Question

Write balanced net ionic equations for the reactions that occur when the following aqueous solutions are mixed. If no reaction is likely to occur, so indicate. (Use the lowest possible coefficients. Include states-of-matter under SATP conditions in your answer. If no reaction occurs, enter "NONE".)

A). Na2CO3 and AgNO3

B). NaOH and K2SO4

C). FeSO4 and Pb(NO3)2

Answer 1

Solution :-

First we balance the equation so that both sides of the equation have same number of atoms of each elements.

Then we split the aqueous (ionic) species into the respective ions.

Then to write the net ionic equation we cancel the spectator ions ( same ions on both side of equation) and remaining equation is written as net ionic equation.

A)Balanced reaction equation

Na2CO3(aq) + 2AgNO3(aq) --- > Ag2CO3(s) + 2NaNO3(aq)

Complete ionic equation

2Na^+(aq) + CO3^2-(aq) + 2Ag^+(aq) + 2NO3^-(aq) --- > Ag2CO3(s) + 2Na^+(aq) + 2NO3^-(aq)

Net ionic equation

CO3^2-(aq) + 2Ag^+(aq)   --- > Ag2CO3(s)

B)Balanced reaction equation

2NaOH(aq) + K2SO4(aq) ---- > Na2SO4(aq) + 2KOH(aq)

Both products of the reaction are soluble (aqueous ) therefore it do not have net ionic equation

None

C)Balanced reaction equation

FeSO4(aq) + Pb(NO3)2(aq) --- >PbSO4(s) + Fe(NO3)2(aq)

Total ionic equation

Fe^2+(aq) + SO4^2-(aq) + Pb^2+(aq) + 2NO3^-(aq) --- >PbSO4(s) + Fe^2+(aq) + 2NO3^-(aq)

Net ionic equation

SO4^2-(aq) + Pb^2+(aq)   --- >PbSO4(s)