How Do You Calculate the Solubility of AgCl in an HCl Solution with pH 2.30?

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To calculate the solubility of AgCl in an HCl solution with a pH of 2.30, first determine the concentration of HCl, which is approximately 0.005 M. Using the Ksp of AgCl (1.7 x 10^-10), the concentration of Cl- from HCl can be used to find the Ag+ concentration. The solubility product expression allows for solving the molar solubility of AgCl, which is equivalent to the Ag+ concentration. Finally, convert the molar solubility to grams per liter to obtain the final solubility value.
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[SOLVED] equilibirum and solubility product

I need some help with this question, if there are any chemistry whizzes around id really appreciate it:

Calculate the solubility of AgCl (in grams of AgCl/ L of solution) in an HCl solution having pH of 2.30. Ksp of silver chloride = 1.7 x 10^-10.
 
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so far all i can tell is that from the ph u get the concentration of HCL, then...im lost
 
ok i got some help, apparently u use the cl concentration from hcl and the ksp and solve for Ag conc. which should be same as the molar solubility for in mol/l of AgCl then just convert. thanks for any help or good intentions.
 

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