Formation Constants of Metal Complexes of Tropolone and its Derivatives. II. Some Alkyltropolones1,2

1954 ◽  
Vol 76 (6) ◽  
pp. 1696-1697 ◽  
Author(s):  
Burl E. Bryant ◽  
W. Conard Fernelius
Keyword(s):  
Metal Complexes ◽  
Formation Constants

The formation constants of some metal complexes with 3-Acetyl-4-hydroxycoumarin, dehydroacetic acid, and their oximes

1971 ◽  
Vol 24 (5) ◽  
pp. 925 ◽  
Author(s):  
GCS Manku
Keyword(s):  
Metal Complexes ◽  
Sodium Perchlorate ◽  
Formation Constants ◽  
Ionic Concentration ◽  
Dehydroacetic Acid ◽  
Nitrogen Donors ◽  
Oxygen Donors

The formation constants (K1, K2, and β2) of the complexes of 3-acetyl-4- hydroxycoumarin (ahc) and dehydroacetic acid (dha) and their respective oximes, ahco and dhao, with iron(II), cobalt(II), nickel(II), copper(II), zinc(II), calcium(II), magnesium(II), cadmium(II), dioxouranium(VI), iron(III), aluminium(III), scandium(III), indium(III), yttrium(III), and lanthanon(III) ions (lanthanum to lutetium inclusive with the exception of promethium) have been determined pH-metrically at 35� in 50% v/v aqueous dioxan medium with 0.100M sodium perchlorate as the constant ionic concentration, using Calvin and Wilson's pH-metric technique. The trends in the formation constants of these complexes are discussed. It is observed that, except in the case of Co2+, Ni2+, and Cu2+ ions, for which chelation through nitrogen donors is more favoured, all other ions prefer coordination through oxygen donors.

Solubility and Complex-Ion Equilibria

2021 ◽  
pp. 313-324
Author(s):  
Christopher O. Oriakhi
Keyword(s):  
Metal Complexes ◽  
Solubility Product ◽  
Formation Constants ◽  
Aqueous Systems ◽  
Complex Ions ◽  
Ionic Compounds ◽  
Molar Solubility ◽  
Solubility Product Constant ◽  
Complex Ion

Solubility and Complex-Ion Equilibria broadens the previous chapter’s coverage of equilibria to include aqueous systems containing two or more solutes of slightly soluble ionic compounds and the formation of metal complexes in solution. Solubility equilibria which allow quantitative predictions of how much of a compound will dissolve under given conditions are covered. The meaning of the solubility product constant (K sp) and how to calculate it from molar solubility values is presented. Also discussed is determination of molar solubility from K sp. Calculations demonstrate how to predict the formation of a precipitate by comparing the ion product or solubility quotient (Q) with K sp. Formation constants of complex ions and calculations involving complex ion equilibria are explained.

scholarly journals The proton and metal complexes of adenyl-5′-yl imidodiphosphate

1976 ◽  
Vol 159 (1) ◽  
pp. 169-171 ◽  
Author(s):  
L D Pettit ◽  
K F Siddiqui
Keyword(s):  
Complex Formation ◽  
Transition Metal ◽  
Metal Ions ◽  
Metal Complexes ◽  
Transition Metal Ions ◽  
Formation Constants ◽  
Enthalpy Change ◽  
Two Temperatures ◽  
Bivalent Transition Metal

The formation constants of the complexes of adenyl-5′-yl imidodiphosphate with H+ Mg2+, Ca2+ and a number of bivalent transition-metal ions were measured potentionmetrically. The complexes are generally a little more stable than the analogous complexes of ATP. By measuring the formation constants at two temperatures, this increase in stability was shown to result from an increased enthalpy change on complex-formation.

scholarly journals Studies on thermodynamic and formation constants of metal complexes in solution

2009 ◽  
Vol 6 (2) ◽  
pp. 357-400
Author(s):  
Basavaraj M. Kalshetty ◽  
R.C. , ◽  
M.C. Sangannavar ◽  
M.B. Kalashetti
Keyword(s):  
Metal Complexes ◽  
Formation Constants
Sign in / Sign up

Export Citation Format

Share Document