- An electrolyte is a substance that when dissolved in a solvent, such as water, forms ions that conduct electric current. - Electrolytes are typically ionic compounds, such as salts, acids, or bases, that dissociate into positive and negative ions in a solution. - The ability of a substance to form ions and conduct electricity is determined by its chemical composition and structure. - Ionic compounds, such as sodium chloride (NaCl) or potassium nitrate (KNO3), readily dissociate into positive and negative ions in water. - Acids, such as hydrochloric acid (HCl) or sulfuric acid (H2SO4), release hydrogen ions (H+) in water, making them electrolytes. - Bases, like sodium hydroxide (NaOH) or potassium hydroxide (KOH), release hydroxide ions (OH-) in water and are also considered electrolytes. - Some compounds, known as weak electrolytes, only partially dissociate into ions in solution. Examples include weak acids like acetic acid (CH3COOH) or weak bases like ammonium hydroxide (NH4OH). - The conductivity of electrolytes depends on factors such as concentration, temperature, and viscosity of the solvent. - Electrolytes are essential for various biological processes, such as nerve conduction, muscle contraction, and maintaining body fluid balance. - Sources: 1. Giuntini, F. and Tonelli, D., 2018. Electrolytes. StatPearls Publishing. 2. Levine, I.N., 1978. Physical chemistry, chapter 13: Solutions of nonelectrolytes. McGraw-Hill. 3. Huheey, J.E., Keiter, E.A. and Keiter, R.L., 1977. Inorganic chemistry: principles of structure and reactivity. Harper & Row.
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