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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.
At higher temperatures, the Al 2 Cl 6 dimers dissociate into trigonal planar AlCl 3 monomer, which is structurally analogous to BF 3. The melt conducts electricity poorly, [12] unlike more ionic halides such as sodium chloride. Aluminium chloride monomer belongs to the point group D 3h in its monomeric form and D 2h in its dimeric form.
The chart shows solubility curves for some typical solid inorganic salts in liquid water (temperature is in degrees Celsius, i.e. kelvins minus 273.15). [14] Many salts behave like barium nitrate and disodium hydrogen arsenate, and show a large increase in solubility with temperature (ΔH > 0).
Phase behavior Triple point? K (? °C), ? Pa Critical point: 625.7 K (352.6 °C), 2.600 MPa Std enthalpy change of fusionΔ fus H o? kJ/mol Std entropy change
b c is the colligative molality, calculated by taking dissociation into account since the boiling point elevation is a colligative property, dependent on the number of particles in solution. This is most easily done by using the van 't Hoff factor i as b c = b solute · i , where b solute is the molality of the solution. [ 3 ]
Here i is the van 't Hoff factor as above, K b is the ebullioscopic constant of the solvent (equal to 0.512 °C kg/mol for water), and m is the molality of the solution. The boiling point is the temperature at which there is equilibrium between liquid and gas phases.
Solubility equilibrium is a type of dynamic equilibrium that exists when a chemical compound in the solid state is in chemical equilibrium with a solution of that compound. The solid may dissolve unchanged, with dissociation, or with chemical reaction with another constituent of the solution, such as acid or alkali.
Simply because a substance does not readily dissolve does not make it a weak electrolyte. Acetic acid (CH 3 COOH) and ammonium (NH + 4) are good examples. Acetic acid is extremely soluble in water, but most of the compound dissolves into molecules, rendering it a weak electrolyte. Weak bases and weak acids are generally weak electrolytes.