Write a balanced net ionic equation for each of the following solution reactions. Refer to Table 14.5 and Appendix D for electrolyte information.

(a) Zn(NO₃)₂(aq) + NaOH(aq) → Zn(OH)₂(s) + NaNO₃(aq)

(b) MgSO₄(aq) + NH₄OH(aq) → Mg(OH)₂(s) + (NH₄)₂SO₄(aq)

Table 14.5

 

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TABLE 14.5 Strong Electrolytes and Weak Electrolytes Strong Electrolytes Strong Acids- hydrochloric acid, HCl(aq) nitric acid, HNO3(aq) sulfuric acid, H₂SO4(aq) perchloric acid, HClO4(aq) Strong Bases- sodium hydroxide, NaOH(aq) potassium hydroxide, KOH(aq) lithium hydroxide, LiOH (aq) calcium hydroxide, Ca(OH)₂(aq) strontium hydroxide, Sr(OH)₂(aq) barium hydroxide, Ba(OH)₂(aq) Soluble Salts- sodium chloride, NaCl(aq) potassium carbonate, K₂CO3(aq) zinc sulfate, ZnSO4(aq) Weak Electrolytes Weak Acids- hydrofluoric acid, HF(aq) nitrous acid, HNO₂(aq) sulfurous acid, H₂SO3(aq) acetic acid, HC₂H₂O₂(aq) carbonic acid, H₂CO3(aq) phosphoric acid, H₂PO4(aq) Weak Bases- ammonium hydroxide, NH₂OH(aq) insoluble hydroxides such as Mg(OH)2(s), Al(OH)3(s), Fe(OH)3(s) Insoluble Salts*- silver chloride, AgCl(s) calcium carbonate, CaCO3(s) barium sulfate, BaSO4(s)