definition of a buffer

[Sue Bin Park 2I]

what exactly is the practical definition of a buffer? wouldn't any solution of a weak acid/base be a buffer because the acid/base and its conjugate would exist in solution? or am i getting this all confused lol

[505306205]

A buffer is a solution that contains both conjugates. In the ICE table, therefore, the starting concentration for the conjugate acid/base is not 0.

[Jordan Young 2J]

A buffer has a weak acid/base and its conjugate so that it can thus resist a chance in pH. You want to have large enough concentrations of both so that it can react if an acid or base is added to the solution

[Joowon Seo 3A]

A buffer has a weak acid/base with its conjugate. The conjugate can take/give a proton in solution, so it can resist a change in pH.

[aishwarya_atmakuri]

A buffer is a solution that resists changes in pH and it’s made by mixing a weak acid/base with its conjugate.

[Hussain Chharawalla 1G]

If you use a weak acid or weak base, wouldn't it's conjugate be a strong base/acid? So if the buffer demands equal concentrations of weak acid and base, how would it be created?

[Sue Bin Park 2I]

If you use a weak acid or weak base, wouldn't it's conjugate be a strong base/acid? So if the buffer demands equal concentrations of weak acid and base, how would it be created?

i'm pretty sure the conjugate seesaw is only relative; if the acid is weakER then its conjugate base is strongER, etc. irl, if you have a weak acid with a conjugate base that is categorized as strong, it would actually mean the weak acid basically doesn't deprotonate. vice versa with a weak base and strong acid. HCl is a strong acid - its conjugate base Cl- ion doesn't protonate period.

it's like a spectrum
strong acid <--B---A----neutral H2O-B---A-----> strong base
a moderately weak acid/moderately weak conjugate base pairing (A and A) will fall equidistant left and right of the neutral H2O centerpoint. if a weak acid is strongER then the acid will be farther from the center and pull the conjugate base closer to the neutral center point, categorizing it as a weaker base (B and B). if an acid is so strong that it is a literal strong acid, that is it completely dissociates, then that means the conjugate base is pulled into the center point (practically) and is effectively neutral in solution/doesn't protonate more than just H2O would on its own.

this push and pull is a result of the fact that the Ka and Kb have to multiply into the Kw constant always.

[Leila_4G]

Also, I'm not sure about the presence of a salt when making a buffer. Can someone please explain that to me? Thanks!

[Emil Velasco 1H]

A buffer solution is an aqueous solution consisting of a mixture of a weak acid and its conjugate base, or vice versa. Its pH changes very little when a small amount of strong acid or base is added to it.