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

The net ionic equations are: 2Ag+ + 2Br- -> 2AgBr(s); H+ + OH- -> H2O(l); Co2+ + S2- -> CoS(s).

Step-by-step explanation:

The net ionic equation for the reaction between silver nitrate (AgNO3) and magnesium bromide (MgBr2) is:

2Ag+ + 2Br- -> 2AgBr(s)

The net ionic equation for the reaction between perchloric acid (HClO4) and potassium hydroxide (KOH) is:

H+ + OH- -> H2O(l)

The net ionic equation for the reaction between ammonium sulfide ((NH4)2S) and cobalt(II) chloride (CoCl2) is:

Co2+ + S2- -> CoS(s)

Answer 2

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)`