Write the balanced net ionic equations for the reactions that occur in each of the following cases. Identify the spectator ion or ions in each reaction.
a. Cr2(SO4)3(aq) + 3(NH4)2CO3 (aq) =====? Cr2(CO3)3 ( s) + 3(NH4)2SO4 ( aq)
b. Ba(NO3)2 (aq)+ k2SO4(aq)======?BaSO4(s) + 2KNO3(aq)
c. Fe(NO3)2 (aq) + 2KOH(aq)=====?2KNO3(aq) + Fe(OH)2 (s)
The Correct Answer and Explanation is :
Let’s break down each of the reactions step by step and determine the balanced net ionic equations.
a. Cr₂(SO₄)₃(aq) + 3(NH₄)₂CO₃(aq) → Cr₂(CO₃)₃(s) + 3(NH₄)₂SO₄(aq)
- Write the full ionic equation: The ionic compounds will dissociate into their respective ions. [
Cr_2(SO_4)_3 (aq) \rightarrow 2Cr^{3+}(aq) + 3SO_4^{2-}(aq)
]
[
(NH_4)_2CO_3 (aq) \rightarrow 2NH_4^+(aq) + CO_3^{2-}(aq)
] When combined, we get: [
2Cr^{3+}(aq) + 3SO_4^{2-}(aq) + 6NH_4^+(aq) + 3CO_3^{2-}(aq) \rightarrow Cr_2(CO_3)_3 (s) + 6NH_4^+(aq) + 3SO_4^{2-}(aq)
] - Cancel out spectator ions: The ammonium ion (NH₄⁺) and sulfate ion (SO₄²⁻) are spectator ions because they appear on both sides of the equation.
- Net ionic equation: After removing the spectator ions, the balanced net ionic equation is: [
2Cr^{3+}(aq) + 3CO_3^{2-}(aq) \rightarrow Cr_2(CO_3)_3(s)
]
b. Ba(NO₃)₂(aq) + K₂SO₄(aq) → BaSO₄(s) + 2KNO₃(aq)
- Write the full ionic equation: [
Ba(NO_3)_2 (aq) \rightarrow Ba^{2+}(aq) + 2NO_3^-(aq)
]
[
K_2SO_4 (aq) \rightarrow 2K^+(aq) + SO_4^{2-}(aq)
] Combining the ions, we get: [
Ba^{2+}(aq) + 2NO_3^-(aq) + 2K^+(aq) + SO_4^{2-}(aq) \rightarrow BaSO_4(s) + 2K^+(aq) + 2NO_3^-(aq)
] - Cancel out spectator ions: Potassium (K⁺) and nitrate (NO₃⁻) ions are spectator ions.
- Net ionic equation: After canceling the spectator ions, the net ionic equation is: [
Ba^{2+}(aq) + SO_4^{2-}(aq) \rightarrow BaSO_4(s)
]
c. Fe(NO₃)₂(aq) + 2KOH(aq) → 2KNO₃(aq) + Fe(OH)₂(s)
- Write the full ionic equation: [
Fe(NO_3)_2 (aq) \rightarrow Fe^{2+}(aq) + 2NO_3^-(aq)
]
[
KOH (aq) \rightarrow K^+(aq) + OH^-(aq)
] Combining the ions, we get: [
Fe^{2+}(aq) + 2NO_3^-(aq) + 2K^+(aq) + 2OH^-(aq) \rightarrow 2KNO_3(aq) + Fe(OH)_2(s)
] - Cancel out spectator ions: Potassium (K⁺) and nitrate (NO₃⁻) ions are spectator ions.
- Net ionic equation: After removing the spectator ions, the balanced net ionic equation is: [
Fe^{2+}(aq) + 2OH^-(aq) \rightarrow Fe(OH)_2(s)
]
Explanation:
- In each case, the ionic compounds dissociate in solution to form ions.
- The spectator ions (those that don’t participate in the actual reaction) are then removed, leaving only the ions that form the precipitate or product.
- The net ionic equations represent the actual chemical change occurring in the reaction.
Let me generate the image of these ionic equations for you.
Here is the infographic displaying the three reactions with their full ionic and net ionic equations. It shows the dissociation of ions, the spectator ions, and the final balanced net ionic equations. Let me know if you’d like further details or have any questions!
