- #1
david18
- 49
- 0
Hi, I carried out a couple of experiments with unknown group 2 salts; X and Y
I added dilute NaOH to each of the salts which were now mixed with 1cm^3 of water; Y formed a precipitate (initially the solution was colourless as the solute had dissolved) whilst X turned colourless (X's solution was initially insoluble and was therefore a ppt before)
What conclusions could I draw from these observations? I think it might have something to do with Y having an ion that is insoluble when added to OH (ie Be and Mg) and vice versa... but I am not too sure...
Another test was adding AgNO3 + nitric acid, and in another I added BaCl2 - what could these show me?
I added dilute NaOH to each of the salts which were now mixed with 1cm^3 of water; Y formed a precipitate (initially the solution was colourless as the solute had dissolved) whilst X turned colourless (X's solution was initially insoluble and was therefore a ppt before)
What conclusions could I draw from these observations? I think it might have something to do with Y having an ion that is insoluble when added to OH (ie Be and Mg) and vice versa... but I am not too sure...
Another test was adding AgNO3 + nitric acid, and in another I added BaCl2 - what could these show me?