Final answer:
To write a balanced ionic equation for the neutralization of aqueous perchloric acid with aqueous calcium hydroxide, the complete molecular equation is first balanced, then converted to a complete ionic equation, and finally reduced to a net ionic equation by canceling spectator ions.
Step-by-step explanation:
To write a balanced ionic equation for the neutralization of aqueous perchloric acid with aqueous calcium hydroxide, we need to first write the complete molecular equation, then split the soluble compounds into their ions to write the complete ionic equation, and finally cancel the spectator ions to find the net ionic equation.
The unbalanced molecular equation is:
HClO₄(aq) + Ca(OH)₂(aq) → Ca(ClO₄)₂(aq) + H₂O(l)
To balance this, we recognize that two moles of perchloric acid are needed for every mole of calcium hydroxide to form one mole of calcium perchlorate and two moles of water:
2 HClO₄(aq) + Ca(OH)₂(aq) → Ca(ClO₄)₂(aq) + 2 H₂O(l)
The complete ionic equation is then:
2 H⁺(aq) + 2 ClO₄⁻(aq) + Ca²⁺(aq) + 2 OH⁻(aq) → Ca²⁺(aq) + 2 ClO₄⁻(aq) + 2 H₂O(l)
Canceling the spectator ions, we get the net ionic equation:
2 H⁺(aq) + 2 OH⁻(aq) → 2 H₂O(l)
This net ionic equation represents the neutralization reaction between a strong acid and a strong base, producing water.