give the full, ionic and net equations for the reaction (if any) that occurs when aqueous soulutions of Na2CO3 and MgCl2 are mixed.
http://chemistry.bd.psu.edu/jircitano/soluble.html
To determine the full, ionic, and net equations for the reaction between aqueous sodium carbonate (Na2CO3) and magnesium chloride (MgCl2), we need to consider the possible reactions between their ions.
First, let's break down the compounds into their respective ions:
- Sodium carbonate (Na2CO3) dissociates into two sodium ions (Na+) and one carbonate ion (CO3^2-).
- Magnesium chloride (MgCl2) dissociates into one magnesium ion (Mg^2+) and two chloride ions (Cl-).
Now, let's write the possible full ionic equation by combining the ions from the reactants:
2Na+(aq) + CO3^2-(aq) + Mg^2+(aq) + 2Cl-(aq) → 2Na+(aq) + 2Cl-(aq) + MgCO3(s)
In this equation, the two sodium ions and two chloride ions remain as aqueous (aq), while the carbonate ion combines with the magnesium ion to form solid magnesium carbonate (MgCO3).
Next, let's write the ionic equation by breaking down the reactants and products into their individual ions (specifying their states):
2Na+(aq) + CO3^2-(aq) + Mg^2+(aq) + 2Cl-(aq) → 2Na+(aq) + 2Cl-(aq) + MgCO3(s)
Finally, let's simplify the equation by canceling out the common ions that are the same on both sides of the equation, resulting in the net ionic equation:
CO3^2-(aq) + Mg^2+(aq) → MgCO3(s)
So, the full equation is 2Na+(aq) + CO3^2-(aq) + Mg^2+(aq) + 2Cl-(aq) → 2Na+(aq) + 2Cl-(aq) + MgCO3(s).
The ionic equation is the same as the full equation: 2Na+(aq) + CO3^2-(aq) + Mg^2+(aq) + 2Cl-(aq) → 2Na+(aq) + 2Cl-(aq) + MgCO3(s).
And the net ionic equation is CO3^2-(aq) + Mg^2+(aq) → MgCO3(s).