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  2. pH - Wikipedia

    en.wikipedia.org/wiki/PH

    A strong acid, such as hydrochloric acid, at concentration 1 mol dm −3 has a pH of 0, while a strong alkali like sodium hydroxide, at the same concentration, has a pH of 14. Since pH is a logarithmic scale, a difference of one in pH is equivalent to a tenfold difference in hydrogen ion concentration.

  3. Acid dissociation constant - Wikipedia

    en.wikipedia.org/wiki/Acid_dissociation_constant

    At half-neutralization the ratio ⁠ [A −] / [HA] ⁠ = 1; since log(1) = 0, the pH at half-neutralization is numerically equal to pK a. Conversely, when pH = pK a, the concentration of HA is equal to the concentration of A −. The buffer region extends over the approximate range pK a ± 2. Buffering is weak outside the range pK a ± 1.

  4. Hammett acidity function - Wikipedia

    en.wikipedia.org/wiki/Hammett_acidity_function

    The Hammett acidity function (H 0) is a measure of acidity that is used for very concentrated solutions of strong acids, including superacids.It was proposed by the physical organic chemist Louis Plack Hammett [1] [2] and is the best-known acidity function used to extend the measure of Brønsted–Lowry acidity beyond the dilute aqueous solutions for which the pH scale is useful.

  5. List of logarithmic identities - Wikipedia

    en.wikipedia.org/wiki/List_of_logarithmic_identities

    These are the three main logarithm laws/rules/principles, [3] from which the other properties listed above can be proven. Each of these logarithm properties correspond to their respective exponent law, and their derivations/proofs will hinge on those facts. There are multiple ways to derive/prove each logarithm law – this is just one possible ...

  6. Henderson–Hasselbalch equation - Wikipedia

    en.wikipedia.org/wiki/Henderson–Hasselbalch...

    The ocean contains a natural buffer system to maintain a pH between 8.1 and 8.3. [11] The oceans buffer system is known as the carbonate buffer system. [ 12 ] The carbonate buffer system is a series of reactions that uses carbonate as a buffer to convert C O 2 {\displaystyle \mathrm {CO_{2}} } into bicarbonate . [ 12 ]

  7. Predominance diagram - Wikipedia

    en.wikipedia.org/wiki/Predominance_diagram

    The three species all have concentrations equal to ⁠ 1 / K D ⁠ at pH = pK 1, for which [Cr] = ⁠ 4 / K D ⁠. [3] The three lines on this diagram meet at that point. Green line Chromate and hydrogen chromate have equal concentrations. Setting [CrO 2− 4] equal to [HCrO − 4] in eq. 1, [H +] = ⁠ 1 / K 1 ⁠, or pH = log K 1. This ...

  8. Logarithm - Wikipedia

    en.wikipedia.org/wiki/Logarithm

    Because log(x) is the sum of the terms of the form log(1 + 2 −k) corresponding to those k for which the factor 1 + 2 −k was included in the product P, log(x) may be computed by simple addition, using a table of log(1 + 2 −k) for all k. Any base may be used for the logarithm table. [53]

  9. Acid strength - Wikipedia

    en.wikipedia.org/wiki/Acid_strength

    When the acidic medium in question is a dilute aqueous solution, the is approximately equal to the pH value, which is a negative logarithm of the concentration of aqueous + in solution. The pH of a simple solution of an acid in water is determined by both K a {\displaystyle K_{{\ce {a}}}} and the acid concentration.