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The sour taste o lemon juice is a result o it bein componed o aboot 5% tae 6% citric acid, an acid wi a pH o roughly 2.2.

In chemistry, pH (/p / or /p h/) is a measur o the acidity or basicity o an aqueous solution. Solutions wi a pH less nor 7 are said tae be acidic an solutions wi a pH greater than 7 are basic or alkaline. Pure watter haes a pH very close tae 7.

The pH scale is traceable tae a set o staundart solutions whose pH is established bi internaitional agreement.[1] Primary pH staundart values are determined uisin a concentration cell wi transference, bi measurin the potential difference atween a hydrogen electrode an a staundart electrode sic as the silver chloride electrode. Measurment o pH for aqueous solutions can be duin wi a glass electrode an a pH meter, or uisin indicators.

pH measurements are important in medicine, biology, chemistry, agricultur, forestry, fuid science, environmental science, oceanography, ceevil ingineerin, chemical ingineerin, nutrition, watter treatment & watter purification, an mony ither applications.

Mathematically, pH is the negative logarithm o the activity o the (solvatit) hydronium ion, mair eften expressed as the measur o the hydronium ion concentration.[2]

References[eedit | eedit soorce]

  1. Covington, A. K.; Bates, R. G.; Durst, R. A. (1985). "Definitions of pH scales, standard reference values, measurement of pH, and related terminology" (PDF). Pure Appl. Chem. 57 (3): 531–542. doi:10.1351/pac198557030531.
  2. Bates, Roger G. Determination of pH: theory and practice. Wiley, 1973.