Respuesta :
Hydroxylamine in water: HONH₂(aq) + H₂O(l) ⇄ HONH₃⁺(aq) + OH⁻(aq).
Hydroxylammonium nitrate in water: HONH₃NO₃(aq) → OHNH₃⁺(aq) + NO₃⁻(aq).
1) with positive hydrogen ions (protons) react base and gives weak conjugate acid:
H⁺(aq) + HONH₂(aq) ⇄ HONH₃⁺(aq).
2) with hydroxide anions react acid and produce weak base and weak electrolyte water:
HONH₃⁺(aq) + OH⁻(aq) ⇄ HONH₂(aq) + H₂O(l).
Hydroxylammonium nitrate in water: HONH₃NO₃(aq) → OHNH₃⁺(aq) + NO₃⁻(aq).
1) with positive hydrogen ions (protons) react base and gives weak conjugate acid:
H⁺(aq) + HONH₂(aq) ⇄ HONH₃⁺(aq).
2) with hydroxide anions react acid and produce weak base and weak electrolyte water:
HONH₃⁺(aq) + OH⁻(aq) ⇄ HONH₂(aq) + H₂O(l).
Answer : When hydroxylamine is dissolved along with hydroxylammonium nitrate to prepare a buffer into water.
The chemical equation that can represent this reaction is -
- [tex]HONH_{2}[/tex] + [tex]H_{2}O[/tex] ⇔ [tex]HONH_{3}^{+}[/tex] + [tex]OH^{-}[/tex]
- [tex]HONH_{3}NO_{3}[/tex]⇔ [tex] OHNH_{3}^{+} + NO{3}^{-}[/tex]
This is the buffer which will resists the changes when an acid or base is added to this solution.
- Acid addition [tex]H^{+}[/tex]
[tex]HONH_{2} + H^{+} [/tex] → [tex] HONH_{3}^{+} [/tex]
When an acid is added to this buffer solution the extra [tex]H^{+}[/tex] will be converted into hydroxylammonium ion (which is a weak conjugate acid).
- When adding [tex]OH^{-}[/tex]
[tex]HONH_{3}^{+} + OH^{-}[/tex] → [tex] HONH_{2} + H_{2}O[/tex]
when a base it added to the buffer it stabilizes the extra [tex]OH^{-}[/tex] ions in the solution by converting them into hydroxylamine (which is weak base) and water molecules.