3.9 x 10^-6
The above value could be true. However, it also depends on the concentration of the acid and base at that given experiment. In a general sense, it would have a Ka value of somewhere in the 10^-6 range.
P.S. Correct me if I am wrong by any given chance
The pKa of salicylic acid is 2.97, and so the Ka = 1.07 x 10-3.
In my chemistry lab book, it states it is 1.1 X10^-3
the Ka of salicylic acid is 1.07 x 10-3 the pKa of salicylic acid is 2.97
I don't think it has a Ka because its not an acid
Ka=3.3 x 10-7
Ka for Nicotinic Acid = 1.4 x 10-5
Log K = -0.18 according to Stafansson et al
The strength of an acid or the measure of its tendency to release proton ions (H+) can be indicated from its dissociation constant which is called Ka. The acid dissociation constant, pKa , is the negative logarithm of dissociation constant (Ka).
Ka for benzoic acid is 6.46 x 10-5.
The equation is acid + water equalizes into hydronium and conjugate base, and Ka (acid dissociation constant) is products divided by reactants. If the Acid = (H+)(base)/Ka, then the acid concentration is (H+)(H+)/Ka, or (0.0001)(0.0001)/0.0000001, which equals 1M.
An acid dissociation constant, Ka, (also known as acidity constant, or acid-ionization constant) is a quantitative measure of the strength of an acid in solution. It is the equilibrium constant for a chemical reaction known as dissociation in the context of acid-base reactions. The equilibrium can be written symbolically as: HA A− + H+,
A larger Ka indicates that the acid will more readily react as the molecular bonds are relatively weak. The Ka is known as the dissociation constant.
The strength of an acid or the measure of its tendency to release proton ions (H+) can be indicated from its dissociation constant which is called Ka. The acid dissociation constant, pKa , is the negative logarithm of dissociation constant (Ka).
Acid dissociation constant
acid dissociation constant
Ka for benzoic acid is 6.46 x 10-5.
H2CO3---------- 2 H+ + (CO3)2-
The equation is acid + water equalizes into hydronium and conjugate base, and Ka (acid dissociation constant) is products divided by reactants. If the Acid = (H+)(base)/Ka, then the acid concentration is (H+)(H+)/Ka, or (0.0001)(0.0001)/0.0000001, which equals 1M.
An acid dissociation constant, Ka, (also known as acidity constant, or acid-ionization constant) is a quantitative measure of the strength of an acid in solution. It is the equilibrium constant for a chemical reaction known as dissociation in the context of acid-base reactions. The equilibrium can be written symbolically as: HA A− + H+,
A larger Ka indicates that the acid will more readily react as the molecular bonds are relatively weak. The Ka is known as the dissociation constant.
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.
Salicylic acid is also known as 2-Hydroxybenzoic acid. The literature Ka value is 2x10 to the negative 14th power. Which makes salicylic acid a somewhat strong acid.
dissociation of acid in water: A + H2O <-> A- + H3O+ with dissociation constant Ka = [A-][H3O+]/[A][H2O] = [A-][H3O+]/[A]. dissociation of base in water: B + H2O <-> HB+ + OH- with dissociation constant Kb = [HB+][OH-]/[B][H2O] = [HB+][OH-]/[B] dissociation of water in itself: 2H2O <-> H3O+ + OH- with dissociation constant Kw = [H3O+][OH-]/[H2O]^2 = [H3O+][OH-] where [H2O] has been ommitted because it is a pure liquid. substituting relations for Ka and Kb into Kw gives: Kw = [H3O+][OH-] = (Ka[A]/[A-])(Kb[B]/[HB+]) = KaKb where [A] = [HB+] and [B] = [A-].
Because it has a greater/higher Ka (dissociation constant). This is related to the ease with which the H+ can be released from the COOH group.