Henderson-Hasselbalch equation a formula for calculating the pH of a buffer solution such as blood plasma, pH = pKa + log [BA/HA]; [HA] is the concentration of a free weak acid; [BA] the concentration of the ionized form of this acid; pKa the acid dissociation constant, a measure of...
Write a balanced net ionic equation to show why the solubility of Pb(OH)_2(s) increases in the presence of a strong acid and calculate the equilibrium constant for the reaction of this sparingly solub Write a balanced equation that describes the follo...
Dissociation constantsError calculationActivity coefficient of protonEquivalence volumesIt is shown that acid–base titration can be treated, in general, as an additive property. This is based on the fact that the average charge on the undissociated and dissociated solute species at equilibrium is an...
The Henderson-Hasselbalch equation solves for the pH of a solution using pKa, which is the negative log of the acid dissociation constant. This value is an equilibrium constant for the reaction of {eq}HA \rightleftharpoons A^- + H^+ {/eq}, which is a measure of how strong an acid ...
The meaning of HENDERSON-HASSELBALCH EQUATION is an equation that equates the pH of a buffered solution (as the blood) to the sum of the cologarithm (p) of the dissociation constant (K) of the acid in the buffer and the logarithm of the ratio of the conc
TheHenderson Hasselbalch equationisan approximate equation that shows the relationship between thepHor pOH of asolutionand the pKaor pKband the ratio of theconcentrationsof the dissociated chemical species. In order to use the equation, the acid dissociation constant must be known. ...
the formula for calculating the pH of a buffer solution, which states that: where pK is the dissociation constant of an acid. The variable term is really a ratio of concentration values and can be taken as being proportional to the amount of acid and base added in the buffer. For exampl...
The discussion centers on the titration of a weak acid with sodium hydroxide. Approximate pH values obtained from the Henderson-Hasselbalch equation are compared with exact hydrogen ion concentrations and the percentage errors are displayed as a function of the acid dissociation constant and buffer ...
Since the Henderson-Hasselbalch equation does not consider the self-dissociation undergone by water, it fails to offer accurate pH values for extremely dilute buffer solutions. Solved Example A buffer solution is made from 0.4M CH3COOH and 0.6M CH3COO–. If the acid dissociation constant of CH3CO...
Calculate the pHof a buffer solution made from 0.20 M HC2H3O2and 0.50 M C2H3O2-that has an acid dissociation constant for HC2H3O2of 1.8 x 10-5. This is a straightforward example because all of the terms are given. Solve this problem by plugging the values into the Henderson-Hasselbalch eq...