Water $(H_2O)$ is a liquid while hydrogen sulphide $(H_2S)$ is a gas because

Orthophosphoric acid $(H_3PO_4)$ exhibits high viscosity due to:

Structures of molecules of two compounds are given below:
$(a)$ Which of the two compounds will have intermolecular hydrogen bonding and which compound is expected to show intramolecular hydrogen bonding.
$(b)$ The melting point of a compound depends on,among other things,the extent of hydrogen bonding. On this basis,explain which of the above two compounds will show a higher melting point.
$(c)$ Solubility of compounds in water depends on the power to form hydrogen bonds with water. Which of the above compounds will form hydrogen bonds with water easily and be more soluble in it?

The correct order of increasing intermolecular hydrogen bond strength is .... .

The boiling point of hydrogen halides varies in the order:

Water,Ethanol,and Ether are all liquids at room temperature; why do their boiling points differ?