Question

Interpretation of Reactions by Ionic Type Equations. Aqueous solutions of the following substances
or their mixtures with water if they are only slightly soluble, are mixed. Write first the
conventional equation, second the total ionic equation, and lastly the net ionic equation. If you
predict no appreciable reaction, indicate this, and state why.
a. Magnesium chloride and sodium carbonate

b.Aqueous ammonia and hydrofluoric acid

c.Aqueous ammonia and hydrofluoric acid

d.Ammonium chloride and sodium hydroxide

e.Barium chloride and calcium nitrate

f.Potassium hydrogen carbonate and sulfuric acid
g.Aluminum hydroxide and nitric acid

Answer 1

1. MgCl_{2 (aq)} + Na₂CO_{3 (Aq)} $\rightarrow$ MgCO_3(s) + 2 NaCl (aq), this is the overall reaction

Total ionic equation is

Mg⁺² + 2Cl^- + 2Na¹ + CO₃^-2 $\rightarrow$ MgCO_3(s) + 2Na⁺¹ + 2Cl^-, the MgCO₃ is not splitted into cations because it is solid

Net ionic equation

This is to remove the spectator ions, the ones that are on every side of the equation unchanged

Mg⁺² + CO₃^-2 $\rightarrow$ MgCO_3(s)

2.

NH₃ + HF $\rightarrow$ NH₄F

Total ionic equation

NH₃ + H ⁺ + F^- $\rightarrow$ NH₄⁺ + F^-

Net ionic equation

NH₃ + H ⁺   $\rightarrow$ NH₄⁺

3. NH4Cl + NaOH $\rightarrow$ NH₃ + NaCl + H₂O

(It actually will create NH4OH + NaCl but NH4OH = NH3 + H2O)

total ionic equation

NH₄⁺ + Cl^- + Na⁺ + OH^- $\rightarrow$ NH₃ + Na⁺ + Cl^- + H₂O

Net ionic equation (Remove spectactor ions)

NH₄⁺  + OH^- $\rightarrow$ NH₃ + H₂O

4. This reaction is not going to occur because if we want these compounds to react we will just be getting 2 soluble compounds , this is that all the ions will be spectator ions that move freely in the solution, if we try to write a equation

BaCl₂ (aq) + Ca(NO₃)_{2 (aq)} $\rightarrow$ Ba(NO₃)_{2 (aq)} + CaCl_{2 (aq)}

the total ionic equation

Ba⁺² + 2Cl^- + Ca⁺² + 2 NO₃^- $\rightarrow$ Ba⁺² + 2 NO₃^-+ Ca⁺² + 2Cl^-

There is no net ionic equation because all the ions are spectors, they don´t really participate in a reaction