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
1. MgCl2 (aq) + Na2CO3 (Aq) MgCO3(s) + 2 NaCl (aq), this is the overall reaction
Total ionic equation is
Mg+2 + 2Cl- + 2Na1 + CO3-2 MgCO3(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 MgCO3(s)
2.
NH3 + HF NH4F
Total ionic equation
NH3 + H + + F- NH4+ + F-
Net ionic equation
NH3 + H + NH4+
3. NH4Cl + NaOH NH3 + NaCl + H2O
(It actually will create NH4OH + NaCl but NH4OH = NH3 + H2O)
total ionic equation
NH4+ + Cl- + Na+ + OH- NH3 + Na+ + Cl- + H2O
Net ionic equation (Remove spectactor ions)
NH4+ + OH- 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) Ba(NO3)2 (aq) + CaCl2 (aq)
the total ionic equation
Ba+2 + 2Cl- + Ca+2 + 2 NO3-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
Interpretation of Reactions by Ionic Type Equations. Aqueous solutions of the following substances or their mixtures...
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