You can surely conclude the acidic nature of $\text{NH}_4^+$ using the ionic reaction mentioned.
Otherwise, you can also conclude the same by acid-base the reaction through which it is formed:
$$\text{NH}_3 + \text{HCl} \longrightarrow \text{NH}_4^+\text{Cl}^-$$
Here, $\text{NH}_3$ is a comparatively weaker, Lewis base (since it has a donatable lone pair) while $\text{HCl}$ is a strong protonic acid. Thus, the salt formed by this acid-base reaction will show a mild acidic character.
The above reaction can also be represented as the following ionic reaction:
$$\text{NH}_3 + \text{H}^+ \longrightarrow \text{NH}_4^+$$
Now, note that $\text{NH}_4^+\text{Cl}^-$ can be considered equivalent to $\text{NH}_4^+$ in most of the reactions since $\text{NH}_4\text{Cl}^-$ dissociates into $\text{NH}_4^+$ and $\text{Cl}^-$ in the aqueous solution and thus $\text{Cl}^-$ has no direct impact on the reactivity of $\text{NH}_4^+$. The only thing keeping them together in a non-aqueous solution is the ionic attraction between them.
Now for the final question:
Is it correct to say that $\ce{NH4Cl}$ is the acid or that $\ce{NH4+}$
is the acid?
The thing is, theoretically when we are talking about acid-base reactions, $\text{NH}_4^+$ is considered as the salt product of acid-base reaction of ammonia and hydrochloric acid, which are far more reactive species and stronger base and acid, respectively. Hence we actually classify it as a conjugate acid, that is the product formed due to protonation of a base. Here, the lone pair of Nitrogen atom of $\text{NH}_4^+$ are providing with the electron pair to the proton ($\text H^+$), giving the nitrogen atom a positive charge. It is the conjugate acid of the base, ammonia.
Please note that the term conjugate acid or conjugate base are reaction specific. That is, these are used only for the product of an acid-base reaction.
For example, I already explained that $\text{NH}_4^+\text{Cl}^-$ is the conjugate acid of ammonia. However, if it further reacts with a base, say:
$$\text{NH}_4^+ + \text{OH}^- \longrightarrow \text{NH}_3 + \text{H}_2\text{O}$$
Since $\text{NH}_4^+$ has donated an electron here, it behaves as an acid and ammonia is its product, hence ammonia is the conjugate base of $\text{NH}_4^+$ while $\text{H}_2\text{O}$ is the product due to acceptance of a proton by $\text{OH}^-$ , so $\text{H}_2\text{O}$ is the conjugate acid of hydroxide ion.
Conjugate acid of a strong base is a weak acid, meanwhile conjugate base of a strong acid is a weak base. Conversely, conjugate acid of a weak base is a strong acid and conjugate base of a weak acid is a strong base.
So concluding the answer here, $\text{NH}_4^+\text{Cl}^-$ is the ionic salt while $\text{NH}_4^+$ is a weak acid or conjugate acid of ammonia.