Want this question answered?
Be notified when an answer is posted
The pKa of drotaverine is around 8.67.
You can calculate the pKa value by using the Henderson-Hasselbalch equation: pH = pKa + log([A-]/[HA]), where [A-] is the concentration of the conjugate base and [HA] is the concentration of the acid. Rearranging the equation, you can solve for pKa by taking the antilog of both sides after isolating pKa.
pKa (dissociation constant) is variable with temperature.
The pKa value of azithromycin is around 8.4.
pKa = -log KapKa = -log 5.4x10^-10pKa = 9.27
Yes, I think some do.
The pKa of diisopropylamine is around 10-11.
The pKa of bromoacetic acid is approximately 2.64.
The pKa value of Doxofylline is approximately 4.22.
yes it can only in certain condition
The pKa of Triethylamine is approximately 10.75.
The pKa of ethanol is approximately 16.
The pKa of drotaverine is around 8.67.
To calculate pKa, you can use the Henderson-Hasselbalch equation: pKa = pH + log([A−]/[HA]), where [A−] is the concentration of the conjugate base and [HA] is the concentration of the acid. Alternatively, you can look up the pKa value in a table or use a chemical database.
You can calculate the pKa value by using the Henderson-Hasselbalch equation: pH = pKa + log([A-]/[HA]), where [A-] is the concentration of the conjugate base and [HA] is the concentration of the acid. Rearranging the equation, you can solve for pKa by taking the antilog of both sides after isolating pKa.
pKa (dissociation constant) is variable with temperature.
The pKa value of Acebrophylline is approximately 1.8.