Question

for each chemical reaction in the table below, decide whether the highlighted reactant is a bronsted - lowry acid, a bronsted - lowry base, or neither.

reaction
highlighted reactant
bronsted - lowry acid
bronsted - lowry base
neither
hso₄⁻(aq) + nh₄⁺(aq) → h₂so₄(aq) + nh₃(aq)
o
o
o
hso₄⁻(aq) + nh₄⁺(aq) → h₂so₄(aq) + nh₃(aq)
o
o
o
h₂so₄(aq) + nh₃(aq) → hso₄⁻(aq) + nh₄⁺(aq)
o
o
o
h₂so₄(aq) + nh₃(aq) → hso₄⁻(aq) + nh₄⁺(aq)
o
o
o

Explanation:

• For the first reaction with highlighted \( \text{NH}_4^+ \):
• A Brønsted - Lowry acid donates \( H^+ \). \( \text{NH}_4^+ \) loses an \( H^+ \) to form \( \text{NH}_3 \), so it is a Brønsted - Lowry acid.
• For the second reaction with highlighted \( \text{HSO}_4^- \):
• A Brønsted - Lowry base accepts \( H^+ \). \( \text{HSO}_4^- \) gains an \( H^+ \) to form \( \text{H}_2\text{SO}_4 \), so it is a Brønsted - Lowry base.
• For the third reaction with highlighted \( \text{NH}_3 \):
• A Brønsted - Lowry base accepts \( H^+ \). \( \text{NH}_3 \) gains an \( H^+ \) to form \( \text{NH}_4^+ \), so it is a Brønsted - Lowry base.
• For the fourth reaction with highlighted \( \text{H}_2\text{SO}_4 \):
• A Brønsted - Lowry acid donates \( H^+ \). \( \text{H}_2\text{SO}_4 \) loses an \( H^+ \) to form \( \text{HSO}_4^- \), so it is a Brønsted - Lowry acid.

Answer:

reaction	highlighted reactant
\( \text{HSO}_4^-(aq)+\text{NH}_4^+(aq)\to\text{H}_2\text{SO}_4(aq)+\text{NH}_3(aq) \) (highlighted \( \text{HSO}_4^- \))	Brønsted - Lowry base
\( \text{H}_2\text{SO}_4(aq)+\text{NH}_3(aq)\to\text{HSO}_4^-(aq)+\text{NH}_4^+(aq) \) (highlighted \( \text{NH}_3 \))	Brønsted - Lowry base
\( \text{H}_2\text{SO}_4(aq)+\text{NH}_3(aq)\to\text{HSO}_4^-(aq)+\text{NH}_4^+(aq) \) (highlighted \( \text{H}_2\text{SO}_4 \))	Brønsted - Lowry acid