Solubility combined with Buffer solutions ugh

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    Buffer Solubility
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To calculate the solubility of C6H5COOAg in a buffer solution with a pH of 3.20, the Henderson-Hasselbalch equation and Ksp must be applied correctly. The user struggled with obtaining the correct concentration of C6H5COO, indicating potential calculation errors or misapplication of equations. Clarification on the buffer concentration is necessary, as pH alone does not provide complete information about acid/base concentrations. Engaging in equilibrium problems may also be beneficial for solving the solubility challenge. Accurate calculations and a thorough understanding of the buffer system are crucial for determining the solubility in this context.
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Homework Statement


Calculate the solubility of C6H5COOAg(s) in a buffer solution that has a pH of 3.20. (Ka = 6,5 x10^-5M ; Ksp = 2,5 x10^-5M^2)
a) 0,0164M
b) 0,0050M
c) 0,0287M
d) 0,0012M


Homework Equations



Henderson-Hasselbach, Ksp equation

The Attempt at a Solution



This is driving me nuts. I used Henderson-Hasselbach to find [C6H5COO], wrong answer, tried an equilibrium problem, wrong answer. Can someone give me a method for this. Thanks.
 
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could you illustrate your workings, maybe there is a calculation error or a way you used your equations wrongly
 
What is your buffer concentration? Knowing pH you can only calculate acid/base ratio, not their real concentrations.
 

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