Question

Medal and fan

How does a buffer work?
A. It neutralizes acids and bases by precipitating a salt
B. It bonds with the added H+ and OH- in a solution
C. It forms new conjugate pairs with the added ions
D. It prevents added acids and bases from dissociating.

Wouldn't it be D since a buffer neutralizes the reaction and attempts to keep the pH from moving?

Answer 1

A buffer neutralizes small amounts of other acids and bases in the form of \(\sf H_3O^+\)and \(\sf OH^-\)
The exact mechanism is explained in this article: http://chemcollective.org/activities/tutorials/buffers/buffers3

Answer 2

Oh, alright! Thankyou!

Answer 3

Wait, I guess I'm still confused when contemplating the answers. Would it be D still like I said? I read the article and I'm still weighing towards that answer.

Answer 4

@Abhisar

Answer 5

ok idk this but i'll post whats written in my book
1

Answer 6

2

Answer 7

3

Answer 8

4

Answer 9

5

Answer 10

and las tiny part

Answer 11

hope that helps :)

Answer 12

Kinda. Like, I understand that. I just don't see where it fits in with those answers.

Answer 13

@aaronq

Answer 14

from what i gave you and read myself
im kinda thinking is B though

Answer 15

It doesn't bond to it though does it? I just thought it neutralizes it. Does it have to bond to them to neutralize it?

Answer 16

coz it does form bonds with H+ ions and then because H+ ions are becoming more thus according Le Chatlier's principle the equilibrium position shifts to minimize the change

Answer 17

i think it does have to bond to it
( well thats what im reading and it kinda makes sense to me)

Answer 18

how can it neutralize it without bonding to it?

Answer 19

I think it's both B and C

B for obvious reasons.. it forms chemical bonds

C because any acid-base reaction forms new conjugate pairs. Say if you have an acetate buffer and you add some HCl

\(HCl+CH_3COO^-\rightarrow Cl^-+CH_3COOH\)

Answer 20

Cl- is conjugate base??

Answer 21

Cl is a conjugate base @somy cause the Hcl was the acid and gave and CH3COOH a hydrogen ion.

It can only be one answer though...

Answer 22

Sorry, openstudy was being extremely laggy.

Answer 23

i dont know, multiple answers fit the description. flawed question

Answer 24

I don't understand why it couldn't be D if it stops the ADDED bases and acids from dissociating. Wouldn't that keep the pH neutralized?

Answer 25

is't more of equilibrium reaction??? i mean addition of acid would mean that H+ ions are increased thus equilibrium will favor CH3COOH production
and addition of OH- , it will react with H+ ion in the equilibrium and thus cause formation of water so now less H+ ions are there thus equilibrium shifts to favor H+ production

Answer 26

D is wrong, that's not how a buffer works. It doesnt stop the dissociation but it scoops up \(H^+\)'s or \(OH^-\)'s.

Answer 27

Which answer would you lean towards most? I can always prove an argument with my teacher. The system has a lot of flawed questions and I usually have to go back for questions I missed and justify why my answer is more correct than the one the system deems correct.

Answer 28

OS app is so slow (*￣m￣)

Answer 29

It would probably be looking for B then. C could be in any acid/base reactions, not just with buffers.

Answer 30

i'd go with B though

Answer 31

yeah well and again i learnt something new :3 thnx :*

Answer 32

Yeah, I'm gonna go with B too.

Answer 33

hope its right :3