A Short on Water as an “Amphoteric Weak Electrolyte

When we try to dissolve weak electrolytes in water, the resultant aqueous solution contains molecules of that electrolyte apart from the independent ions. The ratio of ions to molecules is typically represented as 1:10. It behaves like a stubborn material in the process of electrolysis. Poor conduction of electricity takes place in the solution due to the production of fewer ions as compared to the total number of ions formed when strong electrolytes dissociate in water. The process by which ions are released in the aqueous solution is termed ionization in chemistry. Electricity can be conducted by these ions due to their constituent charges (either positive or negative). This charge is present due to deficiency or abundance of electrons in the valence shell. 

Weak acids and weak bases are the two branches of weak electrolytes. Examples of weak electrolytes include hydrofluoric acid, carbonic acid, and acetic acid. These are all weak acids. On the other hand, bases like pyridine and ammonia can be included as popular examples of weak electrolytes.

Water as an amphoteric weak electrolyte

In electrolysis, the oppositely charged ions are needed to be transferred to both ends of the electrode. Otherwise, electricity cannot be conducted efficiently. The pure molecular structure of water does not accommodate enough ions to supply a minimum number of electrons to both cathode and anode. This makes people consider water a poor electrolyte. It is unable to disintegrate into its constituent hydrogen (H+) and hydroxyl (OH–) ions. This is due to strong intermolecular hydrogen bonding which is an intrinsic quality of water. In addition to this, water is also an amphoteric agent. This means that it can behave both as an acid and a base. This is a rare phenomenon for other examples of weak electrolytes. Addition of acid in small amounts to water results in the formation of extra hydrogen cations. Simultaneously the density of hydroxyl ions drops. Hence, in this scenario, the aqueous solution behaves as a base. Likewise, the addition of base provokes the formation of more hydroxyl groups which convert the neutral state of water into acidic nature. Thus it is safe to conclude that water is an amphoteric weak electrolyte. 

Examples of weak electrolytes 

The ionic compounds that do not completely dissociate in an aqueous solution are included in the weak electrolytes list. If we analyze the weak electrolyte formula, we can conclude that both constituent ions, as well as molecules of the electrolyte, are there. 

Examples of weak electrolytes include both weak acids and weak alkalis. Acetic acid is an example of weak acid that fails to dissociate properly in water. Its chemical formula is represented as CH3COOH. Although it is a weak electrolyte, it readily dissolves to produce the final solution. However, the original molecules stay intact in the solution even after the compound is fully dissolved. The ions are not present which indicates that there is no chance of conducting an electric charge. The molecular structures in the aqueous solution of acetic acid are named ethanoates. A few portions of the solution are composed of positively charged hydronium ions. 

Chemical reaction: CH3COOH (aq.) + H20 (aq.) ⇔ H3O+ + CH3COO– (Ethanoate) 

The weak electrolytes list is also composed of compounds like ammonia, phosphoric acid, and hydrofluoric acid. 

Significance of weak electrolytes 

• The molecules that are formed after the dissociation of weak electrolytes contain primary ions. For example, hydrogen carbonate includes hydrogen and carbonate ions respectively. 

HCO3– = H+ + CO3–. This explanation further helps us to understand complex physiological processes involving electrolytes. 

• The study of electrolytic events inside the cell fluids is essential to understanding the functionality of human muscles and the nervous system. It is also considered for other multicellular organisms. The specialized band 3 and glycophorin proteins within the plasma membrane are made of ion channels. These channels facilitate the transmission of certain weak electrolytes within the human body. 
• Electrolytes are utilized to rehydrate the human body in excess heat. Such drinks include sodium and potassium. The simplest way to prepare an electrolytic solution that is fit for oral consumption is by mixing sugar and salt with water. 

Conclusion 

Electrolytes are not only produced in scientific laboratories to conduct research. Electrolytes are classified into strong and weak alternatives based on their capacity to dissociate into ions. They are abundantly present in nature. One can find such compounds in fruits, vegetables, and even in human blood. The content of potassium and sodium ions in the blood is tested to recommend vital diagnostic therapy.