Does Henderson Hasselbalch equation work for bases?

The Henderson-Hasselbalch equation is valid when it contains equilibrium concentrations of an acid and a conjugate base. In the case of solutions containing not-so-weak acids (or not-so-weak bases) equilibrium concentrations can be far from those predicted by the neutralization stoichiometry.

How do you calculate pH using Henderson Hasselbalch equation?

Henderson-Hasselbalch EquationHenderson-Hasselbalch Equation. The Henderson-Hasselbalch equation relates pH, pKa, and molar concentration (concentration in units of moles per liter): The equation can be rewritten to solve for pOH: [ B ] = molar concentration of a weak base (M) pH = pK_a + log ([A^–]/[HA]) pH = -log (1.8 x 10^–5) + log (2.5)

What is pKa in Henderson Hasselbalch equation?

The pKa is the pH value at which a chemical species will accept or donate a proton. The lower the pKa, the stronger the acid and the greater the ability to donate a proton in aqueous solution. The Henderson-Hasselbalch equation relates pKa and pH.

Is pKa equal to pH?

Remember that when the pH is equal to the pKa value, the proportion of the conjugate base and conjugate acid are equal to each other. As the pH increases, the proportion of conjugate base increases and predominates.

What is the use of Henderson Hasselbalch equation?

can be used to estimate the pH of a buffer solution. The numerical value of the acid dissociation constant, K_a, of the acid is known or assumed.

What is pKa formula?

pKa is defined as -log10 K_a where K_a = [H⁺][A^–] / [HA]. From these expressions it is possible to derive the Henderson-Hasselbalch equation which is. pKa = pH + log [HA] / [A^–] This tells us that when the pH = pK_a then log [HA] / [A^–] = 0 therefore [HA] = [A^–] ie equal amounts of the two forms.

How do I calculate pH?

To calculate the pH of an aqueous solution you need to know the concentration of the hydronium ion in moles per liter (molarity). The pH is then calculated using the expression: pH = – log [H₃O⁺].

What is the difference between KA and pKa?

Ka is the acid dissociation constant. pKa is simply the -log of this constant. Similarly, Kb is the base dissociation constant, while pKb is the -log of the constant. The acid and base dissociation constants are usually expressed in terms of moles per liter (mol/L).

Is pKa the equivalence point?

Therefore, at the half-equivalence point, the pH is equal to the pKa. A plot of the titration curve allows the equivalence point to be determined. At exactly one- half the volume of the equivalence point, the measured pH is equal to pKa as illustrated in Figure 3.

Why buffer capacity is greatest pH pKa?

As expected buffer exhibits the highest resistance to acid and base addition for the equimolar solution (when pH=pKa). From the plot it is also obvious that buffer capacity has reasonably high values only for pH close to pKa value. The further from the optimal value, the lower buffer capacity of the solution.

What happens if pKa is lower than pH?

If the pH is lower than the pKa, then the compound will be protonated. If the pH is higher than the pKa, then the compound will be deprotonated. Acids are neutral when protonated and negatively charged (ionized) when deprotonated. Bases are neutral when deprotonated and positively charged (ionized) when protonated.

What is the pKa of Naoh?

Sodium hydroxide is the conjugate base of H2O (pKa 15.7). That’s a difference of about 24 pKa units – and since each pKa unit represents one order of magnitude, this reaction is favorable with an equilibrium constant of about 10 to the power of 24.