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2. Boric acid - Wikipedia

   en.wikipedia.org/wiki/Boric_acid

   Boric acid in equilibrium with its conjugate base the borate ion is widely used (in the concentration range 50–100 ppm boron equivalents) as a primary or adjunct pH buffer system in swimming pools. Boric acid is a weak acid, with p K a (the pH at which buffering is strongest because the free acid and borate ion are in equal concentrations) of ...

3. Oligodynamic effect - Wikipedia

   en.wikipedia.org/wiki/Oligodynamic_effect

   Boric acid esters derived from ... swimming pools, and ... Phenylmercuric borate and acetate were used for disinfecting mucous membranes at an effective concentration ...

4. Boric acid (data page) - Wikipedia

   en.wikipedia.org/wiki/Boric_acid_(data_page)

   This page provides supplementary chemical data on boric acid. Thermodynamic properties. Phase behavior Triple point? K (? °C), ? Pa Critical point? K (? °C), ?

5. Swimming pool sanitation - Wikipedia

   en.wikipedia.org/wiki/Swimming_pool_sanitation

   Swimming pool contaminants are introduced from environmental sources and swimmers. Affecting primarily outdoor swimming pools, environmental contaminants include windblown dirt and debris, incoming water from unsanitary sources, rain containing microscopic algae spores and droppings from birds possibly harboring disease-causing pathogens. [4]

6. Borax - Wikipedia

   en.wikipedia.org/wiki/Borax

   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

7. Fluoroboric acid - Wikipedia

   en.wikipedia.org/wiki/Fluoroboric_acid

   Fluoroboric acid is corrosive and attacks the skin. It is available commercially as a solution in water and other solvents such as diethyl ether. It is a strong acid with a weakly coordinating, non-oxidizing conjugate base. [2] It is structurally similar to perchloric acid, but lacks the hazards associated with oxidants.

8. Borate buffered saline - Wikipedia

   en.wikipedia.org/wiki/Borate_buffered_saline

   Borate concentration (giving buffering capacity) can vary from 10 mM to 100 mM. As BBS is used to emulate physiological conditions (as in animal or human body), the pH value is slightly alkaline, ranging from 8.0 to 9.0. NaCl gives the isotonic (mostly used 150 mM NaCl corresponds to physiological conditions: 0.9% NaCl) salt concentration.

9. Dakin's solution - Wikipedia

   en.wikipedia.org/wiki/Dakin's_solution

   Other formulations have been developed over time. In 1916, Marcel Daufresne substituted sodium bicarbonate for Dakin's boric acid as buffering agent. [7] [17] This formulation is the basis of current commercial products. [18] The concentration chosen by Dakin (0.5%) was the maximum highest concentration found tolerable to the skin.