Question

Question about BUFFERS!

Answer 1

@Mertsj

Answer 2

@ParthKohli

Answer 3

@ParthKohli

Answer 4

@Zarkon

Answer 5

Shoot!

Answer 6

do you know about buffers

Answer 7

Maybe I can help, maybe I can't, but if you ask the question I will try to help.

Answer 8

Does a buffer have unlimited capacity to neutralize a base? How about an acid? explain

Answer 9

No, it does not have unlimited capacity. Eventually, you can overload it.

Answer 10

Can you explain why for both please

Answer 11

A buffer is so-called because it resists a change in pH. You add acid, it neutralizes with a base. You add base, and it neutralizes with the conjugate acid. As long as there is base or conjugate acid (or vice versa), you will be hardly changing the pH. Once you have used up the acid or base being used in the neutralization, you no longer have a buffer solution, and your pH will change like usual.

Answer 12

ok i have one column for the acid part and one column for the base. can you tell me what to write in each one :)

Answer 13

i have an F in chemistry

Answer 14

24%

Answer 15

also i have a question how do you do net ionic equations backwards

Answer 16

One thing at a time, we'll get it right.

Basically, if you are adding acid to a buffer (which is an acid/base combination), there exists base in the solution that neutralizes/nullifies/cancels out the incoming acid. This will continue until the buffer base runs out.

If you are adding base to a buffer (acid/base combo again), there exists enough acid in that solution that neutralizes/nullifies/cancels out the incoming base. This will continue until the buffer acid runs out.

Ok now?

Answer 17

wow that was really good!!!!!!!

Answer 18

i have more questions if you are able to answer

Answer 19

OK, I am helping another person at the same time, I'll do my best. There may be a little delay though.

Answer 20

Question 1: If OH- ions are added to a buffer, what will they react with?

Answer 21

Question2: If H3O+ ions are added to a buffered system, what wil they react with ?

Answer 22

A1: If OH- ions (this is a base) are added to a buffer, they will react (be neutralized) with the buffer's conjugate acid.

A2: H3O+ ions added to a buffer will react with a buffer's conjugate base.

Answer 23

you are awesome, man!!

Answer 24

i have more question please

Answer 25

go ahead

Answer 26

write the balanced equation, total ionic and net ionic equation for the neutralization reaction that produce the following salt : BaSO4

Answer 27

adastra = god

Answer 28

Neutralization means you will have: Acid + Base -> BaSO4 + H2O
H2SO4(aq) + Ba(OH)2(aq) -> BaSO4(s) + 2 H2O(aq)

This is actually a little tricky: BaSO4 is practically insoluble in water, so it will be a solid in this reaction.

Total ionic equation (break up the aqueous phase compounds into respective ions):
2 H^1+(aq) + SO4^2-(aq) + Ba^2+(aq) + 2 OH^1-(aq) -> BaSO4(s) + 2 H^1+(aq) + 2 OH^1-(aq)

Net ionic equation (cancel out everything from above that appears "exactly" on both sides):
SO4^2-(aq) + Ba^2+(aq) ->BaSO4(s)

Answer 29

wow you are good at this. how about Rb Clo4

Answer 30

Like the last one, only all charges are either +/-1 so it's a little simpler:

RbOH(aq) + HClO4(aq) -> RbClO4(s) + H2O(aq)
Rb^1+(aq) + OH^1-(aq) + H^1+(aq) + ClO4^1-(aq) -> RbClO4(s) + H^1+(aq) + OH^1-(aq)
Rb^1+(aq) + ClO4^1-(aq) -> RbClO4(s)

Answer 31

thanks. i will be right back please stay online if u can

Answer 32

a little while longer

Answer 33

why is ba oh 2 aqueous

Answer 34

It is slightly soluble, so it will dissolve in water and break up into Ba^2+ and OH^1- ions

Answer 35

why soluble. solubility rules say otherwise

Answer 36

I looked it up. It is slightly soluble in water at room temperature.

Answer 37

EXCUSE ME. BUT H20 is not aqeuis. its a liquid.

Answer 38

water does not dissolve in water...

Answer 39

OK, so some of the balanced ionic and net ionic reactions would change. The products for both would have H2O(l) instead of H^1+ and OH^1- ions.

Answer 40

so then for the first one how do you even cancel anything out. .

Answer 41

Very good, right, nothing would change.
Balanced ionic equation = net ionic equation

Answer 42

UGH I HATE MY LIFE

Answer 43

Sorry about that mistake.

Answer 44

no i just hate my life in general because i have to take chemistry.

Answer 45

are you in ap chemistry

Answer 46

Well, I actually am in my first year teaching high school chemistry.

Answer 47

omg you are an adult? wait i have talked to you on here before right

Answer 48

actually rboh is solid and rbclo4 is aqueous.