Ammonium chloride in aqueous solution
When ammonium chloride is hydrolyzing, there is established equilibrium

$$\ce{NH4+  + H2O &lt;&lt;=&gt; NH3 + H2O+}$$

with $$\mathrm{pH}=7-\frac 12 ( 4.75 + \log {c_{\ce{NH4Cl}}} )$$

$$\mathrm{pOH}=14 - \mathrm{pH}=7+\frac 12 ( 4.75 + \log {c_{\ce{NH4Cl}}} )$$

Concentration of ammonia is several orders higher than concentration of hydroxide ions, with origin of water dissociation, so no ammonia hydroxide there.

When ammonia is dissolved, there is established equilibrium

$$\ce{NH3  + H2O &lt;&lt;=&gt; NH4+ + OH-}$$

with $$\mathrm{pH}=14-\frac 12 ( 4.75 - \log {c_{\ce{NH3}}} )$$

Equimolar concentrations of $\ce{NH4+ + OH-}$ are sometimes formally called ammonium hydroxide, but using this term is deprecated and it cannot be isolated.