For C2H5NH3+, write an equation that shows how the cation acts as an acid.
Why is my answer wrong?
CH2H5NH3^+(aq) + H2O(l) ---> CH2H5NH2(aq) + H3O+(aq)
Its C2H5 and not CH2H5
Ethylamine, which you have represented as an acid, is a very weak base. The reaction that you wrote should be reversible.
You do have a typo.
CH2H5NH3^+(aq) + H2O(l) ---> CH2H5NH2(aq) + H3O+(aq)
CH5NH3^+(aq) + H2O(l) <---> CH5NH2(aq) + H3O+(aq)
Sorry, don't know how to type half arrows on this forum.
CH2H5NH3^+(aq) + H2O(l) ---> CH2H5NH2(aq) + H3O+(aq)
C2H5NH3^+(aq) + H2O(l) <---> C2H5NH2(aq) + H3O+(aq)
Sorry, don't know how to type half arrows on this forum
And I am just all over the place......
Well, it looks like your answer is wrong because you forgot to add the water molecule to the equation! Thankfully, I'm here to help. Let me fix it for you:
C2H5NH3+(aq) + H2O(l) ⟶ C2H5NH2(aq) + H3O+(aq)
See, the cation (C2H5NH3+) is acting as an acid by donating a proton (H+) to water, forming the ethylamine molecule (C2H5NH2) and the hydronium ion (H3O+). Don't worry, chemistry can be a balancing act sometimes!
Your answer is correct. The equation you provided correctly shows how the cation, C2H5NH3+, acts as an acid.
C2H5NH3+ is actually the conjugate acid of the base C2H5NH2 (ethylamine). When the cation donates a proton (H+) to water, it forms the conjugate base C2H5NH2 and generates the hydronium ion, H3O+.
It's possible that you were told your answer was wrong due to a typo or misunderstanding. Double-check the question and consult with your instructor or textbook to confirm if there was a mistake.