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Chapter 8: Problem 25

How should each of the following substances be represented in a total ionic equation? $$\begin{array}{l}{\text { a. } \mathrm{KCl}(a q)} \\ {\text { b. } \mathrm{H}_{2} \mathrm{O}(l)} \\ {\text { c. } \mathrm{Cu}\left(\mathrm{NO}_{3}\right)_{2}(a q)} \\ {\text { d. } \mathrm{AgCl}(s)}\end{array}$$

Short Answer

Expert verified
a. KCl(aq) is represented as K+ (aq) + Cl- (aq)\n b. H2O(l) is represented as H2O(l)\n c. Cu(NO3)2(aq) is represented as Cu2+ (aq) + 2NO3- (aq)\n d. AgCl(s) is represented as AgCl(s)

Step by step solution

01

Representation of KCl(aq)

Potassium chloride or KCl contains potassium (K+) ions and chlorine (Cl-) ions. Since it is in aqueous solution (aq), it dissociates completely into its constituent ions. Therefore, in a full ionic equation, it would be represented as K+ (aq) + Cl- (aq).
02

Representation of H2O(l)

Water or H2O is a liquid and does not ionize in its liquid state. Therefore, it would be represented as H2O(l) in a full ionic equation, and not broken down into its components.
03

Representation of Cu(NO3)2(aq)

Copper(II) nitrate or Cu(NO3)2 is a strong electrolyte and therefore dissociates completely into its constituent ions in an aqueous solution. Thus, it would be represented as Cu2+ (aq) + 2NO3- (aq) in a full ionic equation.
04

Representation of AgCl(s)

Silver chloride or AgCl is a solid and does not dissociate into its ions. Therefore, it would be represented as AgCl(s) in a full ionic equation, not separated into its components.

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