## Chemistry: The Central Science (13th Edition)

Published by Prentice Hall

# Chapter 4 - Reactions in Aqueous Solution - Exercises: 4.39b

#### Answer

Balanced: $Cu(OH)2(s)+2HClO_4(aq)→Cu(ClO_4)_2(aq)+2H2O(l)$ Net Ionic Equation: $Cu(OH)_2 (s) + 2H^+ (aq) \rightarrow Cu^{2+} (aq) + 2H_2O (l)$

#### Work Step by Step

Recall that ionic compounds ionize in aqueuous solutions and have a charge. Given molecular equation: $Cu(OH)_2(s) + HClO_4(aq) \rightarrow$ Balanced: $Cu(OH)_2(s) + 2HClO_4(aq) \rightarrow Cu(ClO_4)_2 (aq) + 2H_2O (l)$ The net ionic: equation can be found by separating compounds into cations and anions (we are looking for dissociation). Only ionic compounds with high solubility will ionize. $Cu(OH)_2 (s) + 2H^+(sq) +2ClO_4^- \rightarrow Cu^{2+} (aq) + 2ClO_4^- (aq) + 2H_2O (l)$ $ClO_4$ can be cancelled of because it is a spectator ion appearing on both sides of the equation $Cu(OH)_2 (s) + 2H^+ (aq) \rightarrow Cu^{2+} (aq) + 2H_2O$

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