explain how the buffer H2CO3 neutralizes a base that is added to a solution that contains it. If the pH of the solution was 5.0 before the base was added, what would it be after the base was added?

Question

anonymous · Answer

this question is different

ash2326 · Answer

pH<7 => acidic
pH>7=> basic solution
if pH was 5 earlier, if we add a base then what do you think would happen?

anonymous · Answer

be less acidic ?

anonymous · Answer

i for the most part understand it i think i just cant figure out how to explain it

anonymous · Answer

could you explain it all to me please :)

ash2326 · Answer

A base adds more $OH^{-}$ ions to the solution
We had an acidic solution earlier
Acidic solution have $H^{+}$ ions
when we added base, the  $OH^{-}$ ions combined with $H^{+}$ ions of our original solution to form $H_2O$ , which is neutral.
For Finding the pH, we need the no. of moles of base and acidic solutions.
We don't have this data, but we could certainly say that $H^+$ ions will diminish in number, so the pH will increase

ash2326 · Answer

do you get thus @needhomeworkhelp ?

vincent-lyon.fr · Answer

The buffer must be a mixture of $H_2CO_3$and $HCO_3^-$

When a base is added, let's say a strong base, then the following reaction will take place:

$H_2CO_3+OH^- \rightarrow HCO_3^- + H_2O$

This will change the amounts of carbonic acid and hydrogencarbonate ions in the solution, but the pH will increase only slightly.