Question #71402

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Question #71402

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Answer 1 · 2017-08-23T19:29:56

The conjugate acid-base pairs are $HB {(OH)}_{4} / B {(OH)}_{4}^{-}$ $"HB"("OH")_4//"B"("OH")_4^"-"$ and $H_{3} O^{+} / H_{2} O$ $"H"_3"O"^"+"//"H"_2"O"$ .

Explanation:

Write the equation in two steps.

$B {(OH)}_{3} + H_{2} O \to HB {(OH)}_{4}$ $"B"("OH")_3 + "H"_2"O" → "HB"("OH")_4"$

Then

$underbrace("HB"("OH")_4)_color(red)("acid") + overbrace("H"_2"O")^(color(blue)("base")) ⇌ underbrace("B"("OH")_4^"-")_color(red)("conjugate base") + overbrace("H"_3"O"^"+")^(color(blue)("conjugate acid"))$

A conjugate base is a Brønsted-Lowry acid minus a proton, and a conjugate acid is a Brønsted-Lowry base plus a proton.

Thus, $"HB"("OH")_4$ and $"B"("OH")_4^"-"$ are a conjugate acid-base pair.

Also, $"H"_3"O"^"+"$ and $"H"_2"O"$ are a conjugate acid-base pair.

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Question #71402

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