![]() ![]() All the species listed above water are stronger acids, transferring protons to water to some extent when dissolved in an aqueous solution to generate hydronium ions. These species do not undergo acid ionization in water they are not Bronsted-Lowry acids. In the acid column, those species listed below water are weaker acids than water. The listing of conjugate acid–base pairs shown in Figure 14.8 is arranged to show the relative strength of each species as compared with water, whose entries are highlighted in each of the table’s columns. The ionization constants increase from first to last of the listed equations, indicating the relative acid strength increases in the order CH 3CO 2H < HNO 2 < HSO 4 − : HSO 4 − :įigure 14.8 This figure shows strengths of conjugate acid-base pairs relative to the strength of water as the reference substance. To illustrate this idea, three acid ionization equations and K a values are shown below. A table of ionization constants for weak acids is provided in Appendix H. Acids that are partially ionized are called “weak,” and their acid ionization constants may be experimentally measured. An acid is classified as “strong” when it undergoes complete ionization, in which case the concentration of HA is zero and the acid ionization constant is immeasurably large ( K a ≈ ∞). The larger the K a of an acid, the larger the concentration of H 3 O + H 3 O + and A − relative to the concentration of the nonionized acid, HA, in an equilibrium mixture, and the stronger the acid. ![]() ![]() Although water is a reactant in the reaction, it is the solvent as well, so we do not include in the equation. Where the concentrations are those at equilibrium. ![]()
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