CHEM 1210 Lecture Notes - Lecture 8: Equilibrium Constant, Ph
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Acid-base equilibrium constant, ka: used to determine the composition of an acid- reaction at equilibrium. When a weak acid, ha, dissolves in water. The equilibrium constant expression, ka, for its ionization is: Because ka for weak acids are numbers with negative exponents, we commonl express acid strengths as pka where: pka = -log(ka) The value of pka for acetic acid is: 4. 75. The stronger the acid, the larger its ka , but the smaller its pka (inverse relationship) Pure water contains a very small number of h3o+ ions and oh- ions. Formed by proton transfer from one water molecule (the proton donor) to another (the proton acceptor) The equilibrium constant for the ionization of water, kw, is: n acid-base ommonly onship) nother (the. If we add 0. 010 mol of hcl to 1. 00 l of pure water, it reacts completely with water t give 0. 010 mol of h3o+ In this solution, [h3o+] is 0. 010 m or 1. 0e-2.
