Question

question 3
true or false? bicarbonate ion can act as an acid and as a base.
false
true
question 4
10 pts
which of the following does not describe (or does not apply to) an aqueous solution of hbr?
it is a solution of hydrobromic acid.
it should be handled with caution.
there are more hydroxide ions than hydronium ions in the solution.
if a koh is added to this solution, a neutralization (acid - base) reaction will occur.

Explanation:

Step1: Define amphoteric species

Bicarbonate ion ($HCO_3^-$) is amphoteric. It can donate a proton ($H^+$) to act as an acid (e.g., $HCO_3^-+OH^-
ightarrow CO_3^{2 -}+H_2O$) and accept a proton to act as a base (e.g., $HCO_3^- + H^+
ightarrow H_2CO_3$). So the answer to Question 3 is True.

Step2: Analyze properties of HBr solution

Hydrobromic acid ($HBr$) is a strong acid. In an aqueous solution of a strong - acid like $HBr$, $HBr$ dissociates completely into $H_3O^+$ and $Br^-$. So, there are more hydronium ions ($H_3O^+$) than hydroxide ions ($OH^-$). The statement "There are more hydroxide ions than hydronium ions in the solution" does not apply to an aqueous solution of $HBr$.

Answer:

Question 3: True
Question 4: There are more hydroxide ions than hydronium ions in the solution.