Give the complete ionic equation for the reaction (if any) that occurs when aqueous solutions of MgSO3 and HI are mixed
SO3^2-(aq) + 2H^+(aq) ==> H2SO3(aq)
To determine the complete ionic equation for the reaction between aqueous solutions of MgSO3 and HI, let's first write the balanced molecular equation:
MgSO3(aq) + 2HI(aq) → MgSO4(aq) + H2O(l) + I2(g)
Now, let's break down the aqueous compounds into their ionic components:
Mg2+(aq) + SO3^2-(aq) + 2H+(aq) + 2I-(aq) → Mg2+(aq) + SO4^2-(aq) + H2O(l) + I2(g)
Since both the Mg2+ and SO4^2- ions remain unchanged on both sides of the equation, they are considered spectator ions and can be removed from the equation:
SO3^2-(aq) + 2H+(aq) + 2I-(aq) → H2O(l) + I2(g)
Therefore, the complete ionic equation for the reaction would be:
SO3^2-(aq) + 2H+(aq) + 2I-(aq) → H2O(l) + I2(g)
To determine the complete ionic equation for the reaction between aqueous solutions of MgSO3 and HI, we need to first write down the balanced molecular equation and then break down the soluble ionic compounds into their respective ions.
1. Start by writing the balanced molecular equation:
MgSO3(aq) + 2HI(aq) → MgI2(aq) + H2SO3(aq)
2. Now, let's break down the soluble ionic compounds into their ions:
MgSO3(aq) dissociates into Mg2+(aq) + SO3^2-(aq)
HI(aq) dissociates into H+(aq) + I-(aq)
MgI2(aq) dissociates into Mg2+(aq) + 2I-(aq)
H2SO3(aq) does not dissociate further as it is a weak acid.
3. Write down the complete ionic equation by including all the dissociated ions:
Mg2+(aq) + SO3^2-(aq) + 2H+(aq) + 2I-(aq) → Mg2+(aq) + 2I-(aq) + H2SO3(aq)
4. Finally, eliminate the spectator ions (ions that appear on both sides of the equation and do not participate in the reaction):
The Mg2+ and I- ions appear on both sides of the equation. Therefore, they are spectator ions and can be eliminated.
The simplified ionic equation is:
SO3^2-(aq) + 2H+(aq) → H2SO3(aq)
So, the complete ionic equation for the reaction between aqueous solutions of MgSO3 and HI is:
SO3^2-(aq) + 2H+(aq) → H2SO3(aq)