Will aqueous Sodium Salicylate (0.0005g of solid in 0.5 mL of water) be soluble in:
a) 6% aqueous HCl
b) 6% aqueous NaOH

My explanations
a) Although HCl is polar molecule would dissolves in it because HCl is electron poor and the oxygen in sodium salicytate is electron rich. The electron rich O would accept the H and give the pair of electrons to CL.
b) The NaOH would dissolve because it has phenol group which is non-polar allowing it to do hydrogen bonding as well.

Just wondering if my explanations are correct or not. If not could you please explain. Thank you very much!

Question

Will aqueous Sodium Salicylate (0.0005g of solid in 0.5 mL of water) be soluble in:
a) 6% aqueous HCl
b) 6% aqueous NaOH

My explanations
a) Although HCl is polar molecule would dissolves in it because HCl is electron poor and the oxygen in sodium salicytate is electron rich. The electron rich O would accept the H and give the pair of electrons to CL.
b) The NaOH would dissolve because it has phenol group which is non-polar allowing it to do hydrogen bonding as well.

Just wondering if my explanations are correct or not. If not could you please explain. Thank you very much!