In a given solution, you initially had 5mL of 0.1M MgCl2 in a test tube, then you mixed this with 5mL of 1M NH3 solution. (No reaction from shaking). Then, 1g of NH4Cl was added to this, and what was observed was this solid falling to the surface of the solution and slowly dissolving away.

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anonymous · Answer

In a given solution, you initially had 5mL of 0.1M MgCl2 in a test tube, then you mixed this with 5mL of 1M NH3 solution. (No reaction from shaking). Then, 1g of NH4Cl was added to this, and what was observed was this solid falling to the surface of the solution and slowly dissolving away. =============================================================================== Is there no reaction that occurred after the addition of NH4Cl? The question asks: Explain your observation with respect to the equilibrium reactions that exist in this test tube. The only equilibrium reaction(s) that I can think of from this is NH3 + H2O <=> NH4+ + H3O+, and NH4+ + H2O <=> NH3 + H3O+. I checked the solubility for MgCl2 twice in the textbook and I concluded (from not seeing it anywhere in the solubility constant tables) that it is soluble. Is there any other equilibrium reactions that can be happening be present?