Question

determine if the following salt is neutral, acidic or basic. if acidic or basic, write the appropriate equilibrium equation for the acid or base that exists when the salt is dissolved in aqueous solution. if neutral, simply write only nr. be sure to include the proper phases for all species within the reaction.
nh₄br

Explanation:

Step1: Analyze the salt

$\mathrm{NH_4Br}$ is a salt composed of $\mathrm{NH_4^+}$ (ammonium ion) and $\mathrm{Br^-}$ (bromide ion).

Step2: Consider the nature of ions

$\mathrm{Br^-}$ is the conjugate base of a strong acid ($\mathrm{HBr}$), so it does not hydrolyze. $\mathrm{NH_4^+}$ is the conjugate acid of a weak base ($\mathrm{NH_3}$).

Step3: Write the hydrolysis reaction

$\mathrm{NH_4^+}$ undergoes hydrolysis:

$$\mathrm{NH_4^+(aq) + H_2O(l) ightleftharpoons NH_3(aq) + H_3O^+(aq)}$$

. Since $\mathrm{H_3O^+}$ (hydronium ion) is produced, the solution is acidic.

Answer:

Acidic.

$$\mathrm{NH_4^+(aq) + H_2O(l) ightleftharpoons NH_3(aq) + H_3O^+(aq)}$$