how can magnesium chloride be lost in a reaction and how can we ensure that it is pure?
Magnesium chloride (MgCl2) can be lost in a reaction through a few different mechanisms. Let's explore two common ways this could happen:
1. Volatility: Magnesium chloride can evaporate or sublimate if the reaction conditions promote high temperatures or low pressures. This loss can occur mainly in open systems or when the reaction is conducted at elevated temperatures.
2. Solubility: Magnesium chloride is highly soluble in water. If the reaction involves an aqueous environment and magnesium chloride is produced, there is a possibility that it could dissolve and be lost in the resulting solution.
To ensure the purity of magnesium chloride, you can take the following steps:
1. Utilize a closed system: Minimize exposure to high temperatures and low pressures to prevent the loss of magnesium chloride due to volatility. By sealing the reaction vessel, you can prevent the escape of any volatile substances, including magnesium chloride.
2. Control environmental conditions: By conducting the reaction under specific temperature and pressure conditions, you can minimize the chance of magnesium chloride loss. Lower temperatures and higher pressures typically reduce the volatility of substances.
3. Recover magnesium chloride from the reaction solution: If the magnesium chloride produced dissolves in a reaction solution, you can recover it by evaporating the solvent. This process is known as "drying" or "desiccation." Once the solvent is evaporated, magnesium chloride can be collected as a solid residue.
4. Purification techniques: Additional purification steps can be employed to ensure the purity of magnesium chloride. For example, filtration or recrystallization can help remove impurities or separate magnesium chloride from other byproducts, yielding a more refined product.
Remember, good laboratory practices, such as proper handling, accurate measurements, and careful observation of reaction conditions, are critical to ensuring the purity and availability of magnesium chloride during a reaction.