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Leona [35]
3 years ago
7

In tne equation below identify the bronsted lowry acid bronsted lowry base conjugate acid conjugate base

Chemistry
1 answer:
Ad libitum [116K]3 years ago
6 0

Answer:

  • <em>Brønsted-Lowry acid: HNO₂</em>
  • <em>Brønsted-Lowry base: NH₃</em>
  • <em>Conjugate acid: NH₄⁺</em>
  • <em>Conjugate base: NO₂⁻</em>

Explanation:

The equation is:

                 HNO_2(aq)+NH_3(aq)\rightarrow NH4^+(aq)  + NO2^-(aq)

<em>Brønsted-Lowry acids</em>  are H⁺ donors.

<em>Brønsted-Lowry bases</em> are H⁺ acceptors.

Thus, on the left side, <em>HNO₂</em> is the acid and <em>NH₃ </em>is the base.

The <em>conjugate acids</em> and <em>conjugate bases</em> are on the right side of the equation.

The <em>conjugate acid</em> is the spieces that is formed after a base accepts the proton; thus it is <em>NH₄⁺</em>. A <em>conjugate acid</em> contains one more H atom and one more + charge than the base that formed it.

The <em>conjugate base</em> is the species that is formed after the acid donates its proton; thus, <em>NO₂⁻</em> is the <em>conjugate base</em>. A <em>conjugate base</em> contains one less H atom and one more - charge than the acid that formed it.

Summarizing:

  • Brønsted-Lowry acid: HNO₂
  • Brønsted-Lowry base: NH₃
  • Conjugate acid: NH₄⁺
  • Conjugate base: NO₂⁻

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