Quinoline, [tex]C_{9}H_{7}N[/tex]acts a Bronsted-Lowry base as it can accept a proton, [tex]H^{+}[/tex]from water to form the conjugate base, [tex]C_{9}H_{7}NH^{+}[/tex]. This reaction can be represented as,
[tex]C_{9}H_{7}N(aq)+H_{2}O(l)<==> C_{9}H_{7}NH^{+}(aq)+OH^{-}(aq)[/tex]
Here in the reaction, the weak base quinoline accepts a proton [tex]H^{+}[/tex]from water to form the conjugate base of quinoline, [tex]C_{9}H_{7}NH^{+}[/tex] and hydroxide ion, [tex]OH^{-}[/tex]
Therefore the net ionic equation to show the basic nature of quinoline in water is,
[tex]C_{9}H_{7}N(aq)+H_{2}O(l)<==> C_{9}H_{7}NH^{+}(aq)+OH^{-}(aq)[/tex]
