The pKa of H3O+ is approximately -1.74. This indicates that H3O+ is a strong acid as it readily donates a proton in aqueous solutions.
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 Triethylamine is approximately 10.75.
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.
hydronium, OH3+, is acidic as hydroxide is basic
The pKa for HCO3- ----> CO3-2 + H+ is 10.33 I assume you would have a reaction such as K+ HCO3- + H2O ------> K+CO3-2 + H3O+ In which the potassium acts as a neutral ion.
The pKa of diisopropylamine is around 10-11.
The pKa of bromoacetic acid is approximately 2.64.
No, boric acid is NOT tribasic, although its formula suggests so with formula H3BO3.It is a mono-basic, weak acid:H3BO3 + H2O
The pKa value of Doxofylline is approximately 4.22.
The chemical formula of hydronium is H3O +.
The pKa of Triethylamine is approximately 10.75.
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.
pKa (dissociation constant) is variable with temperature.
h3o is a carbonates
The pKa of sulfonic acid is < 0