Predict the products of the following reaction and write a balanced complete ionic and net ionic...
Question:
Predict the products of the following reaction and write a balanced complete ionic and net ionic equation. Indicate if no reaction occurs.
{eq}NaI(aq)+Hg_2(NO_3)_2(aq) \rightarrow {/eq}
Precipitation Reaction:
When two or more different soluble ionic (salt) compounds are present in the same volume of liquid water, a double displacement reaction can occur. This means that the reactant compounds swap ionic bonds to form two new salt compound products. In some cases one or more of the products formed may be insoluble in water, with such products predicted according to common solubility rules for salt compounds. These insoluble products form precipitates.
Answer and Explanation: 1
Sodium iodide and mercury (I) nitrate are both soluble salt compounds in water. When they are combined in one aqueous mixture the following ion pairs can form:
{eq}NaNO_3 \\ Hg_2I_2 {/eq}
All salt compounds containing sodium cations are highly soluble in water. However most salt compounds containing dimeric mercury (I) cations are insoluble in water, except those with nitrate or acetate anions. Therefore a precipitate reaction will occur, in which mercury (I) iodide is the solid product. Sodium cations and iodide anions are spectators in this process:
{eq}\boxed{\rm ionic: \ 2Na^+ (aq) + 2I^- (aq) + Hg_2^{2+} (aq) + 2NO_3^- (aq) \rightarrow Hg_2I_2 (s) + 2Na^+ (aq) + 2NO_3^- (aq) \\ net-ionic: \ 2I^- (aq) + Hg_2^{2+} (aq) \rightarrow Hg_2I_2 (s) }{/eq}
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Precipitation Reactions: Predicting Precipitates and Net Ionic Equations
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Chapter 10 / Lesson 9
128K
Study precipitate reactions. Determine precipitate solubility according to solubility rules. Learn to write ionic equations by following a molecular reaction.
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