Question

A sodium bromide solution is added to a beaker containing aqueous chlorine. What would happen?

A) Write the complete chemical equation
B) Write the dissociated ionic equation
C) Write the net ionic equation
D) List any spectator ions

Answer 1

See detailed explanation.

Step-by-step explanation:

Hello!

In this case, for the described chemical reaction, we can proceed as follows:

A) For the complete chemical reaction we note down every reacted and produced species as well as the proper balancing process:

`2NaBr(aq)+Cl_2(aq)\rightarrow 2NaCl(aq)+Br_2(g)`

In which gaseous bromine may give off.

B) The dissociated ionic equation requires the ionization of the aqueous species in ions, expect for chlorine which is not ionized:

`2Na^+(aq)+2Br^-(aq)+Cl_2(aq)\rightarrow 2Na^+(aq)+2Cl^-(aq)+Br_2(g)`

C) For the net ionic equation we cancel out the sodium ions as they are at both reactants and products:

`2Br^-(aq)+Cl_2(aq)\rightarrow +2Cl^-(aq)+Br_2(g)`

D) Based on C) we infer that the spectator ions here are the sodium ions.

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