Question

Explain how water behaves in this reaction. Which definition of acids and bases would you apply? Upper subscript 2 upper C upper O subscript 3 plus upper H subscript 2 upper O right arrow upper H upper C upper O subscript 3 superscript minus plus upper H subscript 3 upper O superscript plus.

Answer 1

Answer:

Brownstead- Lowry base

Explanation:

A Brownstead- Lowry base accepts protons. If we look at this reaction, the water molecule accepted a proton to form its conjugate acid H3O^+.

Hence, in this particular instance, water behaved as a Brownstead- Lowry base in accordance with the definition of a Brownstead- Lowry bases.

Answer 2

Answer:

the correct answer is:

Explanation:

Water behaves as a base in this reaction.

The Bronsted-Lowry definition is applied because the reaction involves the transfer of H+ from one reactant to the other.

A Bronsted-Lowry base is defined as a substance that accepts a proton.

Because water gains a proton to form H3O+ in this particular reaction, it acts as a base.

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