16 relations: Acid dissociation constant, Acid strength, Alanine, Ammonia, Aqueous solution, Base (chemistry), Brønsted–Lowry acid–base theory, Chemical equilibrium, Concentration, Diethylamine, Ionization, Methylamine, PH, Proton, Protonation, Self-ionization of water.
An acid dissociation constant, Ka, (also known as acidity constant, or acid-ionization constant) is a quantitative measure of the strength of an acid in solution.
The strength of an acid refers to its ability or tendency to lose a proton (H+).
Alanine (symbol Ala or A) is an α-amino acid that is used in the biosynthesis of proteins.
Ammonia is a compound of nitrogen and hydrogen with the formula NH3.
An aqueous solution is a solution in which the solvent is water.
In chemistry, bases are substances that, in aqueous solution, release hydroxide (OH−) ions, are slippery to the touch, can taste bitter if an alkali, change the color of indicators (e.g., turn red litmus paper blue), react with acids to form salts, promote certain chemical reactions (base catalysis), accept protons from any proton donor, and/or contain completely or partially displaceable OH− ions.
The Brønsted–Lowry theory is an acid–base reaction theory which was proposed independently by Johannes Nicolaus Brønsted and Thomas Martin Lowry in 1923.
In a chemical reaction, chemical equilibrium is the state in which both reactants and products are present in concentrations which have no further tendency to change with time, so that there is no observable change in the properties of the system.
In chemistry, concentration is the abundance of a constituent divided by the total volume of a mixture.
Diethylamine is an organic compound with the formula (CH3CH2)2NH.
Ionization or ionisation, is the process by which an atom or a molecule acquires a negative or positive charge by gaining or losing electrons to form ions, often in conjunction with other chemical changes.
Methylamine is an organic compound with a formula of CH3NH2.
In chemistry, pH is a logarithmic scale used to specify the acidity or basicity of an aqueous solution.
In chemistry, protonation is the addition of a proton (H+) to an atom, molecule, or ion, forming the conjugate acid.
The self-ionization of water (also autoionization of water, and autodissociation of water) is an ionization reaction in pure water or in an aqueous solution, in which a water molecule, H2O, deprotonates (loses the nucleus of one of its hydrogen atoms) to become a hydroxide ion, OH−.