Answer
Bronsted-Lowry acid: $H_{2}O$
Bronsted-Lowry base: $C_5H_5N$
Conjugate acid: $C_5H_5NH^+$
Conjugate base: $OH^{-}$
Work Step by Step
According to the Bronsted-Lowry definition,
Acid: proton ($H^{+}$ ion) donor
Base: proton ($H^{+}$ ion) acceptor
In the reaction, $H_{2}O$ is the acid because it donates a proton to water.
$C_5H_5N$ is the base because it accepts the proton.
A conjugate acid is any base to which a proton has been added. So, $C_5H_5NH^+$ is the conjugate acid.
A conjugate base is an acid from which a proton has been removed. So, $OH^{-}$ is the conjugate base.
