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You can see that hydroxide ion is a stronger base than ammonia (NH 3), because ammonium (NH 4 +, pK a = 9.2) is a stronger acid than water (pK a = 14.00). The stronger the conjugate acid, the weaker the conjugate base.
27 Οκτ 2017 · This page by Professor Hans Reich (UW-Madison) provides a collection of common structural motifs in Organic Chemistry and their corresponding pKa values.
25 Νοε 2010 · pH = pK a + [A -] / [HA] and further. pH - pK a = log [A -] / [HA] Then, a solution with 50% dissociation has pH equal to the pK a of the acid. Polyprotic acids are acids that can lose more than one proton. Then we have more than one dissiciation constant; K a1, K a2, etc.. and similar pK a1, pK a2, etc.
For strengths of organic acids see E. P. Serjeant and B. Dempsey (eds.), Ionization Constants of Organic Acids in Solution, IUPAC Chemical Data Series No. 23, Pergamon Press, Oxford, UK, 1979. The strength of a base is related to the pK a of its conjugate acid as pK b = 14 - pK a.
Ammonium phosphate is the inorganic compound with the formula (NH 4) 3 PO 4. It is the ammonium salt of orthophosphoric acid. A related "double salt", (NH 4) 3 PO 4. (NH 4) 2 HPO 4 is also recognized but is impractical to use. Both triammonium salts evolve ammonia.
28 Απρ 2021 · To know the relationship between acid or base strength and the magnitude of Ka, Kb, pKa, and pKb. The magnitude of the equilibrium constant for an ionization reaction can be used to determine the relative strengths of acids and bases.
pKa = -log [Ka] Acid dissociation constants, or pKa values, are essential for understanding many fundamental reactions in chemistry. These values reveal the deprotonation state of a molecule in a particular solvent. There is great interest in using theoretical methods to calculate the pKa values for many different types of molecules.
