Question

Question #06667

Answer 1

`AgCl + 2NH_4OH -> [Ag(NH_3)_2]Cl + 2H_2O`

Explanation:

The trick here is to realize that ammonium hydroxide, `NH_4OH`, is actually ammonia, `NH_3`, dissolved in water.

`NH_(3(aq)) + H_2O_((l)) rightleftharpoons NH_(4(aq))^(+) + OH_((aq))^(-)`

If you write the complete ionic equation for this reaction, you'll get

`AgCl_((s)) + NH_(3(aq)) + cancel(H_2O_((l))) -> [Ag(NH_3)_2]Cl + cancel(H_2O_((l)))`

The net ionic equation for this reaction is

`AgCl_((s)) + NH_(3(aq)) -> overbrace([Ag(NH_3)_(2(aq))]^(+))^(color(blue)("diamminesilver (I))) + Cl_text((aq])^(-)`

The ammonia reacts with the silver cations to form the diamminesilver (I) metal complex. To balance this equation, simply multiply the ammonia molecules present on the reactants' side by 2.

`AgCl_((s)) + 2NH_(3(aq)) -> [Ag(NH_3)_(2(aq))]^(+) + Cl_text((aq])^(-)`

To get the initial equation balanced, simply multiply `NH_4OH` by 2.

`AgCl + 2NH_4OH -> [Ag(NH_3)_2]Cl + H_2O`

Finally, balance the hydrogen and oxygen atoms by multiplying the water molecule present on the products' side by 2.

`AgCl + 2NH_4OH -> [Ag(NH_3)_2]Cl + 2H_2O`

And that's how the balanced chemical equation looks like.