Question

1. write the balanced formula and net ionic equation for the reaction that occurs when the contents of the two beakers are added together. what colors represent the spectator ions in each reaction? a. b. c.

Explanation:

Part a

Balanced formula equation

Step1: Identify reactants

First beaker: \(CuSO_4\) (since there are \(Cu^{2 +}\) and \(SO_4^{2-}\)), second beaker: \(Na_2S\) (since there are \(Na^{+}\) and \(S^{2-}\))

Step2: Write reaction

\(CuSO_4(aq)+Na_2S(aq)\)

Step3: Predict products

Using double - displacement reaction (\(AB + CD
ightarrow AD+CB\)), products are \(CuS(s)\) and \(Na_2SO_4(aq)\)
Balanced formula equation: \(CuSO_4(aq)+Na_2S(aq)=CuS(s)+Na_2SO_4(aq)\)

Net ionic equation

Step1: Write ionic form

\(Cu^{2 +}(aq)+SO_4^{2-}(aq)+2Na^{+}(aq)+S^{2-}(aq)\)

Step2: Identify precipitate

\(CuS\) precipitates (\(CuS(s)\)), \(Na^{+}\) and \(SO_4^{2-}\) are spectator ions
Net ionic equation: \(Cu^{2 +}(aq)+S^{2-}(aq)=CuS(s)\)
Spectator ions: \(Na^{+}\) (grey) and \(SO_4^{2-}\) (light blue)

Part b

Balanced formula equation

Step1: Identify reactants

First beaker: \(CoCl_2\) ( \(Co^{2+}\) and \(Cl^{-}\) ), second beaker: \(NaOH\) ( \(Na^{+}\) and \(OH^{-}\) )

Step2: Write reaction

\(CoCl_2(aq)+NaOH(aq)\)

Step3: Predict products

Using double - displacement, products are \(Co(OH)_2(s)\) and \(NaCl(aq)\)
Balanced formula equation: \(CoCl_2(aq)+2NaOH(aq)=Co(OH)_2(s)+2NaCl(aq)\)

Net ionic equation

Answer:

• a
• Balanced formula: \(CuSO_4(aq)+Na_2S(aq)=CuS(s)+Na_2SO_4(aq)\)
• Net ionic: \(Cu^{2 +}(aq)+S^{2-}(aq)=CuS(s)\)
• Spectator ions: \(Na^{+}\) (grey), \(SO_4^{2-}\) (light blue)
• b
• Balanced formula: \(CoCl_2(aq)+2NaOH(aq)=Co(OH)_2(s)+2NaCl(aq)\)
• Net ionic: \(Co^{2 +}(aq)+2OH^{-}(aq)=Co(OH)_2(s)\)
• Spectator ions: \(Na^{+}\) (grey), \(Cl^{-}\) (green)
• c
• Balanced formula: \(AgNO_3(aq)+KI(aq)=AgI(s)+KNO_3(aq)\)
• Net ionic: \(Ag^{+}(aq)+I^{-}(aq)=AgI(s)\)
• Spectator ions: \(K^{+}\) (red), \(NO_3^{-}\) (blue)