Scale used to specify the acidity or basicity of an aqueous solution.- PH
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Molecule or ion capable of either donating a proton , known as a Brønsted–Lowry acid, or forming a covalent bond with an electron pair, known as a Lewis acid.
An aqueous solution of an acid has a pH less than 8 and is colloquially also referred to as "acid" (as in "dissolved in acid"), while the strict definition refers only to the solute.
In chemistry, there are three definitions in common use of the word base, known as Arrhenius bases, Brønsted bases, and Lewis bases.
In water, by altering the autoionization equilibrium, bases yield solutions in which the hydrogen ion activity is lower than it is in pure water, i.e., the water has a pH higher than 7.0 at standard conditions.
Common name for the aqueous cation, the type of oxonium ion produced by protonation of water.
The concentration of hydronium or H+ ions determines a solution's pH according to
A pH indicator is a halochromic chemical compound added in small amounts to a solution so the pH (acidity or basicity) of the solution can be determined visually.
A buffer solution (more precisely, pH buffer or hydrogen ion buffer) is an aqueous solution consisting of a mixture of a weak acid and its conjugate base, or vice versa.
Way of displaying numerical data over a very wide range of values in a compact way—typically the largest numbers in the data are hundreds or even thousands of times larger than the smallest numbers.
pH for acidity
Quantitative measure of the strength of an acid in solution.
In particular, the pH of a solution can be predicted when the analytical concentration and pKa values of all acids and bases are known; conversely, it is possible to calculate the equilibrium concentration of the acids and bases in solution when the pH is known.
[[File:Logarithm plots.png|right|thumb|upright=1.35|Plots of logarithm functions, with three commonly used bases. The special points
In chemistry, pH is a logarithmic measure for the acidity of an aqueous solution.
Water that has been mechanically filtered or processed to remove impurities and make it suitable for use.
Softening consists in preventing the possible precipitation of poorly soluble minerals from natural water due to changes occurring in the physico-chemical conditions (such as pCO2, pH, and Eh).
Common laboratory method of quantitative chemical analysis to determine the concentration of an identified analyte (a substance to be analyzed).
Many non-acid–base titrations require a constant pH during the reaction.