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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.
Molar concentration (also called molarity, amount concentration or substance concentration) is a measure of the concentration of a chemical species, in particular, of a solute in a solution, in terms of amount of substance per unit volume of solution. In chemistry, the most commonly used unit for molarity is the number of moles per liter ...
In chemistry, the molar absorption coefficient or molar attenuation coefficient (ε) [1] is a measurement of how strongly a chemical species absorbs, and thereby attenuates, light at a given wavelength. It is an intrinsic property of the species. The SI unit of molar absorption coefficient is the square metre per mole (m2/mol), but in practice ...
The solution was initially prepared at 20 °C and then stored for 2 days at 4 °C. In chemistry, solubility is the ability of a substance, the solute, to form a solution with another substance, the solvent. Insolubility is the opposite property, the inability of the solute to form such a solution. The extent of the solubility of a substance in ...
Iron (II) sulfate (British English: iron (II) sulphate) or ferrous sulfate denotes a range of salts with the formula Fe SO 4 · x H 2 O. These compounds exist most commonly as the heptahydrate (x = 7) but several values for x are known. The hydrated form is used medically to treat or prevent iron deficiency, and also for industrial applications.
Complexometric titration (sometimes chelatometry) is a form of volumetric analysis in which the formation of a colored complex is used to indicate the end point of a titration. Complexometric titrations are particularly useful for the determination of a mixture of different metal ions in solution. An indicator capable of producing an ...
The concentration of the solute in a saturated solution is known as the solubility. Units of solubility may be molar (mol dm −3) or expressed as mass per unit volume, such as μg mL −1. Solubility is temperature dependent. A solution containing a higher concentration of solute than the solubility is said to be supersaturated. A ...
The molar conductivity of an electrolyte solution is defined as its conductivity divided by its molar concentration. [1][2] where: c is the molar concentration of the electrolyte. The SI unit of molar conductivity is siemens metres squared per mole (S m 2 mol −1). [2]