What is the net ionic equation of the reaction of MgSO4 with NaOH

To determine the net ionic equation for the reaction between magnesium sulfate (MgSO4) and sodium hydroxide (NaOH), it is necessary to first write out the balanced chemical equation for the reaction.

The balanced chemical equation for the reaction is as follows:

MgSO4 + 2NaOH -> Mg(OH)2 + Na2SO4

To determine the net ionic equation, we first write out the balanced formula equation. Then, we separate the dissociated aqueous ions and eliminate the spectator ions. The remaining ions make up the net ionic equation.

The dissociation of the reactants and products in this reaction are as follows:

MgSO4 (aq) -> Mg2+ (aq) + SO4^2- (aq)
NaOH (aq) -> Na+ (aq) + OH- (aq)
Mg(OH)2 (s) -> Mg2+ (aq) + 2OH- (aq)
Na2SO4 (aq) -> 2Na+ (aq) + SO4^2- (aq)

The spectator ions in this reaction are Na+ and SO4^2-.

Thus, the net ionic equation for the reaction is:

Mg2+ (aq) + 2OH- (aq) -> Mg(OH)2 (s)

To determine the net ionic equation of the reaction between MgSO4 (magnesium sulfate) and NaOH (sodium hydroxide), we first need to write the balanced chemical equation for the reaction.

The chemical equation for the reaction can be written as:

MgSO4 + 2NaOH → Mg(OH)2 + Na2SO4

Next, we can separate the soluble ionic compounds into their respective ions to determine the complete ionic equation:

Mg2+ + SO42- + 2Na+ + 2OH- → Mg(OH)2 + 2Na+ + SO42-

In this equation, the Mg2+ and the SO42- ions are present on both sides of the equation unchanged, and they are referred to as "spectator ions." The sodium ion (Na+) and hydroxide ion (OH-) combine to form the insoluble precipitate magnesium hydroxide (Mg(OH)2).

Finally, we can write the net ionic equation by removing the spectator ions:

Mg2+ + 2OH- → Mg(OH)2

The net ionic equation represents the species that participate directly in the reaction and excludes any spectator ions. In this case, the net ionic equation shows that magnesium ions combine with hydroxide ions to form magnesium hydroxide.

The net ionic equation is the same between Mg ion and OH ion as in the last post. It makes no difference, as long the ions are soluble) what the anion is with Mg or the cation with OH.