Question

Write the balanced net ionic equation for the reactions that occur when the given aqueous solutions are mixed. Include the physical states. A. silver nitrate, AgNO 3 AgNO3 , and magnesium bromide, MgBr 2 MgBr2 net ionic equation: B. perchloric acid, HClO 4 HClO4 , and potassium hydroxide, KOH KOH net ionic equation: C. ammonium sulfide, ( NH 4 ) 2 S (NH4)2S , and cobalt(II) chloride, CoCl 2 CoCl2 net ionic equation:

Answer 1

Answer : The balanced net ionic equation for the reactions are:

(A) $2Ag^{+}(aq)+2Br^{-}(aq)\rightarrow AgBr(s)$

(B) $H^{+}(aq)+OH^{-}(aq)\rightarrow H_2O(l)$

(C) $Co^{2+}(aq)+S^{2-}(aq)\rightarrow CoS(s)$

Explanation :

Complete ionic equation : In complete ionic equation, all the substance that are strong electrolyte and present in an aqueous are represented in the form of ions.

Net ionic equation : In the net ionic equations, we are not include the spectator ions in the equations.

Spectator ions : The ions present on reactant and product side which do not participate in a reactions. The same ions present on both the sides.

Part A :

The balanced molecular equation will be,

$2AgNO_3(aq)+MgBr_2(aq)\rightarrow Mg(NO_3)_2(aq)+2AgBr(s)$

The complete ionic equation in separated aqueous solution will be,

$2Ag^+(aq)+2NO_3^{-}(aq)+Mg^{2+}(aq)+2Br^{-}(aq)\rightarrow Mg^{2+}(aq)+2NO_3^{-}(aq)+2AgBr(s)$

In this equation the species $Mg^{2+}\text{ and }NO_3^-$ are the spectator ions.

By removing the spectator ions from the balanced ionic equation, we get the net ionic equation.

The net ionic equation will be,

$2Ag^{+}(aq)+2Br^{-}(aq)\rightarrow AgBr(s)$

Part B :

The balanced molecular equation will be,

$HClO_4(aq)+KOH(aq)\rightarrow H_2O(l)+KClO_4(aq)$

The complete ionic equation in separated aqueous solution will be,

$H^+(aq)+ClO_4^{-}(aq)+K^{+}(aq)+OH^{-}(aq)\rightarrow K^{+}(aq)+CLO_4^{-}(aq)+H_2O(l)$

In this equation the species $K^{+}\text{ and }ClO_4^-$ are the spectator ions.

By removing the spectator ions from the balanced ionic equation, we get the net ionic equation.

The net ionic equation will be,

$H^{+}(aq)+OH^{-}(aq)\rightarrow H_2O(l)$

Part C :

The balanced molecular equation will be,

$(NH_4)_2S(aq)+CoCl_2(aq)\rightarrow 2NH_4Cl(aq)+CoS(s)$

The complete ionic equation in separated aqueous solution will be,

$2NH_4^+(aq)+S^{2-}(aq)+Co^{2+}(aq)+2Cl^{-}(aq)\rightarrow 2NH_4^{+}(aq)+2Cl^{-}(aq)+CoS(s)$

In this equation the species $NH_4^{+}\text{ and }Cl^-$ are the spectator ions.

By removing the spectator ions from the balanced ionic equation, we get the net ionic equation.

The net ionic equation will be,

$Co^{2+}(aq)+S^{2-}(aq)\rightarrow CoS(s)$

Answer 2

The balanced net ionic equations are:

• A. Ag⁺(aq) + Br⁻(aq) ⇒ AgBr(s)
• B. H⁺(aq) + OH⁻(aq) ⇒ H₂O(l)
• C. NH₄⁺(aq) + Cl⁻(aq) ⇒ NH₄Cl(s)

We want to write the balanced net ionic equations for the reactions that occur when the given aqueous solutions are mixed.

What is a net ionic equation?

A chemical equation in which only those ions undergoing chemical changes during the course of the reaction are represented.

A. silver nitrate, AgNO₃, and magnesium bromide, MgBr₂.

Ag⁺(aq) + Br⁻(aq) ⇒ AgBr(s)

NO₃⁻ and Mg²⁺ are not in the net ionic equation because they are spectator ions.

B. perchloric acid, HClO₄, and potassium hydroxide, KOH.

H⁺(aq) + OH⁻(aq) ⇒ H₂O(l)

ClO₄⁻ and K⁺ are not in the net ionic equation because they are spectator ions.

C. ammonium sulfide, (NH₄)₂S, and cobalt(II) chloride, CoCl₂

NH₄⁺(aq) + Cl⁻(aq) ⇒ NH₄Cl(s)

S²⁻ and Co²⁺ are not in the net ionic equation because they are spectator ions.

The balanced net ionic equations are:

• A. Ag⁺(aq) + Br⁻(aq) ⇒ AgBr(s)
• B. H⁺(aq) + OH⁻(aq) ⇒ H₂O(l)
• C. NH₄⁺(aq) + Cl⁻(aq) ⇒ NH₄Cl(s)

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