Asked by Could i plz get some help?

What is the Brønsted-Lowry base in this reaction: NH2−+CH3OH→NH3+CH3O−

A. NH3
B.CH3OH
C.CH3O-
D.NH2-
Answered by DrBob222
Acids give away H. Bases are the ones to which H has been added. Take a look at the two pairs in the equation.
NH2− + CH3OH → NH3 + CH3O−
One pair is the NH2- and NH3.
One pair is the CH3OH and CH3O-
Which of the NH2-/NH3 pair ADDED a H? That's the base. The other part of the pair is the conjugate acid.
Which of the CH3OH/CH3O- pair gave away a H? That's the acid? The other part of the pair is the conjugate base.
See how easy this is?
Answered by Could i plz get some help?
no i dont
Answered by DrBob222
C'mon. Don't be so pessimistic.
It doesn't take a rocket scientist to look at the NH2-/NH3 pair and see that NH2- has ADDED a H to make NH3; therefore, NH2- is the base and NH3 is the conjugate acid. I can see that for the second pair of CH3OH/CH3O- that a H has been TAKEN AWAY FROM CH3OH to make CH3O- which makes CH3OH the Bronsted-Lowry acid and CH3O- the Bronsted-Lowry base. If this is not clear to you please explain to me, in clear detail, what you don't understand about it and I shall gladly spend whatever time is need until you do understand it. It's important so let's do it right.
Answered by Ryan
DrBob222, I understand what you are saying. It's quite simple really. This person needs to get a piece of paper and try to learn this.
Answered by Yourmom
So what's the answer ?
It will really help I'm not smart nor dumb
But I really need help on this one
Answered by Wolfgirl07
Yeah same @Yourmom @~@
I'm so freaking confused... I'll just do it and post the answers in a minute
Answered by Wolfgirl07
Acid-Base Solutions Quick Check
What is the Brønsted-Lowry base in this reaction: NH2−+CH3OH→NH3+CH3O−?
NH2−

What products are formed when HBr and NaOH react in an aqueous solution?
H2O andNaBr

Which compound is an Arrhenius base?
Ca(OH)2

Hydrochloric acid is a strong acid. Acetic acid is a weak acid. Which statement about hydrochloric acid and acetic acid is correct?
The dissociation constant for hydrochloric acid is greater than the dissociation constant for acetic acid.

Which change would decrease the pH of a base in a solution at equilibrium?
decreasing the concentration of OH– ions

I actually did better then I thought I'd do
Anyways here Yall go <3 Love ya~
Answered by Billy Haybottom is gone
1: NH2−
2: H2O andNaBr
3: Ca(OH)2
4: The dissociation constant for hydrochloric acid is greater than the dissociation constant for acetic acid.
5: decreasing the concentration of OH– ions

No more fighting, ok?
Answered by itskim
so confusing
Answered by ouro kronii
wolfgirl07 is the best:) tyty
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