2. Preparation of Polymorphs

The commercial sample of lamivudine was recrystallized from a variety of solvents and their mixtures to generate different crystal forms. Saturated solutions of lamivudine were prepared by heating in different solvents under constant stirring until most of lamivudine dissolved; the solutions were filtered and kept at room temperature until crystallization was complete (slow recrystallization). The further analysis of the recrystallized product by DSC and XRPD techniques showed that the crystallization ultimately resulted in only three polymorphic forms. Table1 summarizes the different solvent systems leading to the formation of the three distinct crystal forms of lamivudine.Table 1
Different solvent systems to prepare different crystal forms of lamivudine.
Solvent system
Form obtained
Shape
Water, Methanol,Toluene + ethanol, Ethanol, DMF + methanol, 1,4-dioxane
Form I
elongated needles
Ethyl acetate, Dry ethanol, Acetonitrile, 2-propanol, Toluene, Dry methanol,1,4-dioxane + methanol + water
Form II
prismatic crystals
Heptane + 1-butanolHexane + n-propanolChloroform
Form III
fine needles


## 2.3. Thermal Methods of Analysis

The DSC thermograms were obtained on DSC Q20, TA Instruments-Waters LLC, USA. The calorimeter was calibrated for temperature and heat flow accuracy using the melting of pure indium (mp 156.6°C and ΔH of 25.45 J g−1). A mass between 2 and 8 mg was taken into the aluminium pan, covered with lid and sealed. DSC curves were obtained under a nitrogen purge of 50 mL per minute at a heating rate of 10° per minute with the temperature range from 50 to 250°C.The TGA scans were obtained on TGA, TA Instruments-Waters LLC, USA. TGA traces were recorded at heating rates of 10° per minute under a nitrogen purge of 50 mL per minute. Samples with masses between 1 and 10 mg were analyzed using platinum pan. Mass loss (%) was calculated based on the mass of the original sample.


## 2.4. X-Ray Powder Diffraction Analysis

The powder diffraction patterns were recorded on an X-ray diffractometer (XPERT-PRO, PANalytical, Netherlands) with Cu as tube anode. The diffractograms were recorded under following conditions: voltage 40 kV, 35 mA, angular range 5, and fixed divergence slit. Approximately 200 mg of samples were loaded into the sample holder for analysis.


## 2.5. Scanning Electron Microscopy

A Jeol JSM-6100 scanning electron microscope was used to obtain photomicrographs of lamivudine and its polymorphs. Samples were mounted on a metal stub with an adhesive tape and coated under vacuum with gold.


## 2.6. Microcalorimetric Study

Calorimetric studies were performed on Microreaction calorimeter obtained from Thermal Hazards Technology, UK. Phosphate buffer (pH 7.0) was used to determine the enthalpy of solution and the measurements were performed at 25°C and 37°C. The size of sample used in this study ranged from 1 to 10 mg and was weighed (Sartorius Model CP225D) into a cylindrical glass tube covered with parafilm on one side. This cylindrical tube was submerged into the ampoule containing the solvent. A plunger with a cap was put from the open end of the tube. The same solvent was put into the reference ampoule. These were put into the sample and reference holes until both rest on the base of the holes. The parafilm was shattered mechanically by means of plunger.


## 2.7. Aqueous Solubility Measurement

MSW-275 (Macro scientific works, New Delhi) shaker was used for measuring aqueous solubility of different forms of lamivudine. Solubility studies were performed by adding 10 mg of sample in flask containing 10 mL of phosphate buffer pH 7.0 (50 mM). The mixture was shaken at 37°C for 24 h. The aliquots were filtered through 0.45μm membrane filter and analyzed spectrophotometrically at 270 nm. The standard plot of lamivudine was prepared by dissolving a weighed amount of sample in phosphate buffer pH 7.0, suitably diluted and absorbance taken at wavelength 270 nm on a spectrophotometer. E1%1cm was calculated.


## 2.8. Solvent Mediated Transformation Studies

The stability relationships and transformation between polymorphs were assessed at 25°C by slurry conversion method. Forms IL and IIIL and mixtures of these two forms prepared by mild blending of the solids in 1 : 1 ratio were suspended in water, ethanol, acetonitrile, and propanol and were maintained under constant shaking. To assess the conversion kinetics, the samples were withdrawn at 24 h and after 7 days. The suspensions were then filtered and analyzed by DSC and XRPD and compared with the starting material.


## 3. Results and Discussion

### 3.1. Recrystallization Product

The preliminary investigation of recrystallized product of lamivudine from various solvents by visual inspection and particle morphology by SEM categorized these into three distinct forms. The forms obtained from water, methanol, ethanol, 1,4-dioxane, ethyl acetate, mixture of toluene and ethanol, and a mixture of DMF and methanol showed elongated needle shaped acicular crystals and are designated as Form I (Figure2(a)). The forms obtained from dry ethanol, dry methanol, 2-propanol, toluene, and a mixture of 1,4-dioxane, methanol, and water showed prismatic crystals indicating these to be similar and are designated as Form II (Figure 2(b)). Form III was obtained from chloroform, a mixture of heptane and 1-butanol, and a mixture of hexane and propanol. The crystals of Form III were found to be very fine needles which were easily distinguishable from Form I (Figure 2(c)). Thus on the basis of morphology existence of only three new polymorphic forms was confirmed after screening from various solvents.Scanning electron microscopy of (a) Form I, (b) Form II, and (c) Form III of lamivudine.
(a)
(b)
(c)


### 3.2. Thermal Analysis of Polymorphic Forms

Investigation of the thermal behavior by DSC and TGA techniques shows the existence of low melting metastable forms before they are converted into higher melting stable forms in Form I and III. Thermodynamic relationship between different phases (enantiotropic or monotropic) and transitions between different crystal forms are determined by employing these techniques. The hot stage microscope provides the visual confirmation of events occurring during the transformation of one form to another.DSC scan of Form I showed two endotherms peaking at 117.5°C and 178.2°C separated by an exotherm at 123.8°C (Figure3). Prior to these events there is a very small endotherm in the temperature range 70–100°C. The thermogravimetric scan confirms the presence of unbound water at a level of 1% by weight (corresponding approximately to 1 mole of water for every 10 moles of lamivudine) in the temperature range 70–100°C (Figure 4).Figure 3
DSC plots of (a) Form IL, (b) Form II, and (c) Form IIIL of lamivudine.Figure 4
TGA plots of (a) Form IL, (b) Form II, and (c) Form IIIL of lamivudine.A broad endotherm at 117.4°C is not accompanied by any mass loss in TGA scan, suggesting this endotherm to be a melting event and negate the presence of any solvents. This melting is immediately followed by a small exotherm representing either a solid-solid transition or a liquid-solid transition. The exact nature of transition is confirmed by hot stage microscopy which shows that the crystals of Form I start melting at 118°C; however, the new crystal form starts to grow at 124°C from the melt of previous crystals. These crystals finally melt at 178°C to give a sharp melting endotherm in the HSM images (Figure5). These thermal events represent a liquid-solid transition to generate Form IH (high melting form) from the melt of Form IL (low melting form). This phenomenon suggests this conversion to be heat mediated transformation. The very low enthalpy of fusion indicates that the low melting endotherm is immediately or simultaneously accompanied by exothermic crystallization into other polymorphic form. The Form I prepared in the present study is comparable to some extent with Form I reported in literature [11, 12]. In both studies the forms showed endo-/exo-events followed by sharp melting endotherm. However, the solvent system used in our study varies from polar to nonpolar whereas the previous authors have used only polar solvents. Moreover, Harris et al. have shown the presence of bound water at a level of 2% by weight but in our study only unbound nonstoichiometric water is found to be associated. The thermodynamic relationship and the solvent mediated transformations of the forms have not been reported by previous workers and are a part of our work. All these parameters are dealt with in the present work.Hot stage micrographs of Form I.
(a)
(b)
(c)
(d)
(e)
(f)Form II showed single sharp melting endotherm at 178.6°C in DSC with no mass loss in the TGA scan up to 180°C (Figure4) indicating it to be a phase pure form which is neither solvate nor hydrate. The HSM images show melting around 179°C (Figure 6). The melting temperature of Form II suggests this form to be thermodynamically more stable form. The literature survey reveals that a similar form with almost similar melting temperature exists; however, the crystallization solvents are different [12]. Moreover, other parameters such as enthalpy of fusion and visual inspection of melting by HSM are not reported.Hot stage micrographs of Form II.
(a)
(b)
(c)
(d)
(e)Regarding Form III, the preliminary investigation by DSC shows endo-/exopeaks as were observed in Form I. A broad endotherm accompanied by mass loss (0.2%) in TGA in the temperature range 50–100°C suggests unbound solvent in nonstoichiometric ratio whereas the two endotherms peaking at 114.3°C and 173.8°C separated by an exothermic peak at 118.6°C are suggestive of phase-phase transition. The HSM images confirmed it to be a liquid-solid transition to generate Form IIIH (high melting form) from the melt of Form IIIL (low melting form) (Figure 7). This form (Form IIIH) finally melts at 175.8°C.Hot stage micrographs of Form III.
(a)
(b)
(c)
(d)
(e)
(f)The melting temperature and heat of fusion of the higher melting Form IH is similar to the heat of fusion of Form II suggesting that Form IL might have converted to Form II after melting; however, the melting temperature and heat of fusion of the higher melting Form IIIH is different which suggests that Form IIIL has converted to a new polymorphic form after melting (Table 2).Table 2
Thermal characteristics of Form I, Form II, Form IIH, Form IIIL, and Form IIIH of lamivudine by differential scanning calorimetry.
Sample
Melting temperature(°C)
Enthalpy of fusion(J/g)
Form IL
117.5
19.6
Form IH
178.2
109.9
Form II
178.6
90.9
Form IIIL
114.3
13.9
Form IIIH
173.8
43.7


#### 3.2.1. Heat Mediated Transformation and Thermodynamic Relationship

Table2 shows that Forms IH or II and IIIH obtained after phase-phase transition (liquid-solid) of Forms IL and IIIL, respectively, show higher melting temperature and higher enthalpy of fusion suggesting existence of monotropic relationship between them. The polymorphic pair IIIH/II show enantiotropic transition as the high melting form has lower heat of fusion and the low melting form has higher heat of fusion. The liquid-solid transition as shown by HSM also confirms that the polymorphic pairs IL/II and IIIL/IIIH are monotropically related. To confirm the occurrence of heat mediated transformation of metastable Form IL and IIIL to stable forms as well as to determine whether the transition is reversible or irreversible a separate experiment was performed. Forms I and III were heated on a DSC furnace just above the end of crystallization exotherm, cooled to room temperature (28°C), and heated again to the melting point. It was observed that the first endotherm at 117.4°C in Form I and at 116.3°C in Form III disappeared in the DSC graph of the repeated heating curve (Figure 8). The first endotherm corresponding to metastable form does not appear in the DSC scan even after 5 days. These heating-cooling experiments suggest kinetically irreversible transition confirming Forms IL/IH and IIIL/IIIH to be monotropes.Figure 8
DSC plots of (a) Form IH and (b) Form IIIH of lamivudine.


### 3.3. X-Ray Powder Diffraction (XRPD)

One of the reliable ways to distinguish the various forms of lamivudine is with X-ray powder diffraction. The XRPD patterns of Forms IL, II, and IIIL were recorded at room temperature (Figure 9). All the forms can be easily discriminated by their diffraction pattern particularly by presence and absence of peaks between 9° and 30°. The XRPD pattern of Form IL showed characteristic peaks at 9.0°, 10.1°, 11.6°, 12.1°, 13.3°, 14.7°, 16.9°, 17.5°, 18.5°, 19.9°, 20.5° (100% relative intensity), 24.9°, 25.3°, 26.4°, 27.2°, and 28.3°. The indicative peaks for Form II occur at 11.2°, 12.9°, 14.5°, 15.3°, 17.5°, and 18.3° whereas the characteristic peaks at 22.5°, 31.0°, 33.9°, and 35.4° were absent as compared to Form IL indicating formation of a new phase. The XRPD pattern of Form IIIL showed new peaks at 9.9°, 10.8°, 11.8°, 12.8°, 13.1°, 18.4°, 19.0°, 31.0°, 36.2°, and 36.7° making it different from the other two forms. This form also showed the absence of peak at 14.3°.Figure 9
XRPD patterns of (a) Form IL, and (b) Form II, and (c) Form IIIL of lamivudine.


#### 3.3.1. Conformation of Heat Mediated Transformation with XRPD

In order to explicitly identify to which form the lower melting forms have transitioned to upon heating, different heating experiments were performed. Forms IL and IIIL were heated at temperature 135°C and 130°C, respectively, and held at this temperature for 50 min to ensure complete conversion. The samples were then cooled to room temperature in a desiccator with zero relative humidity and were subjected to XRPD to identify the resulting forms. The XRPD pattern of Form IH corresponds well to the pattern reported for Form II which revealed that this form transferred to Form II upon heating. However, The XRPD pattern of Form IIIH showed appearance of new peaks at 8.3°, 12.8°, 19.0°, and 29.6° indicating formation of a new phase (Figure 10). This supports the observation made by DSC that Form IL has converted to Form II and Form IIIL has converted to a new polymorphic form after heat mediated transformation.Figure 10
XRPD patterns of (a) Form IH and (b) Form IIIH of lamivudine.


### 3.4. Solution Calorimetry

The enthalpy of solution has been utilized to differentiate the metastable Forms IL and IIIL from the stable high melting forms IH and IIIH. Moreover, this data is also required to determine the transition temperature for conversion of metastable forms to stable forms and to determine the stability relationship in a particular polymorphic pair. The molar enthalpy of solution (ΔsolH) determined in phosphate buffer pH 7.0 at 25°C and 37°C is given in Table 3. All the forms showed endothermic behavior and the absolute value of molar enthalpy of solution followed the order: Form II > Form IL > Form IIIL. The highest endothermic ΔsolH associated with Form II and this is very well correlated with XRPD studies. Form IL is less endothermic, less crystalline, and obviously less stable. These results are somewhat contrary to the results reported by Jozwiakowski et al. The authors have determined the ΔsolH of Forms I and II in various solvents ranging from water to alcohols and have shown Form II to be less endothermic than Form IL whereas in the present study Form II is more endothermic. This variation may be due to the fact that Form IL is a hydrate while in the current work water is not incorporated into the crystal lattice of Form IL. The lowest ΔsolH for Form IIIL indicates this form to be least crystalline. The molar enthalpy of solution is increased with increase in the temperature (Table 3). The enthalpy of solution was also determined for the high melting Forms IH and IIIH. The molar enthalpy of solution was found to be more endothermic than their corresponding low melting forms at all the temperatures which is a consequence of lattice energy being more in the higher melting stable crystal form. Moreover, the magnitude of ΔsolH of Forms IH and II is comparable suggesting the similar nature of their crystal lattices. The results further suggest that Form IIIL is a new polymorphic form.Table 3
Enthalpy of solution and solubility of Form I, Form IIL, Form IIH, Form IIIL, and Form IIIH of lamivudine.
Sample
Enthalpy of solution
Solubility
(kJ/mol)
(×10−1 moles/L)
25°C
37°C
25°C
37°C
Form IL
17.72
18.73
0.42
0.46
Form IH
18.22
19.45
0.39
0.41
Form II
18.83
19.90
0.38
0.40
Form IIIL
12.87
14.99
0.58
0.61
Form IIIH
14.13
16.12
0.48
0.52


### 3.5. Solubility Studies

Solubility of all the low melting and high melting forms was determined in phosphate buffer (pH 7.0) at 25°C and 37°C and is given in Table3. The solubility study suggests that Form II is least soluble while Form IIIL is most soluble. The solubility of Forms IH and II are almost identical indicating that they have similar free energies. These similarities agree well with thermoanalytical and XRPD data. The solubility of high melting forms (IH and IIIH) is lower than their corresponding low melting forms; however, the solubility of Form IIIH is found to be still higher than Forms IH and II.


### 3.6. Transition Temperature Determination

The transition temperature of polymorphic pairs IL/II, IIIL/IIIH, and IIIH/II has been estimated by utilizing solubility and enthalpy of solution data. The enthalpy of transition (ΔH(T)), free energy of transition (ΔG(T)), and entropy of transition (ΔS(T)) accompanying the transition of lower melting form to higher melting form are also determined at 25°C and 37°C using the following equations (Gu and Grant) and are given Table 4 one has.
(1)ΔH(T)=ΔsolHL-ΔsolHH,
where ΔsolHL is the enthalpy of solution of lower melting form and ΔsolHH is the enthalpy of solution of higher melting form one has
(2)ΔG(T)=-RTlnSLSH,
where SL is the solubility of low melting polymorph and SH is the solubility of high melting polymorph.Table 4
The enthalpy of transition (ΔH(T)), free energy of transition (ΔG(T)), entropy of transition (ΔS(T)), and transition temperature (Tt) of different polymorphic pairs at 25°C and 37°C.
Δ
H
trans
(kJ/mol)
Δ
G
trans (kJ/mol)
Δ
S
trans (J/mol)
T
t (K)
25°C
37°C
25°C
37°C
25°C
37°C
25°C
37°C
Form IL→II
−0.49
−0.72
−0.18
−0.26
−1.05
−1.52
467.6
468.5
Form IIIL→IIIH
−1.26
−1.13
−0.45
−0.41
−2.72
−2.42
464.3
465.8
Form IIIH→II
−4.69
−3.87
−0.57
−0.64
−13.84
−10.83
339.4
340.4The entropy of transition between the two forms is calculated by the following equation:(3)ΔS(T)={ΔH(T)-ΔG(T)}T.
At the transition temperature, Tt,
(4)ΔtransG=0=ΔtransH-Tt×ΔtransS.
Hence,
(5)Tt=ΔtransHΔtransS.
The negative value of ΔG and ΔS for transition of IL to II indicates that higher melting forms have lower Gibb’s free energy as well as lower entropy. However, the dominant factor in the free energy differences for all the polymorphic pairs at both temperatures is the difference in the enthalpy between these two phases. The transition temperature for polymorphic pairs IL/II and IIIL/IIIH was found to be higher than the melting temperature of both the forms suggesting them to be monotropically related whereas the transition temperature of polymorphic pair IH/II was between 0 K and melting point of lower melting form indicating this pair to be enantiotropically related.


### 3.7. Solvent Mediated Transformation and Stability of Various Forms

The previous section has shown that Form IIIL is most soluble which can be further used for formulation development. However, the most suitable form is the one which exhibits an appropriate balance between solubility and stability. Therefore, it is important to establish the stability of these forms. Thus the solvent mediated transformation experiments of forms (IL, II, and IIIL) of lamivudine were performed in water, ethanol, acetonitrile, and propanol (Table 5). Form IL is stable in water but undergoes transformation into Form II when suspended in ethanol, acetonitrile, and propanol. On the other hand, mixture of Forms IL and II slowly converts to Form II after 7 days in these solvents. Moreover, water has no effect on Form IIIL up to 24 h but it undergoes a transformation to Form IL after 7 days. However, it transforms to stable Form II in ethanol, acetonitrile, and propanol. The analysis of forms recovered after suspending solvents revealed that Form IL is preferred over Form II in water whereas in ethanol, acetonitrile, and propanol Form II is the preferred form.Table 5
Stability of polymorphs by slurry conversion method.
Initial polymorph
Water
Ethanol
Acetonitrile
Propanol
1 day stirring
7 day stirring
1 day stirring
7 day stirring
1 day stirring
7 day stirring
1 day stirring
7 day stirring
Form IL
IL
IL
II
II
II
II
II
II
Form IIIL
IIIL
IL
II
II
II
II
II
II
Form IL/II
IL
IL
II
II
II
II
II
II
Form IIIL/II
IIIL
IL
II
II
II
II
II
II


## 3.1. Recrystallization Product

The preliminary investigation of recrystallized product of lamivudine from various solvents by visual inspection and particle morphology by SEM categorized these into three distinct forms. The forms obtained from water, methanol, ethanol, 1,4-dioxane, ethyl acetate, mixture of toluene and ethanol, and a mixture of DMF and methanol showed elongated needle shaped acicular crystals and are designated as Form I (Figure2(a)). The forms obtained from dry ethanol, dry methanol, 2-propanol, toluene, and a mixture of 1,4-dioxane, methanol, and water showed prismatic crystals indicating these to be similar and are designated as Form II (Figure 2(b)). Form III was obtained from chloroform, a mixture of heptane and 1-butanol, and a mixture of hexane and propanol. The crystals of Form III were found to be very fine needles which were easily distinguishable from Form I (Figure 2(c)). Thus on the basis of morphology existence of only three new polymorphic forms was confirmed after screening from various solvents.Scanning electron microscopy of (a) Form I, (b) Form II, and (c) Form III of lamivudine.
(a)
(b)
(c)


## 3.2. Thermal Analysis of Polymorphic Forms

Investigation of the thermal behavior by DSC and TGA techniques shows the existence of low melting metastable forms before they are converted into higher melting stable forms in Form I and III. Thermodynamic relationship between different phases (enantiotropic or monotropic) and transitions between different crystal forms are determined by employing these techniques. The hot stage microscope provides the visual confirmation of events occurring during the transformation of one form to another.DSC scan of Form I showed two endotherms peaking at 117.5°C and 178.2°C separated by an exotherm at 123.8°C (Figure3). Prior to these events there is a very small endotherm in the temperature range 70–100°C. The thermogravimetric scan confirms the presence of unbound water at a level of 1% by weight (corresponding approximately to 1 mole of water for every 10 moles of lamivudine) in the temperature range 70–100°C (Figure 4).Figure 3
DSC plots of (a) Form IL, (b) Form II, and (c) Form IIIL of lamivudine.Figure 4
TGA plots of (a) Form IL, (b) Form II, and (c) Form IIIL of lamivudine.A broad endotherm at 117.4°C is not accompanied by any mass loss in TGA scan, suggesting this endotherm to be a melting event and negate the presence of any solvents. This melting is immediately followed by a small exotherm representing either a solid-solid transition or a liquid-solid transition. The exact nature of transition is confirmed by hot stage microscopy which shows that the crystals of Form I start melting at 118°C; however, the new crystal form starts to grow at 124°C from the melt of previous crystals. These crystals finally melt at 178°C to give a sharp melting endotherm in the HSM images (Figure5). These thermal events represent a liquid-solid transition to generate Form IH (high melting form) from the melt of Form IL (low melting form). This phenomenon suggests this conversion to be heat mediated transformation. The very low enthalpy of fusion indicates that the low melting endotherm is immediately or simultaneously accompanied by exothermic crystallization into other polymorphic form. The Form I prepared in the present study is comparable to some extent with Form I reported in literature [11, 12]. In both studies the forms showed endo-/exo-events followed by sharp melting endotherm. However, the solvent system used in our study varies from polar to nonpolar whereas the previous authors have used only polar solvents. Moreover, Harris et al. have shown the presence of bound water at a level of 2% by weight but in our study only unbound nonstoichiometric water is found to be associated. The thermodynamic relationship and the solvent mediated transformations of the forms have not been reported by previous workers and are a part of our work. All these parameters are dealt with in the present work.Hot stage micrographs of Form I.
(a)
(b)
(c)
(d)
(e)
(f)Form II showed single sharp melting endotherm at 178.6°C in DSC with no mass loss in the TGA scan up to 180°C (Figure4) indicating it to be a phase pure form which is neither solvate nor hydrate. The HSM images show melting around 179°C (Figure 6). The melting temperature of Form II suggests this form to be thermodynamically more stable form. The literature survey reveals that a similar form with almost similar melting temperature exists; however, the crystallization solvents are different [12]. Moreover, other parameters such as enthalpy of fusion and visual inspection of melting by HSM are not reported.Hot stage micrographs of Form II.
(a)
(b)
(c)
(d)
(e)Regarding Form III, the preliminary investigation by DSC shows endo-/exopeaks as were observed in Form I. A broad endotherm accompanied by mass loss (0.2%) in TGA in the temperature range 50–100°C suggests unbound solvent in nonstoichiometric ratio whereas the two endotherms peaking at 114.3°C and 173.8°C separated by an exothermic peak at 118.6°C are suggestive of phase-phase transition. The HSM images confirmed it to be a liquid-solid transition to generate Form IIIH (high melting form) from the melt of Form IIIL (low melting form) (Figure 7). This form (Form IIIH) finally melts at 175.8°C.Hot stage micrographs of Form III.
(a)
(b)
(c)
(d)
(e)
(f)The melting temperature and heat of fusion of the higher melting Form IH is similar to the heat of fusion of Form II suggesting that Form IL might have converted to Form II after melting; however, the melting temperature and heat of fusion of the higher melting Form IIIH is different which suggests that Form IIIL has converted to a new polymorphic form after melting (Table 2).Table 2
Thermal characteristics of Form I, Form II, Form IIH, Form IIIL, and Form IIIH of lamivudine by differential scanning calorimetry.
Sample
Melting temperature(°C)
Enthalpy of fusion(J/g)
Form IL
117.5
19.6
Form IH
178.2
109.9
Form II
178.6
90.9
Form IIIL
114.3
13.9
Form IIIH
173.8
43.7


### 3.2.1. Heat Mediated Transformation and Thermodynamic Relationship

Table2 shows that Forms IH or II and IIIH obtained after phase-phase transition (liquid-solid) of Forms IL and IIIL, respectively, show higher melting temperature and higher enthalpy of fusion suggesting existence of monotropic relationship between them. The polymorphic pair IIIH/II show enantiotropic transition as the high melting form has lower heat of fusion and the low melting form has higher heat of fusion. The liquid-solid transition as shown by HSM also confirms that the polymorphic pairs IL/II and IIIL/IIIH are monotropically related. To confirm the occurrence of heat mediated transformation of metastable Form IL and IIIL to stable forms as well as to determine whether the transition is reversible or irreversible a separate experiment was performed. Forms I and III were heated on a DSC furnace just above the end of crystallization exotherm, cooled to room temperature (28°C), and heated again to the melting point. It was observed that the first endotherm at 117.4°C in Form I and at 116.3°C in Form III disappeared in the DSC graph of the repeated heating curve (Figure 8). The first endotherm corresponding to metastable form does not appear in the DSC scan even after 5 days. These heating-cooling experiments suggest kinetically irreversible transition confirming Forms IL/IH and IIIL/IIIH to be monotropes.Figure 8
DSC plots of (a) Form IH and (b) Form IIIH of lamivudine.


## 3.2.1. Heat Mediated Transformation and Thermodynamic Relationship

Table2 shows that Forms IH or II and IIIH obtained after phase-phase transition (liquid-solid) of Forms IL and IIIL, respectively, show higher melting temperature and higher enthalpy of fusion suggesting existence of monotropic relationship between them. The polymorphic pair IIIH/II show enantiotropic transition as the high melting form has lower heat of fusion and the low melting form has higher heat of fusion. The liquid-solid transition as shown by HSM also confirms that the polymorphic pairs IL/II and IIIL/IIIH are monotropically related. To confirm the occurrence of heat mediated transformation of metastable Form IL and IIIL to stable forms as well as to determine whether the transition is reversible or irreversible a separate experiment was performed. Forms I and III were heated on a DSC furnace just above the end of crystallization exotherm, cooled to room temperature (28°C), and heated again to the melting point. It was observed that the first endotherm at 117.4°C in Form I and at 116.3°C in Form III disappeared in the DSC graph of the repeated heating curve (Figure 8). The first endotherm corresponding to metastable form does not appear in the DSC scan even after 5 days. These heating-cooling experiments suggest kinetically irreversible transition confirming Forms IL/IH and IIIL/IIIH to be monotropes.Figure 8
DSC plots of (a) Form IH and (b) Form IIIH of lamivudine.


## 3.3. X-Ray Powder Diffraction (XRPD)

One of the reliable ways to distinguish the various forms of lamivudine is with X-ray powder diffraction. The XRPD patterns of Forms IL, II, and IIIL were recorded at room temperature (Figure 9). All the forms can be easily discriminated by their diffraction pattern particularly by presence and absence of peaks between 9° and 30°. The XRPD pattern of Form IL showed characteristic peaks at 9.0°, 10.1°, 11.6°, 12.1°, 13.3°, 14.7°, 16.9°, 17.5°, 18.5°, 19.9°, 20.5° (100% relative intensity), 24.9°, 25.3°, 26.4°, 27.2°, and 28.3°. The indicative peaks for Form II occur at 11.2°, 12.9°, 14.5°, 15.3°, 17.5°, and 18.3° whereas the characteristic peaks at 22.5°, 31.0°, 33.9°, and 35.4° were absent as compared to Form IL indicating formation of a new phase. The XRPD pattern of Form IIIL showed new peaks at 9.9°, 10.8°, 11.8°, 12.8°, 13.1°, 18.4°, 19.0°, 31.0°, 36.2°, and 36.7° making it different from the other two forms. This form also showed the absence of peak at 14.3°.Figure 9
XRPD patterns of (a) Form IL, and (b) Form II, and (c) Form IIIL of lamivudine.


### 3.3.1. Conformation of Heat Mediated Transformation with XRPD

In order to explicitly identify to which form the lower melting forms have transitioned to upon heating, different heating experiments were performed. Forms IL and IIIL were heated at temperature 135°C and 130°C, respectively, and held at this temperature for 50 min to ensure complete conversion. The samples were then cooled to room temperature in a desiccator with zero relative humidity and were subjected to XRPD to identify the resulting forms. The XRPD pattern of Form IH corresponds well to the pattern reported for Form II which revealed that this form transferred to Form II upon heating. However, The XRPD pattern of Form IIIH showed appearance of new peaks at 8.3°, 12.8°, 19.0°, and 29.6° indicating formation of a new phase (Figure 10). This supports the observation made by DSC that Form IL has converted to Form II and Form IIIL has converted to a new polymorphic form after heat mediated transformation.Figure 10
XRPD patterns of (a) Form IH and (b) Form IIIH of lamivudine.


## 3.3.1. Conformation of Heat Mediated Transformation with XRPD

In order to explicitly identify to which form the lower melting forms have transitioned to upon heating, different heating experiments were performed. Forms IL and IIIL were heated at temperature 135°C and 130°C, respectively, and held at this temperature for 50 min to ensure complete conversion. The samples were then cooled to room temperature in a desiccator with zero relative humidity and were subjected to XRPD to identify the resulting forms. The XRPD pattern of Form IH corresponds well to the pattern reported for Form II which revealed that this form transferred to Form II upon heating. However, The XRPD pattern of Form IIIH showed appearance of new peaks at 8.3°, 12.8°, 19.0°, and 29.6° indicating formation of a new phase (Figure 10). This supports the observation made by DSC that Form IL has converted to Form II and Form IIIL has converted to a new polymorphic form after heat mediated transformation.Figure 10
XRPD patterns of (a) Form IH and (b) Form IIIH of lamivudine.


## 3.4. Solution Calorimetry

The enthalpy of solution has been utilized to differentiate the metastable Forms IL and IIIL from the stable high melting forms IH and IIIH. Moreover, this data is also required to determine the transition temperature for conversion of metastable forms to stable forms and to determine the stability relationship in a particular polymorphic pair. The molar enthalpy of solution (ΔsolH) determined in phosphate buffer pH 7.0 at 25°C and 37°C is given in Table 3. All the forms showed endothermic behavior and the absolute value of molar enthalpy of solution followed the order: Form II > Form IL > Form IIIL. The highest endothermic ΔsolH associated with Form II and this is very well correlated with XRPD studies. Form IL is less endothermic, less crystalline, and obviously less stable. These results are somewhat contrary to the results reported by Jozwiakowski et al. The authors have determined the ΔsolH of Forms I and II in various solvents ranging from water to alcohols and have shown Form II to be less endothermic than Form IL whereas in the present study Form II is more endothermic. This variation may be due to the fact that Form IL is a hydrate while in the current work water is not incorporated into the crystal lattice of Form IL. The lowest ΔsolH for Form IIIL indicates this form to be least crystalline. The molar enthalpy of solution is increased with increase in the temperature (Table 3). The enthalpy of solution was also determined for the high melting Forms IH and IIIH. The molar enthalpy of solution was found to be more endothermic than their corresponding low melting forms at all the temperatures which is a consequence of lattice energy being more in the higher melting stable crystal form. Moreover, the magnitude of ΔsolH of Forms IH and II is comparable suggesting the similar nature of their crystal lattices. The results further suggest that Form IIIL is a new polymorphic form.Table 3
Enthalpy of solution and solubility of Form I, Form IIL, Form IIH, Form IIIL, and Form IIIH of lamivudine.
Sample
Enthalpy of solution
Solubility
(kJ/mol)
(×10−1 moles/L)
25°C
37°C
25°C
37°C
Form IL
17.72
18.73
0.42
0.46
Form IH
18.22
19.45
0.39
0.41
Form II
18.83
19.90
0.38
0.40
Form IIIL
12.87
14.99
0.58
0.61
Form IIIH
14.13
16.12
0.48
0.52


## 3.5. Solubility Studies

Solubility of all the low melting and high melting forms was determined in phosphate buffer (pH 7.0) at 25°C and 37°C and is given in Table3. The solubility study suggests that Form II is least soluble while Form IIIL is most soluble. The solubility of Forms IH and II are almost identical indicating that they have similar free energies. These similarities agree well with thermoanalytical and XRPD data. The solubility of high melting forms (IH and IIIH) is lower than their corresponding low melting forms; however, the solubility of Form IIIH is found to be still higher than Forms IH and II.


## 3.6. Transition Temperature Determination

The transition temperature of polymorphic pairs IL/II, IIIL/IIIH, and IIIH/II has been estimated by utilizing solubility and enthalpy of solution data. The enthalpy of transition (ΔH(T)), free energy of transition (ΔG(T)), and entropy of transition (ΔS(T)) accompanying the transition of lower melting form to higher melting form are also determined at 25°C and 37°C using the following equations (Gu and Grant) and are given Table 4 one has.
(1)ΔH(T)=ΔsolHL-ΔsolHH,
where ΔsolHL is the enthalpy of solution of lower melting form and ΔsolHH is the enthalpy of solution of higher melting form one has
(2)ΔG(T)=-RTlnSLSH,
where SL is the solubility of low melting polymorph and SH is the solubility of high melting polymorph.Table 4
The enthalpy of transition (ΔH(T)), free energy of transition (ΔG(T)), entropy of transition (ΔS(T)), and transition temperature (Tt) of different polymorphic pairs at 25°C and 37°C.
Δ
H
trans
(kJ/mol)
Δ
G
trans (kJ/mol)
Δ
S
trans (J/mol)
T
t (K)
25°C
37°C
25°C
37°C
25°C
37°C
25°C
37°C
Form IL→II
−0.49
−0.72
−0.18
−0.26
−1.05
−1.52
467.6
468.5
Form IIIL→IIIH
−1.26
−1.13
−0.45
−0.41
−2.72
−2.42
464.3
465.8
Form IIIH→II
−4.69
−3.87
−0.57
−0.64
−13.84
−10.83
339.4
340.4The entropy of transition between the two forms is calculated by the following equation:(3)ΔS(T)={ΔH(T)-ΔG(T)}T.
At the transition temperature, Tt,
(4)ΔtransG=0=ΔtransH-Tt×ΔtransS.
Hence,
(5)Tt=ΔtransHΔtransS.
The negative value of ΔG and ΔS for transition of IL to II indicates that higher melting forms have lower Gibb’s free energy as well as lower entropy. However, the dominant factor in the free energy differences for all the polymorphic pairs at both temperatures is the difference in the enthalpy between these two phases. The transition temperature for polymorphic pairs IL/II and IIIL/IIIH was found to be higher than the melting temperature of both the forms suggesting them to be monotropically related whereas the transition temperature of polymorphic pair IH/II was between 0 K and melting point of lower melting form indicating this pair to be enantiotropically related.


## 3.7. Solvent Mediated Transformation and Stability of Various Forms

The previous section has shown that Form IIIL is most soluble which can be further used for formulation development. However, the most suitable form is the one which exhibits an appropriate balance between solubility and stability. Therefore, it is important to establish the stability of these forms. Thus the solvent mediated transformation experiments of forms (IL, II, and IIIL) of lamivudine were performed in water, ethanol, acetonitrile, and propanol (Table 5). Form IL is stable in water but undergoes transformation into Form II when suspended in ethanol, acetonitrile, and propanol. On the other hand, mixture of Forms IL and II slowly converts to Form II after 7 days in these solvents. Moreover, water has no effect on Form IIIL up to 24 h but it undergoes a transformation to Form IL after 7 days. However, it transforms to stable Form II in ethanol, acetonitrile, and propanol. The analysis of forms recovered after suspending solvents revealed that Form IL is preferred over Form II in water whereas in ethanol, acetonitrile, and propanol Form II is the preferred form.Table 5
Stability of polymorphs by slurry conversion method.
Initial polymorph
Water
Ethanol
Acetonitrile
Propanol
1 day stirring
7 day stirring
1 day stirring
7 day stirring
1 day stirring
7 day stirring
1 day stirring
7 day stirring
Form IL
IL
IL
II
II
II
II
II
II
Form IIIL
IIIL
IL
II
II
II
II
II
II
Form IL/II
IL
IL
II
II
II
II
II
II
Form IIIL/II
IIIL
IL
II
II
II
II
II
II


## 4. Conclusion

The DSC and SEM results suggest that Forms I and III in the present study are sensitive to thermal stress and the heat mediated transformation of these forms leads to generation of stable Form II and a new polymorphic form, respectively. The interpretation of the DSC data is facilitated by visual observations in thermal microscopy. Monotropic relationship has been identified in the polymorphic pairs IL/II and IIIL/IIIH while Form IIIH is shown to be enantiotropic modification of Form II. On the basis of comparison of differences between the enthalpies of solution and XRPD data, Form IIIL is found to be least crystalline and most soluble. However, the metastable Form IL, which shows better solubility than Form II, though transforms to Form II in solvents but is stable in aqueous suspension and can be categorized as suitable candidate for solid dosage.



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*Source: 671027-2012-11-14.xml*