What is the net ionic equation of MgS04 with Sr(N03)2? I get most of the equation right but i think im missing something...
To determine the net ionic equation of the reaction between MgSO4 and Sr(NO3)2, we first need to write the balanced chemical equation of the reaction.
The balanced chemical equation for the reaction between these two compounds is:
MgSO4 + Sr(NO3)2 → Mg(NO3)2 + SrSO4
To write the net ionic equation, we need to identify and exclude any spectator ions that do not participate in the reaction. Spectator ions are ions that remain unchanged throughout the reaction and can be found on both sides of the equation.
In this reaction, the spectator ions are NO3- and Mg2+. Both of these ions are present on both sides of the equation and do not participate in the chemical changes. Therefore, we can exclude them from the net ionic equation.
The net ionic equation for the reaction between MgSO4 and Sr(NO3)2 is:
SO4^2- + Sr^2+ → SrSO4
In this equation, only the sulfate ion (SO4^2-) and the strontium ion (Sr^2+) are shown because they are the only ions involved in the actual chemical reaction.