The silver halides $\ce{AgCl},~\ce{AgBr},~\ce{AgI}$ are insoluble in $\ce{HNO3}$. This is given in J.D.Lee's inorganic chemistry text. (The strength of nitric acid is not specified though).
But won't this reaction take place? $$\ce{X- + HNO3 -> X2}$$
This example is taken from JD Lee's book itself: $$\ce{6Br- + 8HNO3 -> 3Br2 + 2NO + 6NO3- + 4H2O}$$
because concentrated Nitric acid is a powerful oxidizing agent.
Nitric acid (even concentrated) is essentially an aqeuous solution.
Effectively, silver halides will not dissolve in water (they have incredibly low $K_\text{sp}$), so the reaction indicated is moot.... there is no appreciable concentration of bromide in solution to be oxidized.
$K_\text{sp}(\ce{AgBr}) = 5.0\times10^{-13} \Rightarrow [\ce{Br-}] \approx 700~\text{nM}$
The diagnostic test for Cl-, Br- and I- is reaction with Ag+ in a dilute nitric acid solution. The reason for the nitric acid is not because the silver halides are not attacked by nitric but that the dilute acid solution prevents the formation of other insoluble silver salts such as silver oxide, carbonate, phosphate, cyanide [careful here] and who knows what else. You cannot use sulfuric [perchloric will work but why even have it around] and acetic might work. Nitric is perfect. I have little doubt that the silver halides would be oxidized to the halogens or even higher oxidation states by hot concentrated nitric acid. You are welcome to try the next time you are in the lab.
