do you know ^^effect of ph on metal complex equilibria^^???

ıts my homework and ı didnt find it anywhere

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  • 1 decade ago
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    You will have to look at each individual equation.

    For example, consider the well-known

    [Cu(H2O)6]2+ + 4NH3 <-----> [Cu(NH3)4]2+ + 6H2O.

    You might not think that this was pH dependent from the equation, but adding an acid will make it go to the left. This is because H+ ions react with the free NH3 molecules, lowering their concentration. Le Chatelier's Principle then says that the equilibrium will move to the left to raise their concentration again.

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