https://www.youtube.com/watch?v=TUKxfMi_xOY
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https://en.wikipedia.org/wiki/Acid_dissociation_constant
In chemistry, an acid dissociation constant (also known as acidity constant, or acid-ionization constant; denoted ) 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 chemical species HA is an acid that dissociates into A −, called the conjugate base of

https://byjus.com/chemistry/pka/
pKa - The pKa value is the negative base -10 logarithm of the acid dissociation constant (Ka) of a solution. The quantitative behavior of acids and bases in solution can be understood only if their pKa values are known. To learn more about Calculation of pka, List of pKa values, Relationship between pKa and pH and FAQs of pKa, Visit BYJU'S

https://sciencenotes.org/what-is-pka-in-chemistry-acid-dissociation-constant/
pKa is the negative base 10 log of the acid dissociation constant Ka. It indicates the strength of an acid. pKa in chemistry relates to the acid dissociation constant Ka as well as to pH and the strength of acids. Here is the pKa definition, its relationship with Ka and pH, and how pKa indicates whether an acid is strong or weak.

https://chem.libretexts.org/Courses/SUNY_Potsdam/Book%3A_Organic_Chemistry_I_(Walker)/06%3A_Acids_Bases_and_Electron_Flow/6.04%3A_Acid_strength_and_pKa
3. Nitro groups are very powerful electron-withdrawing groups. The phenol derivative picric acid (2,4,6 -trinitrophenol) has a pK a of 0.25, lower than that of trifluoroacetic acid. Use a resonance argument to explain why picric acid has such a low pKa. [reveal-answer q="475315″]Show Solution [/reveal-answer]

https://chem.libretexts.org/Courses/University_of_Illinois_Springfield/UIS%3A_CHE_267_-_Organic_Chemistry_I_(Morsch)/Chapters/Chapter_02%3A_Acids_and_Bases/5.2%3A_Acid_Strength_and_pKa
Looking at Table 5.2.1 5.2. 1, you see that the pK a of carboxylic acids are in the 4-5 range, the pK a of sulfuric acid is -10, and the pK a of water is 14. Alkenes and alkanes, which are not acidic at all, have pK a values above 30. The lower the pKa value, the stronger the acid. Table 5.2.1 5.2. 1: Representative acid constants.

https://www.khanacademy.org/science/organic-chemistry/organic-structures/acid-base-review/v/using-a-pka-table
So pKa tables are important for thinking about the strengths of acids, and you can also use them to think about the strengths of bases. Learn for free about math, art, computer programming, economics, physics, chemistry, biology, medicine, finance, history, and more. Khan Academy is a nonprofit with the mission of providing a free, world-class

https://organicchemistrydata.org/hansreich/resources/pka/
General Info. pKa is an acid dissociation constant used to describe the acidity of a particular molecule. Its value is directly related to the structure of the given compound. The constant changes depending on the solvent the compound is used in. Typically, organic chemists compare the various values from their determination in water, DMSO and

https://www.thoughtco.com/what-is-pka-in-chemistry-605521
pKa Definition . pK a is the negative base-10 logarithm of the acid dissociation constant (K a) of a solution. pKa = -log 10 K a The lower the pK a value, the stronger the acid.For example, the pKa of acetic acid is 4.8, while the pKa of lactic acid is 3.8. Using the pKa values, one can see lactic acid is a stronger acid than acetic acid.

https://en.wikipedia.org/wiki/Dissociation_constant
Dissociation constant. In chemistry, biochemistry, and pharmacology, a dissociation constant ( KD) is a specific type of equilibrium constant that measures the propensity of a larger object to separate (dissociate) reversibly into smaller components, as when a complex falls apart into its component molecules, or when a salt splits up into its

https://chem.libretexts.org/Courses/Purdue/Purdue%3A_Chem_26505%3A_Organic_Chemistry_I_(Lipton)/Chapter_8._Acid-Base_Reactions/8.3%3A_pKa_Values
A pKa may be a small, negative number, such as -3 or -5. It may be a larger, positive number, such as 30 or 50. The lower the pKa of a Bronsted acid, the more easily it gives up its proton. The higher the pKa of a Bronsted acid, the more tightly the proton is held, and the less easily the proton is given up. Figure AB9.2.

https://www.thoughtco.com/ph-pka-ka-pkb-and-kb-explained-4027791
Ka, pKa, Kb, and pKb are most helpful when predicting whether a species will donate or accept protons at a specific pH value. They describe the degree of ionization of an acid or base and are true indicators of acid or base strength because adding water to a solution will not change the equilibrium constant. Ka and pKa relate to acids, while Kb

https://sciencenotes.org/ph-pka-ka-pkb-and-kb-in-chemistry/
pKa gives the same information, but in a different way. The smaller the pKa value, the stronger the acid. Or, the larger the pKa value, the weaker the acid. Weak acids typically have pKa values between 2 and 14. pKb and Kb. Kb is the base dissociation constant and pKb is the -log of this constant. A base dissociates according to the general

https://www.khanacademy.org/science/chemistry/acids-and-bases-topic/buffer-solutions/v/ph-and-pka-relationship-for-buffers
So let's go ahead and look at all the possible scenarios for these three things. We're going to start with the simplest possible scenario, which is that pH is equal to pK_a. When pH is equal to pK_a, we're raising 10 to the zeroth power. So anything to the zeroth power is equal to one. Which tells us that this ratio is equal to one.

https://www.khanacademy.org/science/organic-chemistry/organic-structures/acid-base-review/v/using-pka-values-to-predict-the-position-of-equilibrium-new
The pKa of the acid isn't dependent on the pKb or strength of the base. The equilibrium constant, Keq, which roughly measures how how readily the reactants will become the products, will. Think of it like two children who want the same toy. Suzy has the toy. Billy wants to take it. How badly Billy wants the toy won't effect how much Suzy wants

https://chemistrytalk.org/what-is-pka/
In simple terms, pKa is a number that shows how weak or strong an acid is. A strong acid will have a pKa of less than zero. More precisely a negative value is the negative log base ten of the Ka value (acid dissociation constant). It measures the strength of an acid — how tightly a proton is held by a Bronsted acid.

https://chem.libretexts.org/Bookshelves/Organic_Chemistry/Map%3A_Essential_Organic_Chemistry_(Bruice)/02%3A_Acids_and_Bases/2.2%3A_pka_and_pH
pH and pOH. Because the constant of water, K w is \(1.0 \times 10^{-14}\) (at 25° C), the \(pK_w\) is 14, the constant of water determines the range of the pH scale. To understand what the pK w is, it is important to understand first what the "p" means in pOH and pH. The addition of the "p" reflects the negative of the logarithm, \(-\log\). Therefore, the pH is the negative logarithm of the

https://www.masterorganicchemistry.com/2010/09/29/how-to-use-a-pka-table/
Click to Flip. In order to get a better grasp on these numbers, we often take the negative logarithm of the acidity constant and call this pKa. pK a = - log K a. Click to Flip. The higher the pK a, the weaker the acid. The lower the pK a, the stronger the acid. One of the strongest acids, H-I has a pK a of -10.

https://www.youtube.com/watch?v=L7flgA0n_tc
This organic chemistry video tutorial provides a list of pKa values of many common acids. Acid strength is inversely related to pKa.Access The Full 57 Minut

https://chem.libretexts.org/Courses/Sacramento_City_College/SCC%3A_Chem_420_-_Organic_Chemistry_I/Text/01%3A_Introduction_and_Review/1.14%3A_Distinguishing_between_pH_and_pKa
Some selected pKa values for compounds in the study of organic chemistry are shown bellow. Since organic reactions can be performed in non-aqueous environments, the pH can exceed 14 and organic compounds can have pKa values above 16. It is a variation on that line from the Wizard of Oz, "We don't live in water anymore."

https://www.khanacademy.org/science/organic-chemistry/organic-structures/acid-base-review/v/ka-and-pka-review
The pKa is defined as the negative log of the Ka. If we wanted to find the pKa for methanol, all we have to do is take the Ka and take the negative log of it. So the pKa is equal to the negative log of 2.9 times 10 to the negative 16. Let's get out the calculator and let's do that. Negative log of 2.9 times 10 to the negative 16.

https://www.omnicalculator.com/chemistry/pka
The pKa of acetic acid is 4.745. Given the K a of 1.8 × 10 -5, pK a can be calculated as follows: pK a = -log 10 [K a] pK a = - (-4.745) = 4.745. This pKa calculator helps you find the pKa from pH with the Henderson-Hasselbalch equation or with acid dissociation constant (Ka) values.

https://chem.libretexts.org/Courses/Brevard_College/CHE_104%3A_Principles_of_Chemistry_II/07%3A_Acid_and_Base_Equilibria/7.12%3A_Relationship_between_Ka_Kb_pKa_and_pKb
We could also have converted Kb to pKb to obtain the same answer: pKb = − log(5.4 × 10 − 4) = 3.27. pKa + pKb = 14.00. pKa = 10.73. Ka = 10 − pKa = 10 − 10.73 = 1.9 × 10 − 11. If we are given any one of these four quantities for an acid or a base ( Ka, pKa, Kb, or pKb ), we can calculate the other three.