Reaction between halogens and concentrated nitric acid
This question can easily be addressed considering reduction potential of each compound. Concentrated nitric acid is a powerful oxidizing acid, which has a high reduction potential:

$$
\begin{align}
\ce{NO3- + 4H+ + 3e- &amp;&lt;=&gt; NO + 2H2O} &amp;\quad E^\circ &amp;= \pu{0.957 V} \tag1\\
\ce{NO3- + 3H+ + 2e- &amp;&lt;=&gt; HNO2 + H2O} &amp;\quad E^\circ &amp;= \pu{0.934 V} \tag2\\
\ce{2NO3- + 4H+ + 2e- &amp;&lt;=&gt; N2O4 + 2H2O} &amp;\quad E^\circ &amp;= \pu{0.803 V} \tag3
\end{align}
$$

Now, let's look at reduction potential of halides:

$$
\begin{align}
\ce{F2 + 2e- &amp;&lt;=&gt; 2F-} &amp;\quad E^\circ &amp;= \pu{2.866 V} \tag4\\
\ce{Cl2 + 2e- &amp;&lt;=&gt; 2Cl-} &amp;\quad E^\circ &amp;= \pu{1.3583 V} \tag5\\
\ce{Br2 + 2e- &amp;&lt;=&gt; 2Br-} &amp;\quad E^\circ &amp;= \pu{1.066 V} \tag6\\
\ce{I2 + 2e- &amp;&lt;=&gt; 2I-} &amp;\quad E^\circ &amp;= \pu{0.5355 V} \tag7\\
\end{align}
$$
Accordingly, we can list oxidizing power at standard conditions in decreasing order:

$$\ce{F2} &gt; \ce{Cl2} &gt; \ce{Br2} &gt; \ce{NO3-} &gt; \ce{I2}$$

Therefore, at standard condition, concentrated $\ce{HNO3}$ acid (meaning $\ce{NO3-}$ in acidic medium) can easily oxidize only $\ce{I2}.$ One such example is documented in Ref.1. According to the authors, the oxidation of iodine by hyperazeotropic nitric acid ($\pu{16–21 M}$) was shown to proceed in at least two steps: 

$$
\begin{align}
\ce{I2 + 3HNO3 &amp;&lt;=&gt;[$k_1$][$k_2$] 2I+ + 2NO3- + 2HNO2 + H2O}\\
\ce{I+ + 6HNO3 &amp;&lt;=&gt;[$k_3$][$k_1$] I^5+ + 4NO3- + 2HNO2 + 2H2O}
\end{align}
$$

Since reduction potentials of $\ce{HNO3}$ and $\ce{Br2}$ are in such close range that each can oxidize the other. In fact, the kinetic studies of this phenomenon has been performed in literature (Ref.2).

In different aspect, there is a publication (Ref.3) claiming that the presence of bromine in fuming nitric acid makes it a brominating reagent (electrophilic aromatic substitution):



This bromination has worked well with deactivated aromatic nucleus. In absence of bromine, the reagent nitrate the ring. Thus, it is safe to suggest that $\ce{HNO3}$ might promote formation of '$\ce{Br+}$', meaning oxidation.

References:


J. C. Mailen, T. O. Tiffany, "The reaction of iodine with concentrated nitric acid," Journal of Inorganic and Nuclear Chemistry 1975, 37(1), 127-132 (https://doi.org/10.1016/0022-1902(75)80139-4).
Istvan Lengyel, Istvan Nagy, Gyorgy Bazsa, "Kinetic study of the autocatalytic nitric acid-bromide reaction and its reverse, the nitrous acid-bromine reaction," J. Phys. Chem. 1989, 93(7), 2801–2807 (https://doi.org/10.1021/j100344a021).
Alexander M. Andrievsky, Vera I. Lomzakova, Mikhail K. Grachev, Mikhail V. Gorelik, "Aromatic Bromination in Concentrated Nitric Acid," Open Journal of Synthesis Theory and Applications 2014, 3(2), Article ID:44941, 5 pages (doi: 10.4236/ojsta.2014.32003).