Question

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

Answer 1

Answer:

See detailed explanation.

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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