What observations are made when a solution of Br(aq) is added dropwise to an aqueous solution of NaCl(aq)?

Question

Describe what will be observed.

Answer 1

I am assuming you mean Br- (aq), i.e. dissolved bromide ion. Please re-check your question; as it is being assumed in order to answer your question.

You are going to observe the consequences of the "competitive" redox reactions that exist when two halogen ions are in the same solution. The reaction, pardon the lack of graphics, is

2X- (aq) ---> X2 (aq)

Whichever halogen anion is the stronger reducing agent will itself be oxidized to yield the respective halogen gas. In order to visually "magnify" the effect of the reaction, it is common at the undergraduate level to then extract the formed X2 into a bit of methylene chloride or some non-polar solvent. Typically, dihalogen gases (Br2, Cl2, I2) have distinct colors that are intensified when extracted from the water into a smaller volume of solvent. Chlorine will appear yellow. Bromine will appear orange/brownish. Iodine will appear purple.

Your question, if conducted experimentally, will yield an orange color in the organic layer. What does that tell you about the relative oxidation strengths of equal concentrations of Br- vs. Cl-?

You tell us....

Answer 2

Sodium bromide can be accomplished by bubbling chlorine gas through an aqueous solution of NaBr, it should be reversed. Because Br2 is not as reactive as Cl2.

Answer 3

No reaction. Cl is more active then Br so Br cannot displace Cl ions.

Answer 4

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