Yes the equation is valid. OH- ligands always seem to substitute H2O ligands.
That pesky OH-...
That pesky OH-...
Original post by Kian Stevens
Yes the equation is valid. OH- ligands always seem to substitute H2O ligands.
That pesky OH-...
That pesky OH-...
But my book show's it forms Al (OH)^-4
When aluminium react with excess ammonia
Original post by Qer
But my book show's it forms Al (OH)^-4
When aluminium react with excess ammonia
When aluminium react with excess ammonia
I don't do the AQA specification so my mileage may vary with this question.
However, reacting with excess ammonia will substitute water ligands for ammonia ligands. Ammonia only acts as a source of OH- ions when it's added dropwise, not in excess.
I can't think of any way how you'd form [Al(OH)4]- from your starting position by reacting with excess ammonia, or anything for that matter.
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