How do you quench TiCl4?
Thereof, is TiCl4 soluble in water?
|Melting point||−24.1 °C (−11.4 °F; 249.1 K)|
|Boiling point||136.4 °C (277.5 °F; 409.5 K)|
|Solubility in water||reacts (exothermic hydrolysis)|
|Solubility||soluble in dichloromethane, toluene, pentane|
Furthermore, why TiCl4 is a strong Lewis acid? It can act as a Lewis acid since it will accept electrons to satisfy its electron deficiency. In fact, it has a +4 charge, so it significantly more electron deficient than a species with a lower positive charge. Thus, it is a very strong Lewis acid that will readily accept electrons from a Lewis base.
Also question is, is TiCl4 polar or nonpolar?
It is non-polar and is soluble in/compatible with benzene and chlorinated solvents. I recently used TiCl4 in an attempt to catalyze a reaction.
How will you prepare TiCl4?
A method for preparing titanium tetrachloride is described which consists of reducing rutile with coke and chlorinating the reduced product at 200° to 500°C. The crude distillate is purified by treatment with copper powder and distillation.