There is a statement given in my textbook (Cengage, Organic Chemistry (Part 1), page 4.33) which is as follows: (I edited the statement to make it simpler)
One can account for the solubilities of o-nitrophenol, salicylaldehyde,and salicylic acid in cold water, in which they are insoluble, while in hot water they are soluble, using the concept of intramolecular hydrogen bonding. However, their para- and meta- isomers are soluble even in cold water. This can be explained by intermolecular H-bonding.
I have difficulty in understanding this statement.
How does hydrogen bonding influence the solubility in hot and cold water and moreover can we draw any conclusions about boiling and melting points of the compounds, in which one has intramolecular hydrogen bonding and the other having intermolecular hydrogen bonding?