In Thompson's Illustrated Guide to Home Chemistry Experiments the chemical formula for Schweizer's reagent is represented as $\ce{[Cu(NH3)4](OH)2}$ (although Wikipedia represents it as $\ce{[Cu(NH3)4(H2O)2](OH)2}$ ).

Using Thompson's formula, it seems a balanced equation for producing Schweizer's reagent by disolving copper (II) hydroxide in aqueous ammonia would be:

$\ce{Cu(OH)2 (s) + 4 NH3 (aq) -> [Cu(NH3)4](OH)2 (l)}$

This indicates a ratio of 1:4 for copper hydroxide to ammonia.

Is the above balanced equation, and the indicated 1:4 ratio, correct? If not, what might be a correct representation?

(Note: This is a more specific question related to a broader question about Schweizer's reagent production.)

  • $\begingroup$ Yes, but as you can see from what you wrote earlier, it's not like stoichiometric ratio has to be enough, rather contrary. $\endgroup$
    – Mithoron
    Oct 3 '19 at 20:20
  • $\begingroup$ Mithoron, can you elaborate? If the balanced equation is correct and I use a 1:5 ratio, shouldn't all of the copper hydroxide be dissolved? $\endgroup$
    – TwoMice
    Oct 3 '19 at 20:29
  • $\begingroup$ Stoichiometric ratio is 1:4 but it doesn't mean using more will complete reaction. $\endgroup$
    – Mithoron
    Oct 3 '19 at 21:27
  • $\begingroup$ Ahah, you mean because of chemical equilibrium a particular reaction may or may not result in complete consumption of all reactants into products? $\endgroup$
    – TwoMice
    Oct 4 '19 at 5:33

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