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What is the conjugate base of [tex]$HSO_4^{-}$[/tex]?

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GinnyAnswer
To determine the conjugate base of the bisulfate ion ([tex]\(HSO_4^-\)[/tex]), we need to understand the concept of conjugate acid-base pairs. In acid-base chemistry, a conjugate base is formed when an acid loses a proton ([tex]\(H^+\)[/tex]).

Here are the steps to find the conjugate base of [tex]\(HSO_4^-\)[/tex]:

1. Identify the Acid: The species we are considering is [tex]\(HSO_4^-\)[/tex], which acts as an acid.

2. Donating a Proton: When [tex]\(HSO_4^-\)[/tex] donates a proton ([tex]\(H^+\)[/tex]), it loses that proton.

3. Resulting Species: By losing one proton, the remaining species is the sulfate ion ([tex]\(SO_4^{2-}\)[/tex]).

4. Charge Consideration: Initially, [tex]\(HSO_4^-\)[/tex] has a charge of -1. When it loses a positively charged proton ([tex]\(H^+\)[/tex]), the charge of the resulting species increases by one negative charge, leading to [tex]\(-2\)[/tex].

Therefore, the conjugate base of [tex]\(HSO_4^-\)[/tex] is the sulfate ion ([tex]\(SO_4^{2-}\)[/tex]).
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