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3 exist in aqueous solutions subjected to pressures of multiple gigapascals (tens of thousands of atmospheres) in planetary interiors. [17] [18] Pressures of 0.6–1.6 GPa at 100 K, and 0.75–1.75 GPa at 300 K are attained in the cores of large icy satellites such as Ganymede, Callisto, and Titan, where water and carbon dioxide are present ...
3. 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 ...
3 Ammonia: NH + 4 Ammonium ion C 5 H 5 N Pyridine: C 5 H 6 N + Pyridinium: C 6 H 5 NH 2 Aniline: C 6 H 5 NH + 3 Phenylammonium ion C 6 H 5 CO − 2 Benzoate ion C 6 H 6 CO 2 Benzoic acid: F − Fluoride ion HF Hydrogen fluoride: PO 3− 4 Phosphate ion HPO 2− 4 Hydrogen phosphate ion OH − Hydroxide ion H 2 O Water (neutral, pH 7) HCO − 3 ...
It is the conjugate base of the hydrogencarbonate (bicarbonate) [8] ion, HCO − 3, which is the conjugate base of H 2 CO 3, carbonic acid. The Lewis structure of the carbonate ion has two (long) single bonds to negative oxygen atoms, and one short double bond to a neutral oxygen atom.
It is equal to 6.1. [HCO − 3] is the concentration of bicarbonate in the blood [H 2 CO 3] is the concentration of carbonic acid in the blood; When describing arterial blood gas, the Henderson–Hasselbalch equation is usually quoted in terms of pCO 2, the partial pressure of carbon dioxide, rather than H 2 CO 3 concentration.
1,3,5,7-Adamantanetetracarboxylic acid is an adamantane derivative containing four carboxylic acid groups bonded to each of its four tetrahedral carbon centers. Its tetrahedral symmetry provides applications as a hydrogen-bonded organic framework linker [ 4 ] and as a dendrimer core.
This list is ordered by the number of carbon atoms in a carboxylic acid. C1. IUPAC name: ... C 4 H 9 CH(C 2 H 5)COOH 3-ethanehexanoic acid C 3 H 7 CH(C 2 H 5)CH 2 COOH
The HCO 3 − and H + are ideal for buffering pH in the blood and tissues because the pKa is close to the physiological pH = 7.2 – 7.6. Since HCO 3 − and H + are regulated in the kidneys and plasma carbon dioxide is regulated in the lungs, both actions in the kidneys and lungs are important to maintain the stability of blood pH.