18637-06-4

Upstream product

• 7732-18-5 water 
• 7446-09-5 sulfur dioxide 
• 7440-70-2 calcium 
• 19229-76-6 iron(III) 
• 14336-71-1 calcium chloride 
• 14127-61-8 calcium(II) ion 
• 14280-50-3 lead⁽²⁺⁾ cation 
• 12261-01-7 Ca⁽²⁺⁾*C₆H₆NO₆^(3-)=Ca(C₆H₆NO₆)^(1-) 
• 16397-91-4 manganese(II) 
• 133811-29-7 acetic acid calcium salt 

Downstream Products

• 7790-75-2 calcium tungstate 
• 14127-61-8 ⁽⁴⁰⁾Ca⁽²⁺⁾ 
• 44001-04-9 tetramminecopper(II)⁽²⁺⁾ 
• 12194-71-7 perowskite 
• 156-62-7 calcium cyanamide 

Relevant academic research and scientific papers

Visible light initiated release of calcium ions through photochemical electron transfer reactions

Photolysis of anthraquinone or flavin photosensitizers in the presence of calcium EDTA complexes results in decomposition of the EDTA complex, releasing free Ca2+. In the case of the flavin sensitizers, it is shown that millimolar concentration

Dissolving behavior and calcium release from fibrous wollastonite in acetic acid solution

The degradability of fibrous wollastonite (CaSiO3) in an aqueous solution of acetic acid and leaching of Ca2+ ions were investigated in the temperature range from 22 to 50 °C. The Inductively Coupled Plasma Atomic Emission Spectrosco

Reactions of hydroxylapatites prepared by different procedures with metal ions in aqueous media

Reactions of hydroxylapatites prepared by different procedures with Pb2+, Cr3+, and Fe3+ ions were studied. Depending on the preparation procedure and the nature of the metal, the reaction either occurs through ion exchange or starts as chemisorption and propagates into the sorbent bulk to proceed as a heterogeneous reaction. In the latter case, the metal sorption capacity of hydroxylapatite is much higher.

Chemical and Phase Transformations of Hydroxylapatite in the Course of Lead(II) Sorption from Aqueous Solutions

Sorption of lead(II) on several hydroxylapatite samples was examined. Differences in the preparation conditions resulted in significant differences in the sorptive capacity of the samples (from 0.5 to 10 mg-equiv. Pb2+ per gram hydroxylapatite). It was found that lead sorption on hydroxylapatite is accompanied by complex chemical and phase transformations, the nature of which is responsible for parameters of the sorption process.

Kinetic study of Bi1.8Pb0.4Ca2Sr2Cu3Oy superconductor in water

The reaction of Bi1.8Pb0.4Ca2Sr2Cu3Oy powder in water was studied quantitatively. It was found that the [H3O+] ion would act as a catalyst in this reaction and the initial rate equation was R0 = -d[A]0/dt = k[A]0[H3O+]00.2, where [A] represented the surface area of the superconducting powder. The rate constant, k, obtained at 10, 25 and 40 °C was 3.98, 8.8 and 19.6×10-4 mol min-1 cm-2 M0.8, respectively. The activation energy and pre-exponential factor calculated from the Arrhenius equation were respectively 39.1 kJ mol-1 and 6.4×103 mol min-1 cm-2 M0.8.

Ca2+ ? Pb2+ exchange reaction of calcium silicate hydrate. Ca5Si6O18H2 · 4H2O

Recently it has been demonstrated that synthetic calcium silicate hydrate Ca5Si6O18H2·4H2O shows cation exchange properties. This paper gives the mass balance and thermodynamic data of the Ca2+/

Iron -->/<-- Calcium Ion Exchange Reaction in Cement Hydration Phase, 11 Angstroem Tobermorite

An important phase formed during the hydration reaction of cements is identical with the mineral tobermorite, a calcium silicate hydrate close to Ca5Si6O18H2.4H2O.The crystalline synthetic 11 Angstroem tobermorite undergoes exchage with iron to give tobermorites having 0.93-14.12 wtpercent of Fe when placed in a dilute solution containing initially 100-1800 ppm of Fe(3+) ions at 25 deg C.The equilibrium is reached after 7-10 days.The 3Ca(2+) -->/-- 2Fe(3+) exchage reaction of this calcium silicate hydrate is very much similar to that of clays and zeolites.The free energy of exchange reaction is -498.6 cal/equiv.

Thermodynamics of Calcium-Isotope-Exchange Reactions. 1. Exchange between Isotopic Calcium Carbonates and Aqueous Calcium Ions

This paper reports our results for the direct experimental determination of the equilibrium constant for the calcium-isotope-exchange reaction 40CaCO3(s) + 44CaCl2(aq) 44CaCO3(s) + 40CaCl2(aq).The reaction was studied in electrochemical double cells