Final answer:
The calculation for equilibrium constants involves determining the concentrations of the reactants and products in a chemical reaction at equilibrium and substituting these into the equilibrium expression for Ke, Ka, or Kb, depending on the context of the reaction.
Step-by-step explanation:
The Keilhauer-Betke method is not explicitly stated in the information provided, but based on the context, it appears to be related to the equilibrium constant (Ke or K) calculation in chemical reactions. The equilibrium constant is a vital concept in chemistry that quantifies the relative concentrations of reactants and products in a chemical reaction at equilibrium.
Calculating equilibrium constants typically involves setting up an ICE (Initial, Change, Equilibrium) table, determining the concentrations of all species at equilibrium, and substituting these values into the equilibrium expression. For instance, if we have an equilibrium constant Ke, and know the concentrations of products [PC13] and [PC15], and the reactant [C1₂], the equation would look like Ke = [PC13][PC15]/[C1₂]. Plugging in the values (0.135)(0.135)/0.87 would provide us with the numerical value of Ke.
If we are interested in the equilibrium concerning acids and bases, such as the base ionization of acetate ion, we would calculate the Kb using the formula Kb = [CH3CO2H][OH-]/[CH3CO2-], substituting in the values for each species. Similarly, for the acid dissociation constant or Ka, the concentration of the acid (H+) and its conjugate base at equilibrium would be used in the calculation.