Chemistry: The Molecular Science (5th Edition)

Published by Cengage Learning
ISBN 10: 1285199049
ISBN 13: 978-1-28519-904-7

Chapter 3 - Chemical Reactions - Exercise 3.6 - Neutralization and Net Ionic Equations - Page 112: a


Complete ionic equation: $H^+(aq) + Cl^-(aq) + K^+(aq) + OH^-(aq) -- \gt Cl^-(aq) + K^+(aq) + H_2O(l)$ Net ionic equation: $H^+(aq) + OH^-(aq) -- \gt H_2O(l)$

Work Step by Step

1. Identify the salt produced by the mixture of this acid and this base. $HCl$ gives $Cl^-$ after the reaction. $KOH$ gives $K^+$ after the reaction. Therefore, the salt formed is: $KCl$ 2. Write the overall equation: $Acid + Base --\gt Salt + Water$ $HCl(aq) + KOH(aq) -- \gt KCl(aq) + H_2O(l)$ * The equation is already balanced. ** According to table 3.1, KCl is soluble in water. 3. On the totally dissociated/ionized compounds, write the separate ions: $H^+(aq) + Cl^-(aq) + K^+(aq) + OH^-(aq) -- \gt Cl^-(aq) + K^+(aq) + H_2O(l)$ ** HCl is a strong acid, KOH is a strong base, and KCl is a soluble salt. This is the complete ionic equation. 4. Remove the spectators ions: $H^+(aq) + OH^-(aq) -- \gt H_2O(l)$ This is the net ionic equation.
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