Conjugate acid of $\mathrm{NH}_2^{-}$and $\mathrm{NH}_3$ are respectively
Conjugate acid of $\mathrm{NH}_2^{-}$and $\mathrm{NH}_3$ are respectively
$\mathrm{NH}_4 \mathrm{OH}$ and $\mathrm{NH}_2 \mathrm{OH}$
$\mathrm{NH}_3$ and $\mathrm{NH}_2^{-}$
$\mathrm{NH}_3$ and $\mathrm{NH}_4{ }^{+}$
$\mathrm{NH}_4{ }^{+}$and $\mathrm{NH}_3$
Solution
Conjugate acid is formed when a BronstedLowry base accepts a proton.
Hence, the conjugate acid of $\mathrm{NH}_2^{-}$is $\mathrm{NH}_3$ and of $\mathrm{NH}_3$ is $\mathrm{NH}_4^{+}$.