anonymous
  • anonymous
Which substance is acting as the Brønsted-Lowry acid in the following chemical reaction? NH4 + OH--> NH3 + H2O
Chemistry
schrodinger
  • schrodinger
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anonymous
  • anonymous
anonymous
  • anonymous
anonymous
  • anonymous
PLEASE HELP, SOMEONE

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anonymous
  • anonymous
@Loser66 being a person of many talent, can you help me out with chem too? or at least fin someone who can?
anonymous
  • anonymous
anonymous
  • anonymous
anonymous
  • anonymous
anonymous
  • anonymous
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)
Photon336
  • Photon336
Bronstead Lowry base is anything that accepts a hydrogen A bronstead Lowry acid is one that produced or loses an H+
Photon336
  • Photon336
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?

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