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Step 1:: Recall the definition of a conjugate acid and base.
A conjugate acid is formed when a base accepts a proton (H+), and a conjugate base is formed when an acid donates a proton. The formula for a conjugate acid is obtained by adding an H+ to the formula of its base, while the formula for a conjugate base is obtained by removing an H+ from the formula of its acid.
Step 2:: Identify the given acids and bases.
Step 3:
The given base is $\mathrm{H}_{2} \mathrm{PO}_{4}^{-}$.
To find its conjugate acid, add an H+: $\mathrm{H}_{2} \mathrm{PO}_{4}^{-} + \mathrm{H}^{+} = \boxed{\mathrm{H}_{3} \mathrm{PO}_{4}}$.
Step 4:
The given base is $\mathrm{HCO}_{3}^{-}$.
To find its conjugate acid, add an H+: $\mathrm{HCO}_{3}^{-} + \mathrm{H}^{+} = \boxed{\mathrm{H}_{2} \mathrm{CO}_{3}}$.
Step 5:
The given base is $\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{O}_{6}^{2-} (\mathrm{C}_{6} \mathrm{H}_{6} \mathrm{O}_{6}^{-})$, the deprotonated form of $\mathrm{H}_{2} \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{O}_{6}$.
To find its conjugate acid, add an H+: $\mathrm{H}_{2} \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{O}_{6} + \mathrm{H}^{+} = \boxed{\mathrm{H}_{3} \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{O}_{6}}$.
Step 6:
The given acid is $\mathrm{HC}_{2} \mathrm{O}_{4}$.
To find its conjugate base, remove an H+: $\mathrm{HC}_{2} \mathrm{O}_{4} \rightarrow \mathrm{C}_{2} \mathrm{O}_{4}^{2 -} + \mathrm{H}^{+} = \boxed{\mathrm{C}_{2} \mathrm{O}_{4}^{2 -}}$.
Step 7:
To find its conjugate acid, add an H+: $\mathrm{I}^{-} + \mathrm{H}^{+} = \boxed{\mathrm{H}\mathrm{I}}$.
The given base is I-.
Step 8:
The given base is $\mathrm{NH}_{3}$.
To find its conjugate acid, add an H+: $\mathrm{NH}_{3} + \mathrm{H}^{+} = \boxed{\mathrm{NH}_{4}^{+}}$.
Final Answer
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