Write a balanced net ionic equation for each of the following acidbase reactions. Refer to Table 14.5
Question:
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) HCl(aq) + KOH(aq) → KCl(aq) + H2O(l)
(b) HC2H3O2(aq) + Ca(OH)2(aq) → Ca(C2H3O2)2(aq) + H2O(l)
Table 14.5
Transcribed Image Text:
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)
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Introductory Chemistry Concepts And Critical Thinking
ISBN: 9780321804907
7th Edition
Authors: Charles Corwin
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