# Is mixture of ammonium hydroxide and ammonium nitrate a buffer solution? [closed]

Is a mixture of $$\ce{NH4OH}$$ and $$\ce{NH4NO3}$$ a buffer solution?

I have seen some examples with $$\ce{NH4OH}$$ and $$\ce{NH4Cl}$$ but never $$\ce{NH4NO3}$$.

• There should be no difference. Both are salts of strong acids, so... – Ivan Neretin Mar 29 at 11:13
• NH4OH does not exist as a molecule in water. There is NH3(aq), reacting with water $\ce{NH3(aq) + H2O <<=> NH4+(aq) + OH-(aq)}$. In extreme conditions, like in interstellar space, it may exist as a donor-acceptor pair NH3.H2O – Poutnik Mar 29 at 12:29

Is a mixture of $$\ce{NH4OH}$$ and $$\ce{NH4NO3}$$ a buffer solution? I have seen some examples with $$\ce{NH4OH}$$ and $$\ce{NH4Cl}$$ but never $$\ce{NH4NO3}$$.
Both mixtures contain $$\ce{NH4+}$$, a weak acid. Where is the conjugate weak base? You can either write $$\ce{NH4OH}$$ more conventionally (or in a more modern way) as ammonia in aqueous solution, $$\ce{NH3(aq)}$$, which is a weak base. Or you can recognize $$\ce{OH-}$$ in ammonium hydroxide as a strong base, which would react with the ammonium to make ammonia. In either way of looking at things, the conjugate base is present as well.