[Ben Cohen]

The addition of 0.01 mol of which of the following to
100 mL of H2O will give the most alkaline aqueous
solution?
(A) NH3
(B) HONH2
(C) CH3NH2
(D) H2NNH2

I drew the four molecules and was between B and D, but I chose D because it had 2 lone pairs on the Nitrogens, and lone pairs tend to give more basicity. However, the answer was C. I have no idea regarding the reasoning behind this.
I also tried to think about conjugate acid stability.
NH₄⁺ is, I thought, relatively stable. The conjugate acids of B and D don't seem too stable (especially D, because with one of the nitrogens having 3 H's and the other having 2, it doesn't seem good, and also there would be resonance).

Additionally, I considered formal charge, but every atom in all 4 of the compounds has a formal charge of 0.

I'm pretty confused, and I would really like to hear the rationale behind this.

Thanks in advance.

[Hunter2]

C because of positiv inductive effect of Methyl group.

http://www.chemguide.co.uk/basicorg/acidbase/bases.html

[Ben Cohen]

C because of positiv inductive effect of Methyl group.

http://www.chemguide.co.uk/basicorg/acidbase/bases.html

Thank you so much this explained it so well!