OpenStudy (anonymous):

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?

4 years ago
thomaster (thomaster):

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

4 years ago
OpenStudy (anonymous):

Oh, alright! Thankyou!

4 years ago
OpenStudy (anonymous):

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.

4 years ago
OpenStudy (anonymous):

@Abhisar

4 years ago
OpenStudy (somy):

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

4 years ago
OpenStudy (somy):

2

4 years ago
OpenStudy (somy):

3

4 years ago
OpenStudy (somy):

4

4 years ago
OpenStudy (somy):

5

4 years ago
OpenStudy (somy):

and las tiny part

4 years ago
OpenStudy (somy):

hope that helps :)

4 years ago
OpenStudy (anonymous):

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

4 years ago
OpenStudy (anonymous):

@aaronq

4 years ago
OpenStudy (somy):

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

4 years ago
OpenStudy (anonymous):

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?

4 years ago
OpenStudy (somy):

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

4 years ago
OpenStudy (somy):

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

4 years ago
OpenStudy (somy):

how can it neutralize it without bonding to it?

4 years ago
OpenStudy (aaronq):

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 $$HCl+CH_3COO^-\rightarrow Cl^-+CH_3COOH$$

4 years ago
OpenStudy (somy):

Cl- is conjugate base??

4 years ago
OpenStudy (anonymous):

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...

4 years ago
OpenStudy (anonymous):

Sorry, openstudy was being extremely laggy.

4 years ago
OpenStudy (aaronq):

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

4 years ago
OpenStudy (anonymous):

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?

4 years ago
OpenStudy (somy):

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

4 years ago
OpenStudy (aaronq):

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

4 years ago
OpenStudy (anonymous):

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.

4 years ago
OpenStudy (somy):

OS app is so slow (*￣m￣)

4 years ago
OpenStudy (anonymous):

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

4 years ago
OpenStudy (somy):

i'd go with B though

4 years ago
OpenStudy (somy):

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

4 years ago
OpenStudy (anonymous):

Yeah, I'm gonna go with B too.

4 years ago
OpenStudy (somy):

hope its right :3

4 years ago