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ATTACHED

Here's what I get  

Explanation:

1. Molecular equation

3(NH₄)₂CO₃(aq) +2FeCl₃(aq) ⟶ 6NH₄Cl(aq) + Fe₂(CO₃)₃(aq)

2. Ionic equation

You write molecular formulas for the solids, and you write the soluble ionic substances as ions.

6NH₄⁺(aq) + 3CO₃²⁻(aq) + 2Fe³⁺(aq) + 6Cl⁻(aq) ⟶ 6NH₄⁺(aq) + 6Cl⁻(aq) + Fe₂(CO₃)₃(s)

3. Net ionic equation

To get the net ionic equation, you cancel the ions that appear on each side of the ionic equation.

6NH₄⁺(aq) + 3CO₃²⁻(aq) + 2Fe³⁺(aq) + 6Cl⁻(aq) ⟶ 6NH₄⁺(aq) + 6Cl⁻(aq) + Fe₂(CO₃)₃(s)

The net ionic equation is

2Fe³⁺(aq) + 3CO₃²⁻(aq) ⟶ Fe₂(CO₃)₃(s)

the correct answer is b. a strong acid completely dissociates to its ions when dissolved in water. completely dissociates to and ions. a is incorrect because does not fully ionize to and ions and some remain as the compound . c and d are incorrect because, and do not fall into the category of bronsted lowry acids. a bronsted lowry acid is a proton donor and since both molecules do not have a proton to donate they are not bronsted lowry acids. likewise,   if we use the lewis acid definition, they cannot be acids. a lewis acid is an electron pair acceptor. both and have a complete octet so can not accept any electrons which disqualifies them as acids.