The correct options are
A The basic nature of X− is in the order F−>Cl−>Br−>I−
B HI is the strongest acid among HF,HCl,HBr and HI
C The ionic character of M−X bond decreases in the order M−F>M−Cl>M−Br>M−I
(a) &(b): The order of acidic strength of HX is HI>HBr>HCl>HF i.e. HI is strongest acid as its bond dissociation energy is lowest due to large size of iodine. Also stronger the acid weaker its conjugate base so order of basic nature is F−>Cl−>Br−>I−
(c) Ionic charater depends upon the electronegativity difference between the cation and the anion in a compound. Since Fluorine has the highest electronegativity, H−F will be more ionic than the other H−X's and as the electronegativity decreases down the groupp, the ionic nature of H−X also decreases down the group.
(d) F does form an oxoacid HOF