[galaxy13]

The % ionization of a weak acid always declines in a solution that contains the salt of the anion, relative to a solution of the acid alone. For example, the % dissociation of acetic acid is less in a solution that contains sodium acetate than if the acetic acid were alone. Verify this for a 0.5 M solution of acetic acid and 0.5 M each acetic acid/acetate, and explain why.

[Borek]

Please read forum rules.

[AWK]

Just calculate degree of dissociation for both solution and compare results

[galaxy13]

Please read forum rules.

What is wrong?

[Borek]

4. Please show that you've at least attempted the problem. We don't mind helping you solve problems but we are ethically opposed to doing homework for you.

[galaxy13]

I suppose I have to write two equations, one for each of the solutions. But I can't understand how these equations are different.

[AWK]

for the acid degree of dissocistion is SQRT(K/c) (c of acid)
for the buffer -  K/c (c of salt)
You have the same both: c of acid and c of salt

These are quite different equations