Search results
Results From The WOW.Com Content Network
Caesium sulfate or cesium sulfate is the inorganic compound and salt with the formula Cs 2 SO 4. It is a white water-soluble solid that is used to prepare dense aqueous solutions for use in isopycnic (or "density-gradient") centrifugation. It is isostructural with potassium salt. [3]
C. Caesium acetate; Caesium auride; Caesium azide; Caesium bicarbonate; Caesium bisulfate; Caesium bromide; Caesium cadmium bromide; Caesium cadmium chloride
Material & heterostructure used for the characterization (electrodes/material, electrode/substrate) Orientation Piezoelectric coefficients, d (pC/N) Relative permittivity, ε r Electromechanical coupling factor, k Quality factor Berlincourt et al. 1958 [30] BaTiO 3: d 15 = 270 ε 11 = 1440 k 15 = 0.57 d 31 = -79 ε 33 = 1680 k 31 = 0.49 d 33 ...
Caesium vapour is used in many common magnetometers. [91] The element is used as an internal standard in ... caesium sulfate, and caesium trifluoroacetate (Cs(O
caesium hydrogen sulfate: 7789-16-4 Cs 2 C 2 O 4: caesium oxalate: 1068-63-9 Cs 2 CrO 4: caesium chromate: 13454-78-9 Cs 2 Cr 2 O 7: caesium dichromate: 13530-67-1 Cs 2 HPO 4: caesium hydrogen orthophosphate: Cs 2 MoO 4: caesium molybdate: 13597-64-3 Cs 2 O: caesium oxide: 20281-00-9 Cs 2 SO 3: caesium sulfite: Cs 2 SO 4: caesium sulfate: 10294 ...
[23] 140 Ce is the most common isotope of cerium, as it can be produced in both the s- and r-processes, while 142 Ce can only be produced in the r-process. Another reason for the abundance of 140 Ce is that it is a magic nucleus , having a closed neutron shell (it has 82 neutrons), and hence it has a very low cross section towards further ...
The following chart shows the solubility of various ionic compounds in water at 1 atm pressure and room temperature (approx. 25 °C, 298.15 K). "Soluble" means the ionic compound doesn't precipitate, while "slightly soluble" and "insoluble" mean that a solid will precipitate; "slightly soluble" compounds like calcium sulfate may require heat to precipitate.
Metals in the middle of the reactivity series, such as iron, will react with acids such as sulfuric acid (but not water at normal temperatures) to give hydrogen and a metal salt, such as iron(II) sulfate: Fe (s) + H 2 SO 4 (l) → FeSO 4 (aq) + H 2 (g) There is some ambiguity at the borderlines between the groups.