it traps the protein onto the paper
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.
The pKa of ethanol is approximately 16.
The pKa of Triethylamine is approximately 10.75.
The pKa of drotaverine is around 8.67.
The pKa value of pyridine is 5.2.
The pKa value of water is approximately 15.7. This value indicates that water is a weak acid. The pKa value of water impacts its chemical properties by determining its ability to donate or accept protons in chemical reactions. This property influences the pH of water and its role as a solvent in various biochemical processes.
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.
The pKa value of azithromycin is around 8.4.
The pKa of bromocresol green is around 4.7.