Is Ammonia (NH3) base?
Your problems are caused by using the Arrhenius theory, which is based on electrolytic dissociation.

According to the Arrhenius definition, acids are compounds that dissociate and release hydrogen ions $(\ce{H+})$ into the solution:
$$\ce{HCl -&gt; H+ + Cl-}$$
Bases are defined as compounds that dissociate and release hydroxide ions $(\ce{OH-})$ into the solution:
$$\ce{NaOH -&gt; Na+ + OH-}$$
The products of a neutralization reaction of an acid with a base are a salt and water:
$$\ce{HCl + NaOH -&gt; NaCl + H2O}$$
This definition works for metal hydroxides such as $\ce{NaOH}$, which can exist as pure compounds. However, it doesn’t work for bases such as $\ce{NH3}$.

In order to solve this problem for $\ce{NH3}$, the fictitious compound “ammonium hydroxide” $\ce{NH4OH}$ was proposed (see also this related answer). Assuming this formula, the Arrhenius definitions of bases and neutralization reactions work again:
$$\ce{NH4OH -&gt; NH4+ + OH-}$$
$$\ce{HCl + NH4OH -&gt; NH4Cl + H2O}$$
However, ammonium hydroxide cannot be isolated; the fictitious solid compound does not exist. Nevertheless, the misleading traditional name “ammonium hydroxide” is still widely used for solutions of ammonia in water.

In order to really solve your problems with $\ce{NH3}$, you need to switch from the definition of bases according to the Arrhenius theory to the definition of bases according to the Brønsted–Lowry theory.