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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.
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What is the Henderson-Hasselbalch equation?
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 for acrylic acid is 0.000056 calculate the pH of 0.10m aqueous solution of acrylic acidCalculate percent dissociation of 0.10m solution of acrylic acid?
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 %
What is recommendation of burglary?
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Scope and delimitation of malunggay?
- Malunggay Disinfectant - Malunggay as Regualar Cooking Oil - Malunggay as Cleaning Agent - Malunggay as Ointment - Malunggay as Shampoo - Malunggay as Herbal Tea - Malunggay as Rice Coffee there are many possible investigatory projects.
How do you make cardboard using peanut shells?
tae ka
What is the dissociation constant or Ka for salicylic acid?
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
What is the ka value for sulfamic acid?
According to CRC reference data, the pKa of sulfamic acid is 1.05, giving a Ka of 11.2. This is a strong acid.
What is the accepted Ka value for sodium hydroxide?
NaOH does not have a Ka because it is not an acid. Ka is the concentration of the acid, therefore non valid. It can have a Kb though. Hope this helps
Why is the PH of the midpoint predicted to be the same value as the weak acid?
if you mean why is it when [H+] = [A-] related to the Ka of a weak acid. look at the definition of Ka. Ka = [H+][A-]/[HA]
Which of the following Ka value represent the weakest acid?
ka= 1.62 x 10^-12
What is the Ka value for hydrobromic acid?
1 x 109
Why is Ka an important value in chemistry?
For a weak acid, the value of Ka gives one an indication of the degree to which that weak acid will dissociate. This then gives one an idea of the acidity of that weak acid, and it can be easily compared to other weak acids.
How do you calculate concentration of phosphoric acid?
You can do it with a pH probe, or, if you are given the Ka value for phosphoric acid, you can do some math and figure it out.
What does a Ka value of approximately 1 show about the equilibrium?
some of the acid has dissociated APEX
Is an acid with a small Ka stronger than an acid with a large Ka?
No. An acid with a large Ka is stronger. A lower pKa indicates a stronger acid.
How do you determine ka from strong acid strong base titration curve?
This is a relatively easy question. First, you should have your chemical equation. HA + h20 <---> A^1- + H30^1+ Basically Ka is our ionization constant. The simple formula for this is Products / Reactants. Water is excluded because it doesnt contribute to the Ka although it acts as a Bronsted-Lowry Base on the left side of the equation. So the Ka of a weak acid should be : Ka = [H30^1+] X [A^1-] / [HA] A^- is the conjugate base of the weak acid. If they give u Kb value its even easier. You should have learned that Kw = [Ka] x [Kb] Kw at 25 degrees celsius should always be 1.00 x 10^-14. So if they give you kb.... Ka = 1.00 x 10^-14 / Kb value. I hope this helped! Galvin H
Is ascorbic acid weak?
The acid dissociation constant (Ka) is the measure of strength of an acid in solution. Symbolically, as HA is added to solution it breaks down into a proton (H+) and it's conjugate base (A-). The value of Ka is equal to products over reactants (aqueous only i.e. no solids or liquids) . Once you solve for Ka, you can solve for the pKa which is equal to -logKa. The pKa will determine if the acid is weak or strong. Strong acids are more willing to dissociate in water and have a pKa value of <-2. The pKa of ascorbic acid is only 4.2, and so it is a weak acid.
