All you need to do to get Ka is to take the antilog of the pKa.
pKa = -log Ka and thus Ka = 10^-pKaKa = antilog pKaKa = 7.76x10^-6
pKa = -log KapKa = -log 5.4x10^-10pKa = 9.27
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.
HA ==> H+ + A-Ka = [H+][A-][HA] and from pH = 2.31, calculated [H+] = 4.89x10^-3 M Ka = (4.89x10^-3)(4.89x10^-3)/0.012 Ka = 1.99x10^-3 pKa = 2.70
As with any acid, that depends entirely on its concentration. The greater the concentration (until saturation) the lower the pH. Lactic acid is a "middle of the road" weak acid; all in equal concentrations, lactic acid is stronger than citric, weaker than acetic, and about the same as formic.
pKa = -log Ka and thus Ka = 10^-pKaKa = antilog pKaKa = 7.76x10^-6
The Ka of hydrogen iodide is approx. 1010. The pKa of hydrogen iodide is approx. - 9.
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.
pKa = -log KapKa = -log 5.4x10^-10pKa = 9.27
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.
At half titration pH=pKa (you need the pH from the graph of your titration, y axis) ph = pKa + log (base/acid) 10^-pKa = Ka Kw=Ka*Kb Kb=Kw/Ka Ka = Kw/Kb
The KB value is listed below: pKa + pKb - 14 pKa = -log10 (Ka), Ka of acetic acid = 1.8*10^-5 pKa = 4.74, pkb = 9.255 9.255 = -log10(Kb), Kb = 5.56*10^-10
The pKa of sulfonic acid is < 0
pKa < 0.0 Ka > 1.0
The pKa of the fluorosulfuric acid is -10; HSO3F is a very strong acid, a so-called superacid. Ka is the dissociation constant; pKa is the decimal logarithm of Ka.
PKa = -log Ka so if you multiply across by -1 and then taking the antilog you can get Ka Ka.Kb = Kw where Kw = 1.0 x 10^14 PKa + PKb = PKw = 14 that should give you a start.
Its an equation you can use to find the pH of a solution. it is.... --- pH = pKa + log (Base/Acid) --- these may help too Ka = 10^-pKa Kw = Ka*Kb