Write the complete ionic equation for the reaction BaCl2(aq)and Na2SO4(aq)
This is just a double replacement reactions. Switch the + and - pairs and separate them.
BaCl2(aq)and Na2SO4(aq)
Ba^2+(aq) + 2Cl^-(aq) + 2Na^+(aq) + SO4^2-(aq) ==> BaSO4(s) + 2Na^+(aq) + 2Cl^-(aq)
If you want to convert to the NEW ionic equation, you remove the ions common both sides; i.e., remove the Na^+ and Cl^- on the left and on the right to leave
Ba^2+(aq) + SO4^2-(aq) --> BaSO4(s)
To write the complete ionic equation for the reaction between BaCl2(aq) and Na2SO4(aq), we need to first identify the ions present in each compound.
BaCl2(aq) contains the Ba2+ cation and the Cl- anion.
Na2SO4(aq) contains the Na+ cation and the SO4^2- anion.
Next, we need to determine the products of the reaction. When BaCl2 and Na2SO4 react, a double displacement reaction occurs. Ba2+ will combine with SO4^2- to form BaSO4, a precipitate, while 2 Na+ will combine with 2 Cl- to form NaCl.
Therefore, the complete ionic equation for the reaction is:
Ba2+(aq) + 2 Cl-(aq) + 2 Na+(aq) + SO4^2-(aq) → BaSO4(s) + 2 Na+(aq) + 2 Cl-(aq)
Note that the Na+(aq) and Cl-(aq) ions are spectator ions and do not participate in the actual reaction. They appear on both sides of the equation and can be eliminated to simplify the equation.
The net ionic equation for the reaction is:
Ba2+(aq) + SO4^2-(aq) → BaSO4(s)
In this equation, only the ions directly involved in the reaction are shown, simplifying the equation and focusing on the chemical changes that occur.