Questions: What is the net ionic equation for each of the following reactions? Note: Reference the Solubility of ionic compounds in water table for additional information. Part 1 of 2 Al(s) + HCl(aq) → Part 2 of 2 AgNO3(aq) + H3PO4(aq) →

What is the net ionic equation for each of the following reactions?
Note: Reference the Solubility of ionic compounds in water table for additional information.

Part 1 of 2
Al(s) + HCl(aq) →

Part 2 of 2
AgNO3(aq) + H3PO4(aq) →

Transcript text: What is the net ionic equation for each of the following reactions? Note: Reference the Solubility of ionic compounds in water table for additional information. Part 1 of 2 \[ \mathrm{Al}(s)+\mathrm{HCl}(a q) \rightarrow \] $\square$ Part 2 of 2 \[ \mathrm{AgNO}_{3}(a q)+\mathrm{H}_{3} \mathrm{PO}_{4}(a q) \rightarrow \] $\square$

Solution

Solution Steps

Step 1: Determine the Reaction for Part 1

The reaction involves solid aluminum ($\mathrm{Al}(s)$) and hydrochloric acid ($\mathrm{HCl}(aq)$). Aluminum reacts with hydrochloric acid to produce aluminum chloride and hydrogen gas. The balanced chemical equation is:

\[ 2\mathrm{Al}(s) + 6\mathrm{HCl}(aq) \rightarrow 2\mathrm{AlCl}_3(aq) + 3\mathrm{H}_2(g) \]

Step 2: Write the Ionic Equation for Part 1

In aqueous solution, $\mathrm{HCl}$ dissociates into $\mathrm{H}^+$ and $\mathrm{Cl}^-$ ions, and $\mathrm{AlCl}_3$ dissociates into $\mathrm{Al}^{3+}$ and $\mathrm{Cl}^-$ ions. The ionic equation is:

\[ 2\mathrm{Al}(s) + 6\mathrm{H}^+(aq) + 6\mathrm{Cl}^-(aq) \rightarrow 2\mathrm{Al}^{3+}(aq) + 6\mathrm{Cl}^-(aq) + 3\mathrm{H}_2(g) \]

Step 3: Write the Net Ionic Equation for Part 1

Cancel out the spectator ions ($\mathrm{Cl}^-$) that appear on both sides of the equation:

\[ 2\mathrm{Al}(s) + 6\mathrm{H}^+(aq) \rightarrow 2\mathrm{Al}^{3+}(aq) + 3\mathrm{H}_2(g) \]

Step 4: Determine the Reaction for Part 2

The reaction involves silver nitrate ($\mathrm{AgNO}_3(aq)$) and phosphoric acid ($\mathrm{H}_3\mathrm{PO}_4(aq)$). Silver phosphate ($\mathrm{Ag}_3\mathrm{PO}_4$) is insoluble in water and will precipitate. The balanced chemical equation is:

\[ 3\mathrm{AgNO}_3(aq) + \mathrm{H}_3\mathrm{PO}_4(aq) \rightarrow \mathrm{Ag}_3\mathrm{PO}_4(s) + 3\mathrm{HNO}_3(aq) \]

Step 5: Write the Ionic Equation for Part 2

In aqueous solution, $\mathrm{AgNO}_3$ dissociates into $\mathrm{Ag}^+$ and $\mathrm{NO}_3^-$ ions, and $\mathrm{H}_3\mathrm{PO}_4$ dissociates into $\mathrm{H}^+$ and $\mathrm{PO}_4^{3-}$ ions. The ionic equation is:

\[ 3\mathrm{Ag}^+(aq) + 3\mathrm{NO}_3^-(aq) + 3\mathrm{H}^+(aq) + \mathrm{PO}_4^{3-}(aq) \rightarrow \mathrm{Ag}_3\mathrm{PO}_4(s) + 3\mathrm{H}^+(aq) + 3\mathrm{NO}_3^-(aq) \]

Step 6: Write the Net Ionic Equation for Part 2

Cancel out the spectator ions ($\mathrm{NO}_3^-$ and $\mathrm{H}^+$) that appear on both sides of the equation:

\[ 3\mathrm{Ag}^+(aq) + \mathrm{PO}_4^{3-}(aq) \rightarrow \mathrm{Ag}_3\mathrm{PO}_4(s) \]

Final Answer

Part 1: $\boxed{2\mathrm{Al}(s) + 6\mathrm{H}^+(aq) \rightarrow 2\mathrm{Al}^{3+}(aq) + 3\mathrm{H}_2(g)}$
Part 2: $\boxed{3\mathrm{Ag}^+(aq) + \mathrm{PO}_4^{3-}(aq) \rightarrow \mathrm{Ag}_3\mathrm{PO}_4(s)}$

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