Question

(Na2CO3 / H2CO3) >>> Is this a buffer solution ?

Answer 1

For our buffer, we have
HCO3- + H3O+ <---> H2CO3 + H2O

Think about the equilibrium. Then think about the shift if small amounts of either strong acid or strong base were added, using Le Chatelier's principle to help you out.

We know that
[H3O+] = Ka(acid) * [acid/base]

Say we added some strong acid (e.g.: HCl). This would cause the equilibrium to shift right, thus increasing the [ ] H2CO3. However, because only a small amount of strong acid was added, according to the equation above, the ratio between acid and base will still be roughly the same as before and thus, [ H3O+] and consequently, the pH of solution will remain fairly constant. Same thing if a strong base (e.g.: NaOH) was added.

Try to figure it out from there.

Answer 2

I have a miss understand @_@

Answer 3

what do you mean

Answer 4

I think to determined this solution is a buffer or not you should to know if this solution is
1- A weak acid with its conjugate base
2- A weak acid (excess) with a strong base
3- A weak base with its conjugate acid
4- A weak base ( excess ) with strong acid

Answer 5

What the shrek are you talking about @blanderos24 ?????
By definition, a buffer is a solution that contains either 1. weak acid/weak base and it's salt

to find what you need for buffers, you can simply use the henderson-hasselbach equation!

Answer 6

a buffer is able to resist pH change. THATs the key! Why? because it contains conjugate acid/conjugate base which are both present at equilibrium. hence, it is able to neutralize small amounts of other acids/bases.