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This precipitation reaction is used in chlor-alkali plants to control the sulfate concentration in the feed brine for electrolysis. Oxalate effects a similar reaction: BaCl 2 + Na 2 C 2 O 4 → 2 NaCl + BaC 2 O 4. When it is mixed with sodium hydroxide, it gives barium hydroxide, which is moderately soluble in water. BaCl 2 + 2 NaOH → 2 NaCl ...
Strong electrolytes conduct electricity only in aqueous solutions, or in molten salt, and ionic liquid. Strong electrolytes break apart into ions completely. The strength of an electrolyte does not affect the open circuit voltage produced by a galvanic cell. But when electric current flows, stronger electrolytes result in smaller voltage losses ...
The ionic strength of a solution is a measure of the concentration of ions in that solution. Ionic compounds, when dissolved in water, dissociate into ions. The total electrolyte concentration in solution will affect important properties such as the dissociation constant or the solubility of different salts. One of the main characteristics of a ...
An electrolyte in a solution may be described as "concentrated" if it has a high concentration of ions, or "dilute" if it has a low concentration. If a high proportion of the solute dissociates to form free ions, the electrolyte is strong; if most of the solute does not dissociate, the electrolyte is weak.
Conversely, when an ionic liquid is cooled, it often forms an ionic solid—which may be either crystalline or glassy. The ionic bond is usually stronger than the Van der Waals forces between the molecules of ordinary liquids. Because of these strong interactions, salts tend to have high lattice energies, manifested in
In a new Netflix docuseries about Aaron Rodgers, the NFL quarterback laments how fame impacted his life and says the women he dated throughout his career contributed to his celebrity. PEOPLE ...
where z is the ionic charge, and F is the Faraday constant. [9] The limiting molar conductivity of a weak electrolyte cannot be determined reliably by extrapolation. Instead it can be expressed as a sum of ionic contributions, which can be evaluated from the limiting molar conductivities of strong electrolytes containing the same ions.
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