QQuestionChemistry
QuestionChemistry
# Identify the conjugate acid for each base:
- Conjugate acid of $\mathrm{HSO}_{4}^{-}$
- Conjugate acid of $\mathrm{SO}_{4}^{2 -}$
- Conjugate acid of $\mathrm{NH}_{3}$
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Answer
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Step 1:I'll solve this chemistry problem step by step, following the specified LaTeX formatting guidelines:
Step 2:: Understanding Conjugate Acids
A conjugate acid is formed when a base accepts a proton (H⁺). To find the conjugate acid, we add a proton (H⁺) to the base.
Step 3:: Conjugate Acid of \mathrm{HSO}_{4}^{-}
- $$\mathrm{HSO}_{4}^{-}$$ is already a conjugate acid of $$\mathrm{SO}_{4}^{2-}
- Adding another H⁺ would form \mathrm{H}_{2}\mathrm{SO}_{4} (sulfuric acid)
Step 4:: Conjugate Acid of \mathrm{SO}_{4}^{2 -}
- Adding one H⁺ to $$\mathrm{SO}_{4}^{2-}$$ forms $$\mathrm{HSO}_{4}^{-}$$ (hydrogen sulfate ion)
Step 5:: Conjugate Acid of \mathrm{NH}_{3}
- Adding one H⁺ to $$\mathrm{NH}_{3}$$ forms $$\mathrm{NH}_{4}^{+}$$ (ammonium ion)
Final Answer
- Conjugate acid of \mathrm{HSO}_{4}^{-}: \mathrm{H}_{2}\mathrm{SO}_{4} - Conjugate acid of \mathrm{SO}_{4}^{2 -}: \mathrm{HSO}_{4}^{-} - Conjugate acid of \mathrm{NH}_{3}: \mathrm{NH}_{4}^{+}
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