The species `H_(2)O, HCO_(3)^(Θ), HSO_(4)^(Θ), NH_(3)` can act both as Bronsted acids and bases. For each case write the corresponding conjugate acid.

Explanation

To find the corresponding conjugate acids for the species \( H_2O, HCO_3^-, HSO_4^-, \) and \( NH_3 \), we follow the Bronsted-Lowry theory, which states that:

- A Bronsted acid is a species that donates a proton (\( H^+ \)).
- A Bronsted base is a species that accepts a proton (\( H^+ \)).
- The conjugate acid is formed when a base accepts a proton.

Now, let's analyze each species step by step:

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