BackDependence of Solubility on pH definitions
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1/15BackSkip to main contentBackActivity Coefficient
A factor that corrects for non-ideal behavior of ions in solution, influenced by ionic strength and ion charge. Ionic Strength
A measure of the total concentration of ions in solution, weighted by the square of each ion's charge. Extended Debye-Hückel Equation
A formula relating activity coefficient to ionic strength, ion charge, and ion size parameter for accurate predictions. Size Parameter
A value, often in nanometers, representing the effective diameter of an ion in solution. Davies Equation
An empirical formula for estimating activity coefficients, especially for monovalent ions when ion size is unknown. Cation
A positively charged ion, which can be acidic, neutral, or basic depending on its charge and group. Anion
A negatively charged ion, classified as basic or neutral based on the acid formed when combined with H+. Acidic Salt
A compound that increases solution acidity due to the presence of an acidic cation. Basic Anion
A negatively charged ion that forms a weak acid upon reaction with H+, increasing solubility in acidic conditions. Neutral Anion
A negatively charged ion that forms a strong acid with H+, resulting in negligible basicity. Amphoteric Species
An ion or molecule capable of acting as either an acid or a base, with solubility affected by pH. Le Chatelier's Principle
A rule stating that a system at equilibrium will adjust to counteract changes, affecting solubility with pH shifts. Transition Metal
A metal ion, typically requiring a charge of +2 or higher to exhibit acidic behavior in solution. Main Group Metal
A metal ion from groups 1A to 3A, needing a charge of +3 or higher to be considered acidic. Monovalent Ion
An ion with a single positive or negative charge, such as sodium or chloride, often used with the Davies equation.
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