Kohlrausch’s law, also known as Kohlrausch’s displacement law, states that the molar conductivity of an electrolyte can be expressed as the sum of the contributions of its individual ions. In other words, the total conductivity of an electrolyte solution is equal to the sum of the conductivities of the cations and anions present in the…
Electrolytic conductance refers to the ability of an electrolyte solution to conduct electric current. Electrolytes are substances that dissociate into ions when they dissolve in water, and these ions can move freely through the solution and carry electric charge. The conductance of an electrolyte solution depends on several factors, including the concentration of ions in…
Faraday’s laws of electrolysis are two fundamental laws that describe the quantitative relationship between the amount of electric charge passed through an electrolytic cell and the amount of chemical change that occurs during electrolysis. These laws were developed by the British scientist Michael Faraday in the early 19th century. Faraday’s First Law of Electrolysis states…
The Nernst equation is an important formula in electrochemistry that relates the concentration of ions in a solution to the potential difference across a membrane or electrode. The equation is named after German chemist Walther Nernst, who formulated it in 1889. The Nernst equation is given as: E = E° – (RT/nF) * ln(Q) where:…
Standard electrode potentials (also known as standard reduction potentials) are a measure of the tendency of a chemical species to undergo reduction or oxidation under standard conditions. These potentials are reported relative to the standard hydrogen electrode (SHE), which is assigned a potential of 0.00 volts. Standard electrode potentials are typically represented using the notation…
Electrochemical cells are devices that convert chemical energy into electrical energy or vice versa. They involve a redox (reduction-oxidation) reaction, which occurs at the interface between two electrodes immersed in an electrolyte solution. In an electrochemical cell, there are two half-cells, each consisting of an electrode and an electrolyte. The half-cell where oxidation occurs is…
Hydrolysis of salts is a chemical reaction in which a salt reacts with water to produce an acidic or basic solution. The nature of the salt and the pH of the resulting solution depend on the cation and anion present in the salt. If the cation is derived from a strong base and the anion…
pH is a measure of the acidity or basicity of a solution. It is defined as the negative logarithm of the hydrogen ion concentration in a solution. pH ranges from 0 to 14, with 7 being neutral, lower pH values indicating acidity, and higher pH values indicating basicity. A pH of 7 is considered neutral…
The common ion effect is a phenomenon in which the solubility of a slightly soluble salt is decreased by the presence of a common ion in the solution. This effect is due to the principle of Le Chatelier’s principle, which states that a system at equilibrium will shift to counteract any stress placed upon it.…
Solubility product is a measure of the maximum amount of a solute that can dissolve in a solvent at a particular temperature, and is represented by the symbol Ksp. It is the equilibrium constant for the dissolution of a sparingly soluble salt in water, and is defined as the product of the concentrations of the…
