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Boric acid is a weak acid, with pK a (the pH at which buffering is strongest because the free acid and borate ion are in equal concentrations) of 9.24 in pure water at 25 °C. But apparent p K a is substantially lower in swimming pool or ocean waters because of interactions with various other molecules in solution.
Boracic lint (/ b ɒ ˈ r æ s ɪ k /) is a type of medical dressing made from surgical lint that is soaked in a hot, saturated solution of boracic acid and glycerine and then left to dry. Medical dressing
Borate anions are largely in the form of the undissociated acid in aqueous solution at physiological pH. No further metabolism occurs in either animals or plants. In animals, boric acid/borate salts are essentially completely absorbed following oral ingestion. Absorption occurs via inhalation, although quantitative data are unavailable.
Borate buffered saline (abbreviated BBS) is a buffer used in some biochemical techniques to maintain the pH within a relatively narrow range. Borate buffers have an alkaline buffering capacity in the 8–10 range. Boric acid has a pK a of 9.14 at 25 °C.
This page provides supplementary chemical data on boric acid. Thermodynamic properties. Phase behavior Triple point? K (? °C), ? Pa Critical point? K (? °C), ?
Boric is a chemistry term that refers to substances containing boron, such as: boric acid or orthoboric acid, B(OH) 3; metaboric acid, an acid containing boron, HBO 2; tetraboric acid or pyroboric acid, an acid containing boron, H 2 B 4 O 7; boric oxide, specifically boron trioxide B 2 O 3; a boric ester, or organic borate; Boric may also refer to:
Boron, silicon, arsenic, and antimony have medical applications, and germanium and tellurium are thought to have potential. Boron is used in insecticides [121] and herbicides. [122] It is an essential trace element. [123] As boric acid, it has antiseptic, antifungal, and antiviral properties. [124]
Borax is also easily converted to boric acid and other borates, which have many applications. Its reaction with hydrochloric acid to form boric acid is: Na 2 B 4 O 7 ·10H 2 O + 2 HCl → 4 H 3 BO 3 + 2 NaCl + 5 H 2 O. Borax is sufficiently stable to find use as a primary standard for acid-base titrimetry. [17]: p.316
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