Asked by Amanda
What is the balanced net ionic equation for magnesium metal being placed in a solution of gold(3) chloride ?(with steps please)
Answers
Answered by
DrBob222
Balanced molecular equation.
2AuCl3(aq) + 3Mg(s) ==> 3MgCl2(aq) + 2Au(s)
To convert to ionic.
1. gases remain as molecules
2. solids remain as molecules
3. strong electrolytes are displayed as ions.
4. weak electrolytes remain as molecules.
From above, AuCl3 will be split.
Mg remains as is
MgCl2 is split
etc.
2Au^2+(aq) + 6Cl^-(aq) + 3Mg(s) ==> 3Mg^2+(aq) + 6Cl^-(aq) + 2Au(s)
To convert from the full ionic equation to the net ionic equation, cancel anything common to both sides; i.e., the 6Cl- will cancel on each side but nothing else will. So you are left with this as the net ionic equation.
2Au^3+(aq) + 3Mg(s) ==> 3Mg^2+(aq) + 2Au(s)
2AuCl3(aq) + 3Mg(s) ==> 3MgCl2(aq) + 2Au(s)
To convert to ionic.
1. gases remain as molecules
2. solids remain as molecules
3. strong electrolytes are displayed as ions.
4. weak electrolytes remain as molecules.
From above, AuCl3 will be split.
Mg remains as is
MgCl2 is split
etc.
2Au^2+(aq) + 6Cl^-(aq) + 3Mg(s) ==> 3Mg^2+(aq) + 6Cl^-(aq) + 2Au(s)
To convert from the full ionic equation to the net ionic equation, cancel anything common to both sides; i.e., the 6Cl- will cancel on each side but nothing else will. So you are left with this as the net ionic equation.
2Au^3+(aq) + 3Mg(s) ==> 3Mg^2+(aq) + 2Au(s)
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