Question

help me

Answer 1

1. expalin why soliton # 1 is acidica and # 5 is basic. show chemical equation to support the answer.


2. are either #1 or #5 solutions buffered solutions? Why?

Answer 2

is number 1 acidc because the initial solution prior to adding acid/base is 2.43. solution 5 is basic because the initial solution prior to adding acid/base is 8.37.

Answer 3

show chemical equation to support the answer.

Answer 4

HA<--> H+ + C2H302 for #1

and number 5 will be C2H302 +H2O <-> HA+OH-.

Answer 5

pKa = -Log(Ka)

Answer 6

are those the chemailc eqautions to supprt the answer

Answer 7

pKa is the pH where 50% of a compound is in its conjugated acid and 50% in its conjugated base form

Answer 8

so to answer the question is it

1. explain why solutions # 1 is acidic and # 5 is basic. show chemical equation to support the answer.

is number 1 acidic because the initial solution prior to adding acid/base is 2.43. solution 5 is basic because the initial solution prior to adding acid/base is 8.37

and the chemical equations are


HA<--> H+ + C2H302 for #1

and number 5 will be C2H302 +H2O <-> HA+OH-.

Answer 9

Yeah that seems correct,
Your chemical reaction equations are not written very well though

Answer 10

CH3COOH ⇌ CH3COO- + H+
CH3COO- + H2O ⇌ -OH + CH3COOH

You shouldn't use HA in your reaction equations

Answer 11

CH3COOH equilibrium arrows CH3COO- + H
CH3COO- + H2O equilibrium arrows -OH + CH3COOH

Answer 12

I don't like to use this arrow <--> because this is the arrows used to denote resonance.

Answer 13

https://en.wikipedia.org/wiki/Buffer_solution

Answer 14

read the first paragraph of the Wikipedia article

Answer 15

is acetic acid a weak acid?

Answer 16

the definition of a buffer is just a solution of a weak acid in a equilibrium with its conjugate weak base

Answer 17

The answer is:

it is a weak acid, a weak acid is normally defined as a compound that does not completely dissociate in water into its conjugate base, thus there is a mix of acetic acid (CH3COOH) and its conjugate base (CH3COO-) in solution. pKa lets you know at what pH that acetic acid is split 50/50 between these two forms, thus making pKa a good indication of a compounds acidity/basicity in water.

Remember acidity and basicity is environment dependent just because something is acidic in water doesnt mean it is a acidic in a vacuum or benzene etc..

Answer 18

pretty much, so you know the answer to your question now and you hardly even needed my help

Answer 19

if you are confused about a term just enter it into a search engine this is basic chemistry there are countless resources that explain this material, not to discourage you from asking questions on this site.

Answer 20

We established that Acetic acid is weak acid
its conjugate base is a weak base read the definition of a buffer solution again

Answer 21

I'm sorry this confuses me just as much as it does you..

Answer 22

this is as much as i can tell you.
The whole point of a buffer solution is that the ph doesn't change much. #5 changes a lot so I would consider it a buffer solution. I'm not sure what the actual bounds of a buffer system are its been awhile

Answer 23

I'm sorry...I'm not familiar with this. Infact, it confuses me :/

Answer 24

I posted the formula above that expresses Ka in terms of pKa

Answer 25

are either #1 or #5 solutions buffered solutions? Why?

so i said solution 1 would be a buffer solution because a buffer solution is one which resists changes in pH when small quantities of an acid are added to it which changes slightly.

for solution 5, the pH after the HCl was added to it changed a lot, which is not considered a buffer solution.

is that right

Answer 26

kkutie is not right

right she put
The whole point of a buffer solution is that the ph doesn't change much. #5 changes a lot so I would consider it a buffer solution. I'm not sure what the actual bounds of a buffer system are its been awhile

Answer 27

so i said solution 1 would be a buffer solution because a buffer solution is one which resists changes in pH when small quantities of an acid are added to it which changes slightly.

for solution 5, the pH after the HCl was added to it changed a lot, which is not considered a buffer solution.


so this is not right

Answer 28

http://en.wikipedia.org/wiki/Buffer_solution#Principles_of_buffering

Answer 29

are you postive

Answer 30

No actually you are right they are both not buffer solutions by the definition of a buffer solution which I showed you earlier

Answer 31

Buffer Definition:
A buffer is a solution containing either a weak acid and its salt or a weak base and its salt , which is resistant to changes in pH .

Answer 32

Both only contain an acid or a conjugate base (salt)

Answer 33

they do not contain a mix of both so you can say that they are not buffer solutions

Answer 34

Solution 5 will become a buffer solution though after addition of HCl though but initially they are both not regarded as buffer solutions based on the definition

Answer 35

Please reframe from spamming me in the future I have my own work to do/life I will help you when I have time.

Answer 36

sleep time now