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Boric acid, more specifically orthoboric acid, is a compound of boron, oxygen, and hydrogen with formula B(OH) 3.It may also be called hydrogen orthoborate, trihydroxidoboron or boracic acid. [3]
The acidity of fluoroboric acid is complicated by the fact that its name refers to a range of different compounds, e.g. [H(CH 3 CH 2) 2 O] + [BF 4] − (dimethyloxonium tetrafluoroborate), [H 3 O] + [BF 4] − (oxonium tetrafluoroborate), and HF·BF 3 (hydrogen fluoride-boron trifluoride 1:1 adduct) – each with a different acidity.
Monobasic may refer to: A monobasic or monoprotic acid, able to donate one proton per molecule; A monobasic salt, with one hydrogen atom, with respect to the parent acid, replaced by cations; Monobasic, or Monotypic taxon, a taxonomic group (taxon) that contains only one immediately subordinate taxon; Monobasic, an album by Jess Cornelius
It can be seen in the table above that the second proton is removed from a negatively charged species. Since the proton carries a positive charge extra work is needed to remove it, which is why pK a2 is greater than pK a1. pK a3 is greater than pK a2 because there is further charge separation. When an exception to Pauling's rule is found, it ...
Structure of ammonium chloride. Acid–base property of the resulting solution from a neutralization reaction depends on the remaining salt products. A salt containing reactive cations undergo hydrolysis by which they react with water molecules, causing deprotonation of the conjugate acids.
Chemical nomenclature is a set of rules to generate systematic names for chemical compounds.The nomenclature used most frequently worldwide is the one created and developed by the International Union of Pure and Applied Chemistry (IUPAC).
There’s no single explanation for why addiction treatment is mired in a kind of scientific dark age, why addicts are denied the help that modern medicine can offer. Family doctors tend to see addicts as a nuisance or a liability and don’t want them crowding their waiting rooms. In American culture, self-help runs deep.
The molar ionic strength, I, of a solution is a function of the concentration of all ions present in that solution. [3]= = where one half is because we are including both cations and anions, c i is the molar concentration of ion i (M, mol/L), z i is the charge number of that ion, and the sum is taken over all ions in the solution.