i would like to see if my reasoning is correct (for aq. solutions): [tex]2HBr_(aq_) + 2NH_3_(aq_) -> 2NH_4_(aq_) + Br_2_(aq_) [/tex] HBR is an acid so it gives H to NH3, which leaves Br all alone. But Br can't exist by itself, so it becoems Br2? ionic: [tex]2H^+_(aq_) + 2Br^-_(aq_) + 2NH^-_3_(aq_) -> 2NH^+_4_(aq_) + 2Br^-_(aq_) [/tex] net ionic: [tex]2H^+_(aq_) + 2NH^-_3_(aq_) -> 2NH^+_4_(aq_) [/tex] Also, I have a question about water and its presence or lackthereof in net ionic equations (for aq. solutions). I have [tex]2HClO_4_(aq_) + Mg(OH)_2_(s_) -> Mg(ClO_4)_2 (s) + 2H_2O[/tex] ionic: (matter states are same as above)[tex]2H^+ + 2CLO^-_4 + Mg^+^2 + 2OH^- -> Mg(ClO_4)_2 + 2H^+ + 2OH^- [/tex] but that last part is really [tex]2H_2O[/tex]. But if i write it like that, then in my net equation i gotta keep [tex]H_2O[/tex] and the H and OH ... making my net equation the same as my ionic equation. That seems wrong to me. Is there a covention where I can write [tex]2H_2O[/tex] and still leave out OH and H as spectator ions in my net ionic equation? Thank you for your time.