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Infusion of bicarbonate is indicated only when the blood pH is markedly low (< 7.1–7.0). [42] HCO 3 − is used for treatment of hyperkalemia, as it will drive K + back into cells during periods of acidosis. [43] Since sodium bicarbonate can cause alkalosis, it is sometimes used to treat aspirin overdoses.
Normal bases are also nucleophiles, but often chemists seek the proton-removing ability of a base without any other functions. Typical non-nucleophilic bases are bulky, such that protons can attach to the basic center but alkylation and complexation is inhibited.
The bicarbonate ion carries a negative one formal charge and is an amphiprotic species which has both acidic and basic properties. It is both the conjugate base of carbonic acid H 2 CO 3; and the conjugate acid of CO 2− 3, the carbonate ion, as shown by these equilibrium reactions: CO 2− 3 + 2 H 2 O ⇌ HCO − 3 + H 2 O + OH − ⇌ H 2 CO ...
[7] Another possibility is the molecular autoionization reaction between two water molecules, in which one water molecule acts as an acid and another as a base. H 2 O + H 2 O ⇌ H 3 O + + HO −. The bicarbonate ion, HCO − 3, is amphoteric as it can act as either an acid or a base: As an acid, losing a proton: HCO − 3 + OH − ⇌ CO 2− ...
According to the original formulation of Lewis, when a neutral base forms a bond with a neutral acid, a condition of electric stress occurs. [7] The acid and the base share the electron pair that formerly belonged to the base. [7] As a result, a high dipole moment is created, which can only be decreased to zero by rearranging the molecules. [7]
sodium chromate Na 2 CrO 4 is made yellow by the chromate ion CrO 2− 4. potassium dichromate K 2 Cr 2 O 7 is made red-orange by the dichromate ion Cr 2 O 2− 7. cobalt(II) nitrate hexahydrate Co(NO 3) 2 ·6H 2 O is made red by the chromophore of hydrated cobalt(II) [Co(H 2 O) 6] 2+. copper(II) sulfate pentahydrate CuSO 4 ·5H 2 O is made ...
In order to distinguish this alternate base pairing scheme from the Watson-Crick scheme, base pairs where a hydrogen bond involves the N7 atom of a purine residue have been referred to as Hoogsteen base pair, and later, the purine base edge which includes its N7 atom is referred to as its Hoogsteen edge.
A mixture of 4,4'-oxydianiline 1 (1.00 g, 5.00 mmol) and o-vanillin 2 (1.52 g, 10.0 mmol) in methanol (40.0 ml) is stirred at room temperature for one hour to give an orange precipitate and after filtration and washing with methanol to give the pure Schiff base 3 (2.27 g, 97%)