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Thermal stability of the C H 2 domain for an IgG1 monoclonal antibody and its aggregation kinetics were systematically studied at pH 4.8, below its pI of 8.8 in individual solutions of arginine salts with acetate, glutamate (Glu - ), chloride, and sulfate as the anion, in comparison to sodium chloride and sodium sulfate. Thermal unfolding temperature, T m , an indicator of thermal stability, was measured by both differential scanning calorimetry (DSC) and differential scanning fluorimetry (DSF). The aggregation kinetics was determined by assessing reversibility for the C H 2 domain in the DSC repetitive scans and then cross-examined by the isothermal aggregation study measured by size exclusion chromatography. The effect of Arg + on the thermal stability and aggregation kinetics of the antibody is shown to be strongly anion-dependent: both ArgAceate and ArgGlu improve the stability, while both Arg 2 SO 4 and ArgCl decrease it. Furthermore, the addition of ArgCl and Arg 2 SO 4 accelerates the aggregation kinetic, but to a lesser extent than the respective Na + salt, suggesting that Arg + binds to the antibody more strongly than Na + . However, the binding of Arg + did not lead to more destabilization of the C H 2 domain by the Arg + salts at low concentrations, comparing to the respective Na + salt. This finding indicates that Arg + prefers the protein surface, rather than the exposed backbone upon unfolding. Furthermore, the change in the ranking for affecting the thermal stability and aggregation kinetics as the salt concentration increases implies the presence of other multiple mechanisms, e.g., cluster formation through the homoion pairing between Arg + molecules and their preferential exclusion from the protein surface, and heteroion pairing between Arg + and SO 4 2- .

The thermal unfolding and subsequent aggregation of the unglycosylated Fc fragment of a human IgG1 antibody (Fc) were studied in the salt solutions of Na(2)SO(4), KF, KCl and KSCN at pH 4.8 and 7.2 below and at its pI of 7.2, respectively, using differential scanning calorimetry (DSC), far ultraviolet circular dichroism (far-UV CD), size exclusion chromatography (SE-HPLC) and light scattering. First, our experimental results demonstrated that the thermal unfolding of the C(H)2 domain of the Fc was sufficient to induce aggregation. Second, at both pH conditions, the anions (except F(-)) destabilized the C(H)2 domain where the effectiveness of SO(4)(2-) > SCN(-) > Cl(-) > F(-) was more apparent at pH 4.8. In addition, the thermal stability of the C(H)2 domain was less sensitive to the change in salt concentration at pH 7.2 than at pH 4.8. Third, at pH 4.8 when the Fc had a net positive charge, the anions accelerated the aggregation reaction with SO(4)(2-) > SCN(-) > Cl(-) > F(-) in effectiveness. But these anions slowed down the aggregation kinetics at pH 7.2 with similar effectiveness when the Fc was net charge neutral. We hypothesize that the effectiveness of the anion on destabilizing the C(H)2 domain could be attributed to its ability to perturb the free energy for both of the native and unfolded states. The effect of the anions on the kinetics of the aggregation reaction could be interpreted based on the modulation of the electrostatic protein-protein interactions by the anions.

The protein denaturing properties of urea are well-known and still the subject of debate. It has been noted that in some cases where urea concentrations are relatively low stabilization is afforded against aggregation. An explanation for this unusual effect has seemingly remained elusive. Evidence is offered to propose urea stabilization is related to its influence on the solvation property of the protein molecules when in contact with an unfolded hydrophobic surface that tends to increase the entropy of the local aqueous solvent. This property of urea is expected to lower the entropic driving force of unfolded-mediated aggregation despite the increase in enthalpy. The data presented from toluene transfer experiments into 2 M urea + 0.1 M sodium phosphate solutions showed that the solvation free energy change was negative up to ∼75 °C. The associated ΔΔH was positive, leading to the conclusion that entropy drives the solvation process within the temperature domain from ∼20° to 75 °C. Using thermodynamic parameters from the toluene solvation experiments, it was possible to accurately determine the T(m) shift of recombinant human interleukin-1 receptor type II (rhuIL-1R(II)). Heating experiments above the apparent T(m) in the same urea/phosphate solution support the thesis that urea inhibits the entropy-driven aggregation process of rhuIL-1R(II), adding yet another molecule to the list of low urea concentration stabilized molecules.

The role of thermal unfolding as it pertains to thermodynamic properties of proteins and their stability has been the subject of study for more than 50 years. Moreover, exactly how the unfolding properties of a given protein system may influence the kinetics of aggregation has not been fully characterized. In the study of recombinant human Interleukin-1 receptor type II (rhuIL-1R(II)) aggregation, data obtained from size exclusion chromatography and differential scanning calorimetry (DSC) were used to model the thermodynamic and kinetic properties of irreversible denaturation. A break from linearity in the initial aggregation rates as a function of 1/T was observed in the vicinity of the melting transition temperature (T(m) approximately 53.5 degrees C), suggesting significant involvement of protein unfolding in the reaction pathway. A scan-rate dependence in the DSC experiment testifies to the nonequilibrium influences of the aggregation process. A mechanistic model was developed to extract meaningful thermodynamic and kinetic parameters from an irreversibly denatured process. The model was used to simulate how unfolding properties could be used to predict aggregation rates at different temperatures above and below the T(m) and to account for concentration dependence of reaction rates. The model was shown to uniquely identify the thermodynamic parameters DeltaC(P) (1.3 +/- 0.7 kcal/mol-K), DeltaH(m) (74.3 +/- 6.8 kcal/mol), and T(m) with reasonable variances.