Lithium nitrate is highly soluble in water and also readily dissolves in several polar organic solvents, including ethanol, methanol, pyridine, ammonia, and acetone.
Lithium nitrate (LiNO₃) is an ionic compound known for its strong affinity for polar solvents. Its solubility characteristics make it useful in various chemical applications.
Solubility in Water
Lithium nitrate exhibits remarkable solubility in water, with its dissolution capacity significantly increasing with temperature. This property is common for many ionic salts, as higher temperatures provide more energy to overcome the lattice energy of the crystal and solvate the ions.
The solubility of lithium nitrate in water at different temperatures is detailed below:
| Temperature | Solubility (grams per 100 mL of water) |
|---|---|
| 20 °C (68 °F) | 52.2 g |
| 28 °C (82.4 °F) | 90 g |
| 100 °C (212 °F) | 234 g |
As shown, the solubility more than quadruples when the water temperature increases from 20 °C to 100 °C, making it exceptionally soluble in hot water.
Solubility in Organic Solvents
Beyond water, lithium nitrate is also soluble in a range of polar organic solvents. This indicates its ionic nature allows it to interact favorably with the dipole moments of these molecules. The organic solvents in which lithium nitrate dissolves include:
- Ethanol
- Methanol
- Pyridine
- Ammonia
- Acetone
These solvents, being polar, can effectively solvate the lithium ions (Li⁺) and nitrate ions (NO₃⁻), leading to the dissolution of the salt. This broad solubility profile highlights its versatility in chemical synthesis and laboratory procedures where aqueous solutions may not be suitable.
Understanding the solubility of lithium nitrate is crucial for its applications, from heat transfer fluids to a catalyst component in various reactions. Its high solubility in both aqueous and non-aqueous systems provides flexibility in its use.
