pKa to pKb Conversion Table

Additional Information

K_a, also known as the acid dissociation constant, quantifies the strength of an acid by measuring the extent to which it dissociates or ionizes in water. A higher K_a value indicates a stronger acid that readily donates protons, while a lower K_a value corresponds to a weaker acid with limited dissociation. K_b, on the other hand, quantifies the strength of a base by measuring the extent to which it dissociates or accepts protons (H⁺) in water. A higher K_b value indicates a stronger base that readily accepts protons, while a lower K_b value corresponds to a weaker base with limited dissociation. The product of these two values is equal to K_w, or the ionization constant of water (K_a * K_b = K_w). K_w represents the equilibrium constant for the self-ionization of water, where water molecules react to form hydronium ions (H3O⁺) and hydroxide ions (OH^-), and is equal to 1.0e^-14 in neutral water at 25 degrees Celsius. When given either the K_a or K_b value of an acid or base, one can calculate the other by dividing it by 1.0e^-14, assuming a neutral environment at 25 degrees Celsius.

pK_a and pK_b provide logarithmic representations of their counterparts for acid and base strengths (K_a and K_b), and allow for a more straightforward comparison of the relative strengths of acids and bases: smaller pK_a values indicate stronger acids, while smaller pK_b values indicate stronger bases. pK_a and pK_b are also useful in predicting the behavior of acids and bases in chemical reactions, determining the pH of a solution, and understanding the position of equilibrium in an acid-base reaction. To determine the value for either pK_a or pK_b, one can use the following formulas: pK_a = -log₁₀(K_a), pK_b = -log₁₀(K_b), and pK_a + pK_b = 14.00 (assuming a neutral environment at 25 degrees Celsius).