What is the thermal stability of potassium phosphate and why?
Thanks.
I assume you mean as a powder, not as an water solution. Potassium phosphate is deliquescent.
At elevated temperatures, phosphorus oxides are released as the compound decomposes.
How elevated? I want to prepare a sample of pure, dry potassium phosphate in my school's lab so I plan to crystallise it then place it in an oven. Will anything happen when I heat it over a bunsen flame during crystallisation?
If you want to prepare a pure sample of tribasic potassium phosphate, The Merck Index gives two references (both in German).
Janecke, Z. Physik. Chem. 2127,75 (1927) OR
Simon, Shultz, Z. Anorg. Allgem. Chem. 242, 331 (1939).
Heating potassium phosphate over a Bunsen flame during crystallization may cause the compound to decompose. As mentioned earlier, at elevated temperatures, phosphorus oxides are released as the compound decomposes. It is important to carefully control the heating process to prevent excessive decomposition.
To determine the thermal stability of potassium phosphate, you can refer to scientific literature or chemical databases like The Merck Index. In this case, there are two references mentioned: Janecke, Z. Physik. Chem. 2127, 75 (1927) and Simon, Shultz, Z. Anorg. Allgem. Chem. 242, 331 (1939). These references provide information regarding the thermal stability of potassium phosphate.
Regarding your plan to crystallize and heat potassium phosphate over a Bunsen flame, it is important to note that potassium phosphate is deliquescent, meaning it absorbs moisture from the air. By heating the compound, you may cause it to lose some of its water content, which can affect its properties. However, heating it over a Bunsen flame during crystallization is generally unlikely to cause any significant reactions or decomposition, as long as you maintain appropriate conditions. However, it is always recommended to carefully follow established procedures and safety guidelines when working with chemicals in a lab setting.