Question

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

Explanation:

Step1: Recall Bronsted - Lowry definitions

A Bronsted - Lowry acid donates \(H^{+}\), and a Bronsted - Lowry base accepts \(H^{+}\).

Step2: Analyze first reaction (\(ClO_{3}^{-}(aq)+NH_{4}^{+}(aq)\to HClO_{3}(aq)+NH_{3}(aq)\))

For \(NH_{4}^{+}\):
\(NH_{4}^{+}\) donates \(H^{+}\) (\(NH_{4}^{+}\to NH_{3}+H^{+}\)), so it is a Bronsted - Lowry acid.

Step3: Analyze second reaction (\(HClO_{3}(aq)+NH_{3}(aq)\to ClO_{3}^{-}(aq)+NH_{4}^{+}(aq)\))

For \(NH_{3}\):
\(NH_{3}\) accepts \(H^{+}\) (\(NH_{3}+H^{+}\to NH_{4}^{+}\)), so it is a Bronsted - Lowry base.

Step4: Analyze third reaction (\(ClO_{3}^{-}(aq)+NH_{4}^{+}(aq)\to HClO_{3}(aq)+NH_{3}(aq)\))

For \(ClO_{3}^{-}\):
\(ClO_{3}^{-}\) accepts \(H^{+}\) (\(ClO_{3}^{-}+H^{+}\to HClO_{3}\)), so it is a Bronsted - Lowry base.

Step5: Analyze fourth reaction (\(HClO_{3}(aq)+NH_{3}(aq)\to ClO_{3}^{-}(aq)+NH_{4}^{+}(aq)\))

For \(HClO_{3}\):
\(HClO_{3}\) donates \(H^{+}\) (\(HClO_{3}\to ClO_{3}^{-}+H^{+}\)), so it is a Bronsted - Lowry acid.

Answer:

reaction	highlighted reactant
\(HClO_{3}(aq)+NH_{3}(aq)\to ClO_{3}^{-}(aq)+NH_{4}^{+}(aq)\)	Bronsted - Lowry base
\(ClO_{3}^{-}(aq)+NH_{4}^{+}(aq)\to HClO_{3}(aq)+NH_{3}(aq)\)	Bronsted - Lowry base
\(HClO_{3}(aq)+NH_{3}(aq)\to ClO_{3}^{-}(aq)+NH_{4}^{+}(aq)\)	Bronsted - Lowry acid