Questions: The preparations of two aqueous solutions are described in the table below. For each solution, write the chemical formulas of the major species present at equilibrium. You can leave out water itself. Write the chemical formulas of the species that will act as acids in the 'acids' row, the formulas of the species that will act as bases in the 'bases' row, and the formulas of the species that will act as neither acids nor bases in the 'other' row. You will find it useful to keep in mind that NH3 is a weak base. 1.2 mol of HNO3 is added to 1.0 L of a 1.2 M NH3 solution. - acids: - bases: - other: 0.05 mol of KOH is added to 1.0 L of a solution that is 0.6 M in both NH3 and NH4Br. - acids: - bases: - other:

The preparations of two aqueous solutions are described in the table below. For each solution, write the chemical formulas of the major species present at equilibrium. You can leave out water itself.
Write the chemical formulas of the species that will act as acids in the 'acids' row, the formulas of the species that will act as bases in the 'bases' row, and the formulas of the species that will act as neither acids nor bases in the 'other' row.

You will find it useful to keep in mind that NH3 is a weak base.

1.2 mol of HNO3 is added to 1.0 L of a 1.2 M NH3 solution.
- acids:
- bases:
- other:

0.05 mol of KOH is added to 1.0 L of a solution that is 0.6 M in both NH3 and NH4Br.
- acids:
- bases:
- other:

Transcript text: The preparations of two aqueous solutions are described in the table below. For each solution, write the chemical formulas of the major species present at equilibrium. You can leave out water itself. Write the chemical formulas of the species that will act as acids in the 'acids' row, the formulas of the species that will act as bases in the 'bases' row, and the formulas of the species that will act as neither acids nor bases in the 'other' row. You will find it useful to keep in mind that $\mathrm{NH}_{3}$ is a weak base. \begin{tabular}{|c|c|} \hline 1.2 mol of $\mathrm{HNO}_{3}$ is added to 1.0 L of a $1.2 \mathrm{M} \mathrm{NH}_{3}$ solution. & acids: bases: other: \\ \hline \begin{tabular}{l} 0.05 mol of KOH is added to \\ 1.0 L of a solution that is 0.6 M in both $\mathrm{NH}_{3}$ and $\mathrm{NH}_{4} \mathrm{Br}$. \end{tabular} & acids: $\square$ bases: $\square$ other: $\square$ \\ \hline \end{tabular}

Solution

Solution Steps

Step 1: Identify the major species in the first solution

For the first solution, 1.2 mol of $\mathrm{HNO}_3$ is added to 1.0 L of a 1.2 M $\mathrm{NH}_3$ solution.

$\mathrm{HNO}_3$ is a strong acid and will dissociate completely into $\mathrm{H}^+$ and $\mathrm{NO}_3^-$.
$\mathrm{NH}_3$ is a weak base and will react with $\mathrm{H}^+$ to form $\mathrm{NH}_4^+$.

The major species at equilibrium will be:

$\mathrm{NH}_4^+$ (formed from the reaction of $\mathrm{NH}_3$ and $\mathrm{H}^+$)
$\mathrm{NO}_3^-$ (from the dissociation of $\mathrm{HNO}_3$)

Step 2: Classify the species in the first solution

Acids: $\mathrm{NH}_4^+$
Bases: None (since $\mathrm{NH}_3$ has reacted completely with $\mathrm{H}^+$)
Other: $\mathrm{NO}_3^-$

Step 3: Identify the major species in the second solution

For the second solution, 0.05 mol of KOH is added to 1.0 L of a solution that is 0.6 M in both $\mathrm{NH}_3$ and $\mathrm{NH}_4Br$.

KOH is a strong base and will dissociate completely into $\mathrm{K}^+$ and $\mathrm{OH}^-$.
$\mathrm{NH}_3$ is a weak base.
$\mathrm{NH}_4Br$ dissociates completely into $\mathrm{NH}_4^+$ and $\mathrm{Br}^-$.

The major species at equilibrium will be: