Cationic Amino Acid Identity and Net Charge Influence Condensate Properties in E. coli
Aaron K Kidane1,2, Jacob R Rosenfeld1, Jake D Johnston2,3
1Department of Chemical Engineering, Columbia University, New York, New York 10027, United States.
Biomacromolecules
|September 3, 2025
Summary
The identity of specific amino acids, like arginine, significantly impacts how biomolecular condensates form and behave. This primary sequence information is crucial for understanding condensate dynamics beyond just charge and disorder.
Area of Science:
- Biochemistry
- Molecular Biology
- Cell Biology
Background:
- Biomolecular condensates (BMCs) are essential for organizing cellular functions, including RNA metabolism and stress responses.
- The precise mechanisms by which primary amino acid sequences influence BMC formation and dynamics are not fully understood.
Purpose of the Study:
- To investigate the role of cationic amino acid identity in shaping the properties of protein-RNA coacervates.
- To determine how arginine, compared to other cationic amino acids, affects condensate formation and dynamics.
Main Methods:
- Utilized engineered recombinant proteins to create protein-RNA coacervates.
- Assessed phase boundaries, salt resistance, condensate formation in vivo (E. coli), and protein mobility in vitro and in cells.
Main Results:
- Phase boundaries of coacervates are influenced by both amino acid identity and protein net charge.
- Arginine promotes higher salt resistance and enhanced condensate formation compared to other cationic amino acids with identical charge at physiological pH.
- Arginine incorporation leads to reduced protein mobility within condensates, both in vitro and in cellular environments.
Conclusions:
- Beyond electrostatics and intrinsic disorder, the primary amino acid sequence and side chain composition are critical determinants of biomolecular condensate dynamics.
- Arginine's specific properties play a significant role in modulating the formation, stability, and internal dynamics of protein-RNA coacervates.
Related Concept Videos
Amino acids
91.3K
Amino acids are the monomers that comprise proteins. Each amino acid has the same fundamental structure, which consists of a central carbon atom, or the alpha (α) carbon, bonded to an amino group (NH2), a carboxyl group (COOH), and to a hydrogen atom. Every amino acid also has another atom or group of atoms bonded to the central atom known as the R group. There are 20 common amino acids present in proteins, each with a different R group. Variation in the amino acid sequence is responsible...
91.3K
Polyprotic Acids
29.5K
Acids are classified by the number of protons per molecule that they can give up in a reaction. Acids such as HCl, HNO3, and HCN that contain one ionizable hydrogen atom in each molecule are called monoprotic acids. Their reactions with water are:
29.5K
Basicity of Aliphatic Amines
6.2K
Amines can behave as Brønsted–Lowry bases by accepting a proton from the acid to form corresponding conjugate acids. Due to a lone pair of nonbonding electrons, aliphatic amines can also act as Lewis bases by forming a covalent bond with an electrophile.
To measure the basicity of amines, two conventions are generally used. The first defines Kb as the basicity constant for the deprotonation reaction of water by the amine, as presented in Figure 1. Conventionally, lower Kb indicates...
To measure the basicity of amines, two conventions are generally used. The first defines Kb as the basicity constant for the deprotonation reaction of water by the amine, as presented in Figure 1. Conventionally, lower Kb indicates...
6.2K
Extraction: Effects of pH
710
Consider a neutral form of an amine, B, with a partition coefficient, K, in a liquid mixture containing organic and aqueous phases. The pH of the aqueous phase affects the charge on acidic and basic solutes, and the charged form is usually more soluble in the aqueous phase. Suppose the conjugate acid form of the amine is soluble only in the aqueous phase while the base form is soluble in both phases. Then the distribution coefficient, D, can be given as the ratio of amine concentration in the...
710
Common Ion Effect
42.2K
Compared with pure water, the solubility of an ionic compound is less in aqueous solutions containing a common ion (one also produced by dissolution of the ionic compound). This is an example of a phenomenon known as the common ion effect, which is a consequence of the law of mass action that may be explained using Le Châtelier’s principle. Consider the dissolution of silver iodide:
42.2K
Basicity of Heterocyclic Aromatic Amines
6.3K
Heterocyclic amines, where the N atom is a part of an alicyclic system, are similar in basicity to alkylamines. Interestingly, the heterocyclic amine having a nitrogen atom as part of an aromatic ring has much less basicity than its corresponding alicyclic counterpart. For this reason, as presented in Figure 1, piperidine (pKb = 2.8) is significantly more basic than pyridine (pKb = 8.8).
6.3K


