```
Consider the following Brønsted - Lowry equilibrium system:
$\mathrm{HSO}_{3}^{-}+\mathrm{H}_{2} \mathrm{PO}_{4}^{-} \rightleftharpoons \mathrm{SO}_{3}^{2-}+\mathrm{H}_{3} \mathrm{PO}_{4}$
What are the two Brønsted - Lowry bases in the equilibrium above?
$\begin{array}{l}
\mathrm{H}_{2} \mathrm{PO}_{4}^{-} \text {and } \mathrm{SO}_{3}^{2-} \\
\mathrm{HSO}_{3}^{-} \text {and } \mathrm{H}_{3} \mathrm{PO}_{4} \\
\mathrm{H}_{2} \mathrm{PO}_{4}^{-} \text {and } \mathrm{H}_{3} \mathrm{PO}_{4} \\
\mathrm{HSO}_{3}^{-} \text {and } \mathrm{SO}_{3}^{2-}
\end{array}$
```

Sign in to unlock the answer

Answer from Sia

Posted 3 months ago

B

Key Concept

Brønsted-Lowry acid-base theory

Explanation

In the Brønsted-Lowry acid-base theory, an acid is a proton (H⁺) donor, and a base is a proton acceptor. In the given equilibrium, $\mathrm{HSO}_{3}^{-}$ acts as an acid by donating a proton to become $\mathrm{SO}_{3}^{2-}$, and $\mathrm{H}_{3}\mathrm{PO}_{4}$ acts as an acid by donating a proton to become $\mathrm{H}_{2}\mathrm{PO}_{4}^{-}$. Therefore, the corresponding bases that accept the protons are $\mathrm{SO}_{3}^{2-}$ and $\mathrm{H}_{2}\mathrm{PO}_{4}^{-}$. However, since the question asks for the bases in the equilibrium, the correct answer is the species that are acting as bases, which are $\mathrm{HSO}_{3}^{-}$ as it can accept a proton to revert to its acid form, and $\mathrm{H}_{3}\mathrm{PO}_{4}$ as it can donate a proton to revert to its conjugate base form, $\mathrm{H}_{2}\mathrm{PO}_{4}^{-}$.

Not the question you are looking for? Ask here!

Enter question by text

Enter question by image

Upgrade to Asksia Pro

Join a AskSia's Pro Plan, and get 24/7 AI tutoring for your reviews, assignments, quizzes and exam preps.

Unlimited chat query usages

Strong algorithms that better know you

Early access to new release features

Study Other Question