posted this question before and wanted to know if I had gotten the right answers.

Question

We have to identify the five compunds of H, N, and O described below. For each compound, I have to write a Lewis structure that is consistent with the information given.
a.) All the compunds are electrolytes, although not all of them are strong electrolytes. Compunds C and D are ionic and compund B is covalent.

b.) Nitrogen occurs in its highest possible oxidation state in compunds A and C; nitrogen occurs in its lowest oxidation state in compunds C,D, and E. The formal charge on both nitrogen in compund C is +1; the formal charge on the only nitrogen in compund B is 0.

c.) Compund A and E exist in solution. Both solutions give off gases. Comercially available concentrated solutions of compund A are normally 16 M. The commercial, concentrated solution of compound E is 15 M.

d) Commercial solutions of compund E are labeled witha misnomer that implies that a binary, gaseous compund of nitrogen and hydrogen reacted with watert to produce ammonium ions and hydroxide ions. Actually this reaction occurs to only a slight extent.

e) Compound D is 43.7% N and 50.0% O by mass. If compound D were a gas at STP, it would have a density of 2.86 g/L.

f) A formula unit of compund C has one more oxygen than a formula unit of compound D. Compounds C and A have one ion in common when compound A is acting as the strong electrolyte.

g) Solutions of C are weakly acidic; solutions of compound A are strongly acidic; solutions of compound B and E are basic. The titration of .726 g of compound B requires 21.98 ml of 1.000 M HCl for complete neutralization.

A) HNO3
B) Still don't understand
C) N2O2 or NO2 not sure
D) NO
E) NH3 any comments will greatly help

Probably compound A is right although I don't think the questions provides data to prove that.
Compound E is right.
Compound B. 21.98 mL x 1.00M HCl = 21.98 millimoles HCl = 21.98 millimoles compound B in 726 mg compound B. That makes the molar mass of compound B what? I get 33. The compound is basic. So if we have an OH and N, how many more H atoms would we need for compound B. I suspect this is hydroxyl amine which has a molar mass of 33.
That leaves compounds C and D. From statement (e), if N is 43.7% and O is 50.0%, what is the extra 6.3%? I don't think NO2 or N2O2 (or NO) will give those percentages. And what have you ignored in the 6.3%? or is that a typo of some kind? And 2.86 x 22.4 = 64. NO, NO2 or N2O2 don't have a molar mass of 64. I hope this is helpful.