According to this data collected from PubChem, polarity of nitrobenzene and benzonitrile should be similar since solubility is dependent on the polarity:
Nitrobenzene: Solubility in water, 0.2 g/100ml
Benzonitrile: Solubility in water, 0.1-0.5 g/100ml at 22 °C
p-Chlorophenol: Solubility in water, 2.7 g/100ml at 20 °C
But according to the simulator (https://www.multidlc.org/hplcsim/4_2_0/) p-chlorophenol and nitrobenzene are more similar in polarity aspect, they both give peak at 2,2 min.
What is the reason of this difference? Is it H-bonding and being a charged molecule cause more affinity to the polar mobile phase, resulting a difference between solubility and polarity?