Answer:
Net Ionic equation
NH₄⁺ + OH⁻ → NH₃ + H₂O
Option B is correct.
Weak Acid Strong Base
Check Explanation for the extent of the reaction.
Explanation:
Ammonium nitrate = NH₄NO₃
Potassium Hydroxide = KOH
Ammonium salts combine with alkalis to liberate NH₃ and form water.
The two reactants combine to give
NH₄NO₃ + KOH → KNO₃ + NH₃ + H₂O
In ionic form,
- NH₄NO₃ exists as NH₄⁺ and NO₃⁻
- KOH exists as K⁺ and OH⁻
- KNO₃ as K⁺ and NO₃⁻
And NH₃ and H₂O stay as they are, as per covalent compounds.
So, we have
NH₄⁺ + NO₃⁻ + K⁺ + OH⁻ → K⁺ + NO₃⁻ + NH₃ + H₂O
Eliminating the ions that exist on both sides, we have the net ionic equation to be
NH₄⁺ + OH⁻ → NH₃ + H₂O
which shows that this reaction is essentially a neutralization reaction in which the Bronsted Lowry acid, NH₄⁺, loses its proton to the base, OH⁻ and gives conjugate base, NH₃ and conjugate acid, H₂O.
This reaction is classified as a Weak acid versus Strong Base reaction as NH₄⁺ is from a Weak acid and OH⁻ is from a strong base.
Since this reaction is between a Weak base and a strong acid, the ionization isn't expected to be 100%, Hence, the extent of this reaction will be any option that is not 100%, a couple pieces of information might be required for the correct estimate, but above 50% seems correct.
Hope this Helps!!!
is a Lewis acid due to the unfilled valence shell on carbon atom (possessing positive charge) it accepts electron readily.
is not a Lewis acid due to the presence of negative charge which represents that there are electrons available for donation.
is not a Lewis acid due to the presence of lone pair on nitrogen which is easily donated to the acceptors.
is a Lewis acid due to the availability of vacant p-orbital on boron atom.