Solubility combined with Buffer solutions ugh

In summary, the conversation is about calculating the solubility of C6H5COOAg(s) in a buffer solution with a pH of 3.20 using the Henderson-Hasselbach and Ksp equations. The options for the solubility are given as 0,0164M, 0,0050M, 0,0287M, and 0,0012M. The person is struggling to find the correct method and asks for help with their calculations. Another person suggests finding the acid/base ratio first and clarifies that the pH alone cannot determine the concentrations.
  • #1
ultimateguy
125
1

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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  • #2
could you illustrate your workings, maybe there is a calculation error or a way you used your equations wrongly
 
  • #3
What is your buffer concentration? Knowing pH you can only calculate acid/base ratio, not their real concentrations.
 

Related to Solubility combined with Buffer solutions ugh

1. What is solubility?

Solubility refers to the ability of a substance to dissolve in a solvent and form a homogeneous mixture. It is usually measured in terms of the maximum amount of solute that can be dissolved in a given amount of solvent at a specific temperature and pressure.

2. How does solubility affect buffer solutions?

Solubility can impact the effectiveness of a buffer solution as it can affect the concentration of the solutes present. If the solubility of a solute in a buffer solution is low, it may not be able to effectively buffer changes in pH.

3. What is a buffer solution?

A buffer solution is a solution that resists changes in pH when small amounts of acid or base are added. It is composed of a weak acid and its conjugate base, or a weak base and its conjugate acid.

4. How do buffer solutions maintain a constant pH?

Buffer solutions maintain a constant pH by utilizing the principle of Le Chatelier's principle. When an acid or base is added to a buffer solution, the equilibrium between the weak acid and its conjugate base shifts to counteract the change in pH, thus maintaining a relatively constant pH.

5. How does temperature affect solubility in buffer solutions?

Temperature can have a significant impact on the solubility of a solute in a buffer solution. In general, as temperature increases, the solubility of most solids in a solvent also increases. However, this relationship can vary depending on the specific chemical properties of the solute and solvent in the buffer solution.

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