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15240672380's Question
Posted 3 months ago

3. For each of the following bases, write the formula for its conjugate acid; for each acid write the formula of the conjugate base.
Base & Conjugate Acid & Acid & Conjugate Base \\
I\mathrm{I}^{-} & & HClO4\mathrm{HClO}_{4} \\
SO32\mathrm{SO}_{3}{ }^{2-} & \square & H2 S\mathrm{H}_{2} \mathrm{~S} & \\
PO43\mathrm{PO}_{4}{ }^{3-} & \square & HCO3\mathrm{HCO}_{3}{ }^{-} & \\
\cline { 2 - 2 } & & &
C2H3O2\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

a) Write the products.
b) For all four (4) species in the equation, indicate whether each will act as an acid or a base.
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Answer from Sia
Posted 3 months ago
Conjugate Acid of I-: To find the conjugate acid of a base, add a proton (H⁺) to the base. For the iodide ion, I \mathrm{I}^{-} , the conjugate acid is HI \mathrm{HI}
Conjugate Acid of \( \mathrm{SO}_{3}^{2-} \): Similarly, adding a proton to the sulfite ion, SO32 \mathrm{SO}_{3}^{2-} , gives the conjugate acid HSO3 \mathrm{HSO}_{3}^{-}
Conjugate Acid of \( \mathrm{PO}_{4}^{3-} \): Adding a proton to the phosphate ion, PO43 \mathrm{PO}_{4}^{3-} , results in the conjugate acid HPO42 \mathrm{HPO}_{4}^{2-}
Conjugate Base of \( \mathrm{HClO}_{4} \): Removing a proton from perchloric acid, HClO4 \mathrm{HClO}_{4} , gives the conjugate base ClO4 \mathrm{ClO}_{4}^{-}
Conjugate Base of \( \mathrm{H}_{2}S \): Removing a proton from hydrogen sulfide, H2S \mathrm{H}_{2}S , gives the conjugate base HS \mathrm{HS}^{-}
Conjugate Base of \( \mathrm{HCO}_{3}^{-} \): Removing a proton from bicarbonate ion, HCO3 \mathrm{HCO}_{3}^{-} , gives the conjugate base CO32 \mathrm{CO}_{3}^{2-}
Conjugate Base of \( \mathrm{C}_{2}\mathrm{H}_{3}\mathrm{O}_{2}^{-} \): Since acetate ion, C2H3O2 \mathrm{C}_{2}\mathrm{H}_{3}\mathrm{O}_{2}^{-} , is already a base, its conjugate acid would be acetic acid, HC2H3O2 \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
Products of the Reaction: The reaction between NH3 \mathrm{NH}_{3} and H2O \mathrm{H}_{2}O produces NH4+ \mathrm{NH}_{4}^{+} and OH \mathrm{OH}^{-}
Acid or Base Identification: In the reaction, NH3 \mathrm{NH}_{3} acts as a base by accepting a proton from H2O \mathrm{H}_{2}O , which acts as an acid. The products NH4+ \mathrm{NH}_{4}^{+} and OH \mathrm{OH}^{-} are the conjugate acid and base, respectively
3 Answer
Conjugate acids: HI \mathrm{HI} , HSO3 \mathrm{HSO}_{3}^{-} , HPO42 \mathrm{HPO}_{4}^{2-}
Conjugate bases: ClO4 \mathrm{ClO}_{4}^{-} , HS \mathrm{HS}^{-} , CO32 \mathrm{CO}_{3}^{2-}
4 Answer
Products: NH4+ \mathrm{NH}_{4}^{+} , OH \mathrm{OH}^{-}
Acid/Base Identification: NH3 \mathrm{NH}_{3} (base), H2O \mathrm{H}_{2}O (acid), NH4+ \mathrm{NH}_{4}^{+} (acid), OH \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.
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.

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