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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.
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
Std enthalpy change. of formation, Δ fH o gas. −992.28 kJ/mol. Standard molar entropy, S o gas. 295.23 J/ (mol K) Heat capacity, cp. J/ (mol K)
The form in which boron is consumed has changed in recent years. The use of ores like colemanite has declined following concerns over arsenic content. Consumers have moved toward the use of refined borates and boric acid that have a lower pollutant content. Increasing demand for boric acid has led a number of producers to invest in additional ...
Boric acid goes to anhydrous microcrystalline B 2 O 3 in a heated fluidized bed. [21] Carefully controlled heating rate avoids gumming as water evolves. Boron oxide will also form when diborane (B 2 H 6) reacts with oxygen in the air or trace amounts of moisture: 2B 2 H 6 (g) + 3O 2 (g) → 2 B 2 O 3 (s) + 6H 2 (g) B 2 H 6 (g) + 3H 2 O(g) → B ...
Sodium borate. Sodium borate is a generic name for any salt of sodium with an anion consisting of boron and oxygen, and possibly hydrogen, or any hydrate thereof. It can be seen as a hydrated sodium salt of the appropriate boroxy acid, although the latter may not be a stable compound. Many sodium borates have important industrial and household ...