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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 ...
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.
In the environment these species usually include boric acid and borate, for example: B T = [H 2 BO − 3] + [H 3 BO 3] where B T is the total boron concentration [H 2 BO − 3] is the dihydrogen borate concentration [H 3 BO 3] is the boric acid concentration
Polymeric boron oxoanions are formed in aqueous solution of boric acid at pH 7–10 if the boron concentration is higher than about 0.025 mol/L. The best known of these is the tetraborate ion [B 4 O 7 ] 2− , found in the mineral borax:
Example Bjerrum plot: Change in carbonate system of seawater from ocean acidification.. A Bjerrum plot (named after Niels Bjerrum), sometimes also known as a Sillén diagram (after Lars Gunnar Sillén), or a Hägg diagram (after Gunnar Hägg) [1] is a graph of the concentrations of the different species of a polyprotic acid in a solution, as a function of pH, [2] when the solution is at ...
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:
Phase behavior Triple point? K (? °C), ? Pa Critical point? K (? °C), ? Pa Std enthalpy change of fusion, Δ fus H o? kJ/mol Std entropy change of fusion, Δ fus S oJ/(mol·K)
Sodium perborate hydrolyzes (i.e. breaks down in contact with water), producing hydrogen peroxide and borate: [3] (HO) 2 B] 2 (OO) 2) 2− + 2 H 2 O ⇌ 2 [(HO) 2 B(OH)(OOH)] − The resulting hydroperoxide then enter in equilibrium with boric acid B(OH) 3, hydrogen peroxide H 2 O 2, the hydroperoxyl anion − OOH, and the tetrahydroxyborate anion [B(OH) 4] −: [2]