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Complete the following equation that illustrates a Bronsted Lowry acid-base reaction. Phases are optional. HCl +...

Complete the following equation that illustrates a Bronsted Lowry acid-base reaction. Phases are optional. HCl + NH3 --->

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Expert Solution

In 1923, a Danish chemist, named Johannes Bronsted, and British scientist, Thomas Lowry, both independently proposed a different definition of acid. They said that an acid should be any substance that can donate a proton. In this case, a proton is just a hydrogen atom that has lost its electron to become a positively charged ion of H+. This definition of an acid is now called a Bronsted-Lowry acid.

  • Conjugate acid: an acid that forms when a base gains a proton.
  • Conjugate base: a base that forms when an acid loses a proton.
  • HCl + NH3 --->NH4++CI-
  • Acid1 Base2 Acid2 Base1
  • In this reaction, HCl donates proton toNH3 & is therefore an acid. on the other hand, NH3 accepts a proton from  HCl & is therefore a base. In the reverse reaction which at equilibrium proceeds at the same rate as the forward reaction, the NH4+ ion donates a protons to CI- ion & hence NH4+is an acid,while Cl- ion which accept a proton from NH4+ is a base.

queen_honey_blossom answered 2 years ago
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