[moop1]

Hi, I was wondering, if I have an acid like :

NH₂NH3₃⁺

and it asks me the conjugate base, where am I supposed to place the H⁺

Or if I have the base :

HCOO^- and it asks me what is the conjugate acid, how do I know if I must place the positive hydrogen at the beginning or at the end ?

Thank you!

[Xenonman]

NH₂NH3₃⁺

and it asks me the conjugate base, where am I supposed to place the H⁺

Did you ask what you wanted to ask?

Or if I have the base :

HCOO^- and it asks me what is the conjugate acid, how do I know if I must place the positive hydrogen at the beginning or at the end ?

Inorganic acids usually have the acidic protons at the begginning of their formula. Organic acids usually have them at the end. It may be confusing. Try drawing the HCOO^- and it should no longer be a problem.

[dk_ch]

Hi, I was wondering, if I have an acid like :

NH₂NH3₃<sup>+

and it asks me the conjugate base, where am I supposed to place the H+

Or if I have the base :

HCOO- and it asks me what is the conjugate acid, how do I know if I must place the positive hydrogen at the beginning or at the end ?

Thank you!</sup>

your acid should be NH₂NH₃⁺ and its conjugate base would be NH₂NH₂ ie by eliminating one H⁺
Again the conjugate acid of the base HCOO- should be HCOOH by adding one H⁺

[moop1]

Why isn't it like : NH1NH3

[Borek]

Why isn't it like : NH1NH3

This molecule would be actually ^-HNNH₃⁺ - with negative charge on one end, and positive on the other. While there are molecules that behave this way (they are called zwitterions), they are never symmetrical. This one has a symmetrical, much more stable from H₂NNH₂.

[sjb]

Why isn't it like : NH1NH3

Can you draw a Lewis structure for this? Whilst not completely wrong (there may be a very very small amount of this around), for all intents and purposes NH₂NH₂ is probably more realistic