Research Article | Open Access
Effect of Hydroxylamine Sulfate on Volumetric Behavior of Glycine, L-Alanine, and L-Arginine in Aqueous Solution
The apparent molar volumes of glycine, L-alanine, and L-arginine in aqueous hydroxylamine sulfate solutions have been determined at K and atmospheric pressure. The standard partial molar volumes, , corresponding partial molar volumes of transfer, , and hydration numbers, , have been calculated for these α-amino acids from the experimental data. The values are positive for glycine, L-alanine, and L-arginine and are all increased with the increase in the concentration of hydroxylamine ions. These parameters obtained from the volumetric data are interpreted in terms of various mixing effects between amino acids and hydroxylamine sulfate in aqueous solutions.
In recent years, the denaturation and renaturation behavior of biological molecules such as proteins in aqueous solutions has been the subject of extensive investigation [1–3]. However, the complex configurational and conformational factors affecting the structure of protein in aqueous solutions make the direct interpretation from studies on proteins very difficult . Volumetric and transport properties of amino acids such as density and viscosity have been extensively investigated and can provide valuable information for conformational stability and unfolding behavior of globular proteins in aqueous solutions [5–13].
It is well recognized that inorganic and organic salts can produce remarkable effects on the conformation and properties of proteins in aqueous solutions. Hydroxylamine derivatives are always used by biologists for their ability to introduce random mutations by switching different base pairs . Hydroxylamine can also be applied to selectively cleave peptide bonds in peptides and proteins . The highly biological activities of hydroxylamine derivatives make it quite interesting to study the behaviour of proteins in the presence of hydroxylamine salts . Consequently, the knowledge of thermophysical and thermodynamic properties of hydroxylamine with small molecules will be required and useful for obtaining information about various interactions occurring in aqueous hydroxylamine solutions with macromolecules.
In this study, we present experimental densities of glycine, L-alanine, and L-arginine in aqueous and aqueous hydroxylamine sulfate solutions of (0.10, 0.25, and 0.40) mol kg−1 at K and atmospheric pressure. From these data, the standard partial molar volumes (), standard partial molar volumes of transfer (), and molar hydration number () have been calculated. The results are discussed in terms of various solute-solute interactions and also their nature occurring in the ternary systems (amino acids + hydroxylamine sulfate + water).
Glycine, L-alanine, and L-arginine that were obtained from Amresco company have mass fraction purities greater than 0.99. These samples were recrystallized from aqueous ethanol solutions and dried in vacuum oven for 12 h at 333 K before use. Analytical grade hydroxylamine sulfate with purity of minimum mass fraction of 0.995 was obtained from UBE (Japan) and used as such after drying for 72 h in a vacuum desiccator at room temperature. The ultrapure water used for the preparation of the mixture with resistivity greater than 18.2 MΩ·cm was supplied by Nanopure Diamond UV/UF Water Purification System (Thermo Scientific Barnstead, USA). All of the studied solutions were freshly prepared by mass on an electronic balance to an accuracy of ±1 × 10−5 g.
The densities of the solutions were measured using an Anton Paar DMA 4500 density meter whose measurement cell temperature was controlled automatically within ±0.01 K of the selected value. The density meter was checked with freshly boiled ultrapure water and with dry air at atmospheric pressure. The uncertainty of the digital vibrating glass tube densimeter is stated as ±5.0 × 10−5 g·cm−3 in the density range of 0 to 3 g·cm−3.
3. Results and Discussion
The measured densities of glycine, L-alanine, and L-arginine in aqueous and aqueous hydroxylamine sulfate solutions with different concentrations of (0.10, 0.25, and 0.40) mol·kg−1 at K and atmospheric pressure have been shown in Tables 1 and 2, respectively.
|Molality of amino acids in the mixture of hydroxylamine sulfate + water as pure solvent.|
The apparent molar volume, , defined as the difference between the volume of the solution and the volume of the pure solvent per mole of solute, is given by the following equation: where and are the molar mass of the amino acid and the molality of the solute and and are the density of the aqueous solution and solvent, respectively. From Tables 1 and 2, we can find that the apparent molar volume increased with the increase in both concentrations of the amino acids and hydroxylamine sulfate.
In diluted conditions, the variation of the apparent molar volume, , for amino acids with the molality of hydroxylamine sulfate can be described by the linear relation where is an experimentally determined slope parameter and is the apparent molar volume at infinite dilution also known as the standard partial molar volume. The standard partial molar volumes for the amino acids in aqueous and aqueous solutions of hydroxylamine sulfate are reported in Table 3. The standard partial molar volumes for pure amino acids in aqueous solution agree well with these values from [17, 18]. It is well recognized that the standard partial molar volume is not necessarily the actual volume that was assigned to the amino acid because the water molecule that was near the amino acid does not have the same molar volume as pure water does. The water near the polar molecules or ions is electrostricted compressed by the electric field of solute. On the other hand, the standard partial molar volumes are all increased with the increase of both amino acids and hydroxylamine sulfate concentration in water. This may attribute to the fact that the hydrophilic-hydrophilic and ion-ion interactions between amino acids and hydroxylamine sulfate make their shrinking ability in water decrease and make more water to be released.
|Molality of hydroxylamine sulfate in water.|
Partial molar volumes of transfer, , at infinite dilution from water to aqueous hydroxylamine sulfate solutions have been calculated from the relation The transfer partial molar volume values are also shown in Table 3. The cosphere overlap model is always used to interpret the volume shrinking or expansion effects in terms of solute-solute interactions [19–22]. According to the theory, the existence of hydrophilic-hydrophilic and ion-ion interactions will lead to a positive value, while the hydrophobic-hydrophobic interactions lead to a negative value. The for amino acids in aqueous hydroxylamine sulfate solution show that the hydrophilic-hydrophilic and ion-ion interactions are in domination. These interactions may be in existence between zwitterionic groups ( and COO−) in amino acids and ions of hydroxylamine sulfate (NH3OH+ and ). In these mixtures, noncovalent ion pairs will be formed and thus the electrostriction of neighboring water molecules will be released, which result in the increase of the apparent molar volumes of the amino acids in solution. It is further confirmed that when the H atom in glycine is changed to the more hydrophobic –CH3 group in L-alanine, the value is further decreased. On the contrary, when the H group is instead of the more hydrophilic or positively charged guanidino group in L-arginine, much more positive value is observed.
It is interesting to find that the values in the presence of hydroxylamine sulfate are smaller to those in the presence of metal salts. For example, the values of glycine in 0.1 M CdCl2  and 0.1 M ZnCl2  are about 1.83 and 2.77 at 298.15 K, respectively. Similar trends are observed for L-alanine. It reflects that interactions between amino acids and hydroxylamine sulfate may be smaller than those with metal salts. This can be attributed to the fact that these metal ions have more electronic polarizabilities than organic ions, such as hydroxylamine ion. On the other hand, the values in hydroxylamine sulfate are larger than those in some aqueous nonionic organic compounds. For example, the values for glycine and L-alanine in 0.2 M N-Methylformamide  are observed for 0.05 and −0.02, which are smaller than those in this study. However, it needs more experimental or spectroscopic data to draw a conclusion for the comparison of interaction between amino acids with organic, nonorganic, and metal ions.
The hydration numbers () that reflect the electrostriction effect of the charged center of the amino acids on neighboring water can been calculated by using the following method : where and are the molar volumes of electrostricted water and bulk water, respectively. According to Millero et al. , for water molecules taken from the bulk phase to the region near the amino acids, the volumes () are −3.3 cm3·mol−1 at 298.15 K. The electrostriction partial molar volume, , can be expressed as where represents the intrinsic partial molar volume of the amino acids. Millero et al.  calculated the from the molar crystal volume for amino acids by using the following relationship: where 0.7 is the packing density for the molecule in an organic crystal and 0.634 is the packing density for a random packing sphere. The crystal volume can be calculated from the density of the dry solid amino acid .
The hydration numbers of amino acid in aqueous hydroxylamine sulfate solutions at 298.15 K are given in Table 4. The for three amino acids in aqueous hydroxylamine sulfate solutions are positive and according to the order (L-arginine) > (L-alanine) > (glycine). These data are all smaller than those in pure water and are further decreased with the increasing concentration of hydroxylamine sulfate. On the other hand, as the hydrophilic part side chains of amino acids increase, the decrease becomes progressively larger. In the case of L-alanine, the hydration number is only slightly larger than that in pure water. This is reasonable, since the existence of ion-ion and hydrophilic-hydrophilic interaction makes the shrinking water to be more released. It is again demonstrated that the ion-ion and hydrophilic-hydrophilic interactions are dominated between amino acids and hydroxylamine sulfate in aqueous solutions.
|Molality of hydroxylamine sulfate in water.|
The apparent molar volumes of glycine, L-alanine, and L-arginine in aqueous and aqueous hydroxylamine sulfate solutions have been determined at K. The interactions between amino acids and hydroxylamine sulfate have been studied using volumetric properties, including the standard partial molar volumes, , corresponding partial molar volumes of transfer, , and hydration numbers, . The values are positive for glycine, L-alanine, and L-arginine and are increased with the increase in the concentration of hydroxylamine ions. The positive values of for all amino acids in aqueous hydroxylamine sulfate solution suggest that the hydrophilic-hydrophilic and ion-ion interactions predominate. The values show that the –CH3 group in L-alanine weakens the interaction between its hydrophilic or charged group with hydroxylamine sulfate, and the guanidino group in L-arginine enhances the hydrophobic-hydrophilic interactions. The for three amino acids are positive and according to the order L-arginine > L-alanine > glycine.
The authors acknowledge financial support from the National Natural Science Foundation of the People’s Republic of China (Project no. 21006094) and the Science and Technology Planning Project of Zhejiang Province (Project no. 2012C37032).
- M. Sahihi, A. K. Bordbar, and Y. Ghayeb, “Thermodynamic denaturation of β-lactoglobulin in the presence of cetylpyridinium chloride,” The Journal of Chemical Thermodynamics, vol. 42, no. 12, pp. 1423–1428, 2010.
- G. Muhammad, B. Said, J. Romain, S. Pierre, and C. Thomas, “Influence of pH on the dry heat-induced denaturation/aggregation of whey proteins,” Food Chemistry, vol. 129, no. 1, pp. 110–116, 2011.
- L. R. He, C. D. Mu, D. F. Li, and W. Lin, “Revisit the pre-transition of type I collagen denaturation in dilute solution by ultrasensitive differential scanning calorimetry,” Thermochimica Acta, vol. 548, pp. 1–5, 2012.
- E. Y. Chi, S. Krishnan, T. W. Randolph, and J. F. Carpenter, “Physical stability of proteins in aqueous solution: mechanism and driving forces in nonnative protein aggregation,” Pharmaceutical Research, vol. 20, no. 9, pp. 1325–1336, 2003.
- A. Pal and N. Chauhan, “Interactions of amino acids and peptides with the drug pentoxifylline in aqueous solution at various temperatures: a volumetric approach,” The Journal of Chemical Thermodynamics, vol. 54, pp. 288–292, 2012.
- F. Koohyar, A. A. Rostami, M. J. Chaichi, and F. Kiani, “Study on thermodynamic properties for binary systems of water + L-cysteine hydrochloride monohydrate, glycerol, and D-sorbitol at various temperatures,” Journal of Chemistry, vol. 2013, Article ID 601751, 10 pages, 2013.
- M. Singh, M. Pandey, R. K. Yadav, and H. S. Verma, “Thermodynamic studies of molar volume, pair and triplet interactions at increasing side-chain length of α-amino acids in aqueous potassium chloride solutions at different concentration and 310.15 K,” Journal of Molecular Liquids, vol. 135, no. 1-3, pp. 188–191, 2007.
- I. Banik and M. N. Roy, “Study of solute-solvent interaction of some bio-active solutes prevailing in aqueous ascorbic acid solution,” Journal of Molecular Liquids, vol. 169, pp. 8–14, 2012.
- M. N. Roy, R. Dewan, P. K. Roy, and D. Biswas, “Apparent molar volumes and viscosity B-coefficients of carbohydrates in aqueous cetrimonium bromide solutions at (298.15, 308.15, and 318.15) K,” Journal of Chemical and Engineering Data, vol. 55, no. 9, pp. 3617–3624, 2010.
- A. Pal and N. Chauhan, “Thermodynamic (volume and compressibility) and spectral investigations of the glycine, diglycine and triglycine in aqueous α- And β-cyclodextrin solutions at T = 298.15 K,” Journal of Molecular Liquids, vol. 169, pp. 163–172, 2012.
- S. Belica, K. Łudzik, and B. Pałecz, “Partial molar heat capacities at chosen temperatures in the range (298.15 to 328.15) K and partial molar volumes at 298.15 K of N-acetyl-N′-methyl-l-α-amino acid amides in aqueous solution,” Journal of Chemical & Engineering Data, vol. 57, no. 5, pp. 1423–1432, 2012.
- Riyazuddeen and U. Gazal, “Transfer partial molar volumes of L-alanine/ L-glutamine/glycylglycine from water to 0. 512 mol·kg−1aqueous KNO3/K2SO4 solutions at (298.15 to 323.15) K,” Journal of Chemical & Engineering Data, vol. 57, no. 5, pp. 1468–1473, 2012.
- Z. Yan, Q. Zhang, W. Li, and J. Wang, “Effect of temperature on the interactions of glycyl dipeptides with sodium dodecyl sulfate in aqueous solution: a volumetric, conductometric, and fluorescence probe study,” Journal of Chemical and Engineering Data, vol. 55, no. 9, pp. 3560–3566, 2010.
- J. H. Philips, D. M. Brown, and L. Grossman, “The efficiency of induction of mutations by hydroxylamine,” Journal of Molecular Biology, vol. 21, no. 3, pp. 405–419, 1966.
- L.-M. Changchien and G. R. Raven, “The use of hydroxylamline cleavage to product a fragment of ribosomal protein S4 which retains the capacity to specifically bind 16S ribosomal RNA,” Nucleic Acids Research, vol. 14, no. 5, pp. 1957–1966, 1986.
- A. J. Yool and T. L. Schwarz, “Interactions of the H5 pore region and hydroxylamine with N-type inactivation in the Shaker K+ channel,” Biophysical Journal, vol. 68, no. 2 I, pp. 448–458, 1995.
- J. A. Siddique and S. Naqvi, “Volumetric behavior on interactions of α-amino acids with sodium acetate, potassium acetate, and calcium acetate in aqueous solutions,” Journal of Chemical and Engineering Data, vol. 55, no. 8, pp. 2930–2934, 2010.
- M. Kikuchi, M. Sakurai, and K. Nitta, “Partial molar volumes and adiabatic compressibilities of amino acids in dilute aqueous solutions at 5, 15, 25, 35, and 45°C,” Journal of Chemical & Engineering Data, vol. 40, no. 4, pp. 935–942, 1995.
- M. T. Zafarani-Moattar and F. Izadi, “Effect of temperature and concentration of KBr or KNO3 on the volumetric and transport properties of aqueous solutions of tripotassium citrate,” Journal of Chemical and Engineering Data, vol. 56, no. 6, pp. 2818–2829, 2011.
- S. S. Dhondge, C. P. Pandhurnekar, S. Garade, and K. Dadure, “Volumetric and transport behavior of different carbohydrates in aqueous and aqueous urea mixtures at different temperatures,” Journal of Chemical and Engineering Data, vol. 56, no. 8, pp. 3484–3491, 2011.
- S. K. Singh, A. Kundu, and N. Kishore, “Interactions of some amino acids and glycine peptides with aqueous sodium dodecyl sulfate and cetyltrimethylammonium bromide at T = 298.15 K: a volumetric approach,” The Journal of Chemical Thermodynamics, vol. 36, no. 1, pp. 7–16, 2004.
- B. K. Sarkar, A. Choudhury, and B. Sinha, “Excess molar volumes, excess viscosities and ultrasonic speeds of sound of binary mixtures of 1,2-dimethoxyethane with some aromatic liquids at 298.15 K,” Journal of Solution Chemistry, vol. 41, no. 1, pp. 53–74, 2012.
- T. S. Banipal, J. Kaur, P. K. Banipal, and K. Singh, “Study of interactions between amino acids and zinc chloride in aqueous solutions through volumetric measurements at T = (288.15 to 318.15) K,” Journal of Chemical and Engineering Data, vol. 53, no. 8, pp. 1803–1816, 2008.
- T. S. Banipal, J. Kaur, P. K. Banipal, A. K. Sood, and K. Singh, “Volumetric and viscometric studies of some amino acids in aqueous solutions of cadmium chloride at T = (288.15 to 318.15) K and at atmospheric pressure,” Journal of Chemical and Engineering Data, vol. 56, no. 6, pp. 2751–2760, 2011.
- C. Liu, L. Zhou, and L. Ma, “Volumetric properties of amino acids in aqueous N-methylformamide solutions at T = 298.15 K,” Journal of Chemical and Engineering Data, vol. 55, no. 10, pp. 4509–4513, 2010.
- F. J. Millero, A. L. Surdo, and C. Shin, “The apparent molal volumes and adiabatic compressibilities of aqueous amino acids at 25°C,” Journal of Physical Chemistry, vol. 82, no. 7, pp. 784–792, 1978.
- E. Berlin and M. J. Pallansch, “Densities of several proteins and L-amino acids in the dry state,” Journal of Chemical Physics, vol. 72, no. 6, pp. 1887–1889, 1968.
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