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

(a) HF(aq) + Li₂CO₃(aq) → LiF(aq) + H₂O(l) + CO₂(g) 

(b) H₂SO₄(aq) + Ba(OH)₂(aq) → BaSO₄(s) + H₂O(l)

Table 14.5

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TABLE 14.5 Strong Electrolytes and Weak Electrolytes Strong Electrolytes Weak Electrolytes Strong Acids- Weak 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) 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)