3. For each of the following bases, write the formula for its conjugate acid; for each acid write the formula of the conjugate base.
\begin{tabular}{llll}
Base & Conjugate Acid & Acid & Conjugate Base \
$\mathrm{I}^{-}$ & & $\mathrm{HClO}_{4}$ \
$\mathrm{SO}_{3}{ }^{2-}$ & $\square$ & $\mathrm{H}_{2} \mathrm{~S}$ & \
$\mathrm{PO}_{4}{ }^{3-}$ & $\square$ & $\mathrm{HCO}_{3}{ }^{-}$ & \
\cline { 2 - 2 } & & &
\end{tabular}
$\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}^{-}$ $\qquad$
4. For the following acid-base reaction:
$$
\mathrm{NH}_{2}^{-}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}_{(\mathrm{l})} \rightleftharpoons
$$
$\qquad$
$\qquad$
a) Write the products.
b) For all four (4) species in the equation, indicate whether each will act as an acid or a base.

Question

3. For each of the following bases, write the formula for its conjugate acid; for each acid write the formula of the conjugate base.
\begin{tabular}{llll} 
Base & Conjugate Acid & Acid & Conjugate Base \
$\mathrm{I}^{-}$ & & $\mathrm{HClO}_{4}$ \
$\mathrm{SO}_{3}{ }^{2-}$ & $\square$ & $\mathrm{H}_{2} \mathrm{~S}$ & \
$\mathrm{PO}_{4}{ }^{3-}$ & $\square$ & $\mathrm{HCO}_{3}{ }^{-}$ & \
\cline { 2 - 2 } & & &
\end{tabular}
$\mathrm{C}_{2} \mathrm{H}_{3} \mathrm{O}_{2}^{-}$ $\qquad$
4. For the following acid-base reaction:
$$
\mathrm{NH}_{2}^{-}(\mathrm{aq})+\mathrm{H}_{2} \mathrm{O}_{(\mathrm{l})} \rightleftharpoons
$$
$\qquad$
$\qquad$
a) Write the products.
b) For all four (4) species in the equation, indicate whether each will act as an acid or a base.

Accepted Answer

∻Solution∻ ‖ 1 ⋮ **Conjugate Acid of I-**: To find the conjugate acid of a base, add a proton (H⁺) to the base. For the iodide ion, $ \mathrm{I}^{-} $, the conjugate acid is $ \mathrm{HI} $. ‖ ‖ 2 ⋮ **Conjugate Acid of $ \mathrm{SO}_{3}^{2-} $**: Similarly, adding a proton to the sulfite ion, $ \mathrm{SO}_{3}^{2-} $, gives the conjugate acid $ \mathrm{HSO}_{3}^{-} $. ‖ ‖ 3 ⋮ **Conjugate Acid of $ \mathrm{PO}_{4}^{3-} $**: Adding a proton to the phosphate ion, $ \mathrm{PO}_{4}^{3-} $, results in the conjugate acid $ \mathrm{HPO}_{4}^{2-} $. ‖ ‖ 4 ⋮ **Conjugate Base of $ \mathrm{HClO}_{4} $**: Removing a proton from perchloric acid, $ \mathrm{HClO}_{4} $, gives the conjugate base $ \mathrm{ClO}_{4}^{-} $. ‖ ‖ 5 ⋮ **Conjugate Base of $ \mathrm{H}_{2}S $**: Removing a proton from hydrogen sulfide, $ \mathrm{H}_{2}S $, gives the conjugate base $ \mathrm{HS}^{-} $. ‖ ‖ 6 ⋮ **Conjugate Base of $ \mathrm{HCO}_{3}^{-} $**: Removing a proton from bicarbonate ion, $ \mathrm{HCO}_{3}^{-} $, gives the conjugate base $ \mathrm{CO}_{3}^{2-} $. ‖ ‖ 7 ⋮ **Conjugate Base of $ \mathrm{C}_{2}\mathrm{H}_{3}\mathrm{O}_{2}^{-} $**: Since acetate ion, $ \mathrm{C}_{2}\mathrm{H}_{3}\mathrm{O}_{2}^{-} $, is already a base, its conjugate acid would be acetic acid, $ \mathrm{HC}_{2}\mathrm{H}_{3}\mathrm{O}_{2} $. However, this is not part of the table, so we do not need to find its conjugate base. ‖ ‖ 8 ⋮ **Products of the Reaction**: The reaction between $ \mathrm{NH}_{3} $ and $ \mathrm{H}_{2}O $ produces $ \mathrm{NH}_{4}^{+} $ and $ \mathrm{OH}^{-} $. ‖ ‖ 9 ⋮ **Acid or Base Identification**: In the reaction, $ \mathrm{NH}_{3} $ acts as a base by accepting a proton from $ \mathrm{H}_{2}O $, which acts as an acid. The products $ \mathrm{NH}_{4}^{+} $ and $ \mathrm{OH}^{-} $ are the conjugate acid and base, respectively. ‖ ∻3 Answer∻ ⚹ Conjugate acids: $ \mathrm{HI} $, $ \mathrm{HSO}_{3}^{-} $, $ \mathrm{HPO}_{4}^{2-} $ ⚹ ⚹ Conjugate bases: $ \mathrm{ClO}_{4}^{-} $, $ \mathrm{HS}^{-} $, $ \mathrm{CO}_{3}^{2-} $ ⚹ ∻4 Answer∻ ⚹ Products: $ \mathrm{NH}_{4}^{+} $, $ \mathrm{OH}^{-} $ ⚹ ⚹ Acid/Base Identification: $ \mathrm{NH}_{3} $ (base), $ \mathrm{H}_{2}O $ (acid), $ \mathrm{NH}_{4}^{+} $ (acid), $ \mathrm{OH}^{-} $ (base) ⚹ ∻Key Concept∻ ⚹ Conjugate acids and bases are pairs that differ by one proton. In a reaction, the acid donates a proton, and the base accepts a proton. ⚹ ∻Explanation∻ ⚹ The conjugate acid of a base is formed by adding a proton to the base, while the conjugate base of an acid is formed by removing a proton from the acid. In the given acid-base reaction, ammonia acts as a base and water as an acid, resulting in ammonium and hydroxide ions. ⚹◊What are the products of the reaction between NH3 (ammonia) and H2O (water)?⍭ Generate me a similar question◊

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