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Compared with pure water, the solubility of an ionic compound is less in aqueous solutions containing a common ion (one also produced by dissolution of the ionic compound). This is an example of a phenomenon known as the common ion effect, which is a consequence of the law of mass action that may be explained using Le Chȃtelier’s principle. Consider the dissolution of silver iodide:
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Few compounds act as strong acids. A far greater number of compounds behave as weak acids and only partially react with water, leaving a large majority of dissolved molecules in their original form and generating a relatively small amount of hydronium ions. Weak acids are commonly encountered in nature, being the substances partly responsible for the tangy taste of citrus fruits, the stinging sensation of insect bites, and the unpleasant smells associated with body odor. A familiar example of a...
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Equilibrium calculations for systems involving multiple equilibria are often complex. For example, to calculate the solubility of a sparingly soluble salt in an aqueous solution in the presence of a common ion, one must consider all the equilibria in this solution. Calculations for these systems can be complicated and tedious, so a systematic approach with a series of steps is often helpful. The process is detailed below.
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The addition of an inert ionic compound increases the solubility of a sparingly soluble salt. For example, adding potassium nitrate to a saturated solution of calcium sulfate significantly enhances the solubility of calcium sulfate. Le Châtelier's principle cannot predict this shift in the equilibrium. Instead, this could be explained in terms of changes in the effective concentration of the ions in solution in the presence of added inert salt.
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When a substance such as sodium chloride is added to water, it dissolves, forming an aqueous solution. The extent of dissolution is called solubility. The process of dissolution can exist in equilibrium, just like other chemical processes. Solubility equilibria are also called precipitation equilibria because the process of solubility can be reversible. The reverse of the solubility process is called precipitation.
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Acid halides are reduced to alcohols in the presence of a strong reducing agent like lithium aluminum hydride.
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Lithium Carbonate Conversion to Lithium Hydroxide Using Calcium Hydroxide: Equilibrium is Governed by Vaterite

Péter Török1, Ilona Halasiné-Varga1, Laurent Duvivier2

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Optimizing lithium hydroxide (LiOH) production requires understanding reaction equilibrium. This study reveals that LiOH yield decreases above a 1.6 mol L-1 threshold and is influenced by calcium carbonate (CaCO3) polymorphs.

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Area of Science:

  • Chemical Engineering
  • Materials Science
  • Electrochemistry

Background:

  • Lithium hydroxide (LiOH) is essential for advanced lithium-ion battery cathodes.
  • The industrial synthesis of LiOH involves converting lithium carbonate (Li2CO3) with calcium hydroxide (Ca(OH)2).
  • Understanding reaction equilibrium and concentration effects is crucial for optimizing LiOH yield.

Purpose of the Study:

  • To investigate the influence of concentration and equilibrium on the Li2CO3-Ca(OH)2 conversion reaction.
  • To determine the maximum LiOH concentration for efficient conversion.
  • To explore the role of solid-phase composition, specifically CaCO3 polymorphs, on reaction thermodynamics.

Main Methods:

  • Systematic variation of Li2CO3 concentration and Ca(OH)2:Li2CO3 molar ratios.
  • Sequential reaction experiments to assess adherence to Le Chatelier's principle.
  • Reverse reaction experiments using LiOH and CaCO3 to establish equilibrium conditions.
  • Analysis of backward reactions involving different CaCO3 polymorphs (calcite and vaterite).

Main Results:

  • Near-complete conversion yields were observed below a 1.6 mol L-1 LiOH concentration threshold.
  • Yields diminished significantly when LiOH concentration exceeded this threshold.
  • The reaction system demonstrated equilibrium behavior consistent with Le Chatelier's principle.
  • Different CaCO3 polymorphs (vaterite and calcite) led to distinct equilibrium states and LiOH concentrations.

Conclusions:

  • The causticization process for LiOH production is concentration-dependent, with an optimal threshold for maximum yield.
  • Solid-phase composition, particularly the presence of vaterite, critically influences the equilibrium thermodynamics of LiOH synthesis.
  • These findings offer insights for optimizing industrial LiOH production processes.