Which substance is acting as the Brønsted-Lowry acid in the following chemical reaction?
NH4 + OH--> NH3 + H2O
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being a person of many talent, can you help me out with chem too? or at least fin someone who can?
I WILL FAN WHOEVER HELPS ME AND GIVE A MEDAL! PLS HELP! On a practice exam and this is the only one I don't know how to do 8)
Bronstead Lowry base is anything that accepts a hydrogen
A bronstead Lowry acid is one that produced or loses an H+
NH4+ -----> NH3
We write our what's going on for each ion: we can clearly see that NH4+ is losing a hydrogen.
[NH3][H+]/[NH4+] = Ka
Now whenever an acid loses a proton it becomes its conjugate base. Above was the Ka acid dissociation constant.
OH- -----> HOH
OH- is gaining a proton to become water, Because it's taking a proton from NH4+
[HOH]/[OH-][H+] = Kb this is our Kb.
Whenever a base gains a proton it becomes its conjugate acid.
So based off of this what do you think the bronstead Lowry acid and base are based off of the description?