Question

Write the balanced NET ionic equation for the reaction when AlCl₃ and NaOH are mixed in aqueous solution. If no reaction occurs, write only NR.

Answer 1

Answer:

$Al^{3+} + 3OH^{-} ---> Al(OH)_{3}$

Explanation:

AlCl3 + 3NaOH ---> Al(OH)3 + 3NaCl

$Al^{3+} +3Cl^{-} +3Na^{+}+3OH^{-}--->AL(OH)_{3}+3Na^{+}+3OH^{-}\\\\Al^{3+} + 3OH^{-} ---> Al(OH)_{3}$

Answer 2

The balanced NET ionic equation for the reaction when AlCl₃ and NaOH are mixed in an aqueous solution is:

Al³⁺(aq) + 3OH⁻(aq) → Al(OH)₃(s)

The reaction between AlCl₃ and NaOH is an exchange reaction:

AlCl₃(aq) + 3NaOH(aq) → Al(OH)₃(s) + 3NaCl(aq)   (1)

In this reaction, the ions Cl⁻ and OH⁻ are exchanged between the ions Al⁺³ and Na⁺.  

To write the NET ionic equation, we need to write the total ionic equation:

Al³⁺(aq) + 3Cl⁻(aq) + 3Na⁺(aq) + 3OH⁻(aq) → Al(OH)₃(s) + 3Na⁺(aq) + 3Cl⁻(aq)   (2)

Since the Al(OH)₃ precipitates, we cannot write it as an ion because it does not dissociate in the aqueous solution.  

The net ionic equation of reaction (2) is the following:

Al³⁺(aq) + 3OH⁻(aq) → Al(OH)₃(s)   (3)

All repeated ions in reactants and products do not participate in the net ionic equation. That is why we canceled the Na⁺ and Cl⁻ ions in the net ionic equation (eq 3).

Therefore, the balanced net ionic equation is:

Al³⁺(aq) + 3OH⁻(aq) → Al(OH)₃(s)

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