pKa=2.86
According to me, The pKa of chlorosulfonic acid is approximately -1.6.
H2SO3 is a weak acid, pKa=1.8, HCl is strong, pKa<<0
Acetic acid (from vinegar) is stronger, though mono-basic. pKa = 4.77 Carbonic acid (H2CO3) is di-basic. pKa,1 = 6.36 and pKa,2 = 10.25
The pka of a protonated ether (the conjugate acid) is about -3.5
pKa=2.86
Salicylic acid has a pKa of 1.96 and acetylsalicylic acid (Aspirin) has a pKa of 3.48. Therefore salicylic acid is the stronger acid.
According to me, The pKa of chlorosulfonic acid is approximately -1.6.
It refers to the acidity of the fatty acid (which make up the oils). Every fatty acid is composed of a non-polar long chain of hydrocarbons (carbon and hydrogen) and a polar head made up of Carboxylic ACID. Every acid has something called pKa which determines the acidity of that acid.The bigger the pKa (e.g. 25), the weaker the acid.The smaller ther pKa (e.g. 2), the stronger the acid.
H2SO3 is a weak acid, pKa=1.8, HCl is strong, pKa<<0
The pka of a protonated ether (the conjugate acid) is about -3.5
Acetic acid (from vinegar) is stronger, though mono-basic. pKa = 4.77 Carbonic acid (H2CO3) is di-basic. pKa,1 = 6.36 and pKa,2 = 10.25
pKa = -log KapKa = -log 5.4x10^-10pKa = 9.27
There are two answers: bicarbonate has two pKa's - because bicarbonate can gain a proton to become carbonic acid or lose a proton to become carbonate. Two reactions; two pKa's. The pKa for bicarbonate carbonic acid reaction is 6.4 The pKa for bicarbonate carbonate reaction is 10.3 Both pKa's are temperature sensitive.
B.G. pKa solutions In solutions of equal concentration: pH= pKa Threrfore pKa 4.68.
2.66
The conjugate acid is Hydrogen (H2), the pKa of which is 35.