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.
Note- See the related link for the complete derivation belowSUMMARY OF ACID-DISSOCIATION CONSTANT (pKa) (from Rhoades and Pflanzer Human Physiology)HA ßà H+ + A-1) Reaction to the right à dissociation reaction2) Reaction to left à association reactionThe rate of the dissociation reaction = [HA] x dissociation rate constant k1 (which is a specific value for this reaction).The rate of the association reaction = [H+] x [A-] x association rate constant k2At equilibrium à rates of association and dissociation are =. Thereforek1 x [HA] = k2 x [H+] x [A-]Hence à [H+] x [A-] /[HA] = k1/k2A NEW CONSTANT à is defined for k1/k2 à we call it Ka (equilibrium constant for the reaction and dissociation constant for the acid)A HIGHER Ka à more completely an acid is dissociated à stronger acid à lower pHA LOWER Ka à not as much dissociation à weak acid à higher pHThe Ka is often small in difficult to manipulate à so we present the number in a logarithmic form à pKa (which is the log10 of the INVERSE of KapKa = log10(1/Ka) = --log10(Ka)LOW pKaà high dissociation constant à STRONG ACIDHIGH pKa à low dissociation constant à WEAK ACIDTHE HENDERSON HASSELBALCH EQUATION[H+] x [A-] /[HA] = Ka à therefore[H+] = Ka x [HA] / [A-]Take log of both sidelog[H+] = logKa + log([HA]/[A-]) à multiple both sides by -1-- log[H+] = --logKa + log([A-]/[HA])And because pH = --log[H+] and pKa = log(1/Ka) = --log(Ka)pH = pKa + log([A-]/[HA])HENCE à WHEN [A-] = [HA] à the pH of solution = it's pKa (because the log1 is 0)Conversely à the pKa is the pH at which there are as many molecules of weak acid as there are conjugate base in solution.For the bicarbonate buffer system à (pK = 6.1)Cheers
Ka = ([H+][A-])/[HA]) Let concentration of dissociated acrylic acid be x. 0.000056 = (x2)/(0.10 - x) Rearrange: 0.0000056 - 0.000056x - x2 = 0 x = 0.002339 Therefore: [H+] = 0.002339 M pH = -log[H+] = 2.63 Percent dissociation: 0.002339/0.10 = 0.02339 = 2.34 %
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Gago patakla ka ne
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 Ka value of a weak acid is inversely related to its acid strength. A higher Ka value indicates a stronger acid, while a lower Ka value indicates a weaker acid. Acid strength is determined by the extent of dissociation of the acid in solution, with stronger acids having higher dissociation constants (Ka values).
ka= 1.62 x 10^-12
According to CRC reference data, the pKa of sulfamic acid is 1.05, giving a Ka of 11.2. This is a strong acid.
The Ka value for hydrobromic acid (HBr) is approximately 9.0 x 10^-10.
The K value, or acid dissociation constant (Ka), indicates the strength of an acid in solution. A smaller Ka value corresponds to a weaker acid, as it signifies a lower degree of dissociation in water. Therefore, the weakest acid would have the smallest Ka value, approaching zero, indicating that it does not ionize significantly in solution.
The Ka value of H3O helps determine the strength of an acid by indicating how well the acid donates protons in a solution. A higher Ka value means the acid is stronger, as it more readily donates protons, leading to a higher concentration of H3O ions in the solution.
The Ka value of nitric acid (HNO3) is approximately 25 × 10^6.
To determine the concentration of H ions from the acid dissociation constant (Ka), you can use the formula H (Ka x acid). This formula helps calculate the concentration of H ions in a solution based on the given Ka value of the acid and the initial concentration of the acid.
To calculate the Ka of an acid, you can use the equation Ka H3OA- / HA, where H3O is the concentration of hydronium ions, A- is the concentration of the conjugate base, and HA is the concentration of the acid. The Ka value represents the acid's strength in donating protons in a solution.
The Ka value of a weak acid is smaller than the Ka value of a strong acid because weak acids only partially dissociate in solution, resulting in lower concentrations of H+ ions. Strong acids like hydrochloric acid (HCl) completely dissociate in solution, leading to higher concentrations of H+ ions and therefore a larger Ka value.
The Ka value closest to 1 x 10^-7 represents the weakest acid, as this value corresponds to a neutral solution and indicates a weaker dissociation of the acid.