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

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SUMMARY

The solubility of silver chloride (AgCl) in an HCl solution with a pH of 2.30 can be calculated using the solubility product constant (Ksp) of AgCl, which is 1.7 x 10^-10. First, determine the concentration of HCl from the pH, which is approximately 0.005 M. The chloride ion concentration from HCl contributes to the equilibrium, allowing the calculation of the silver ion concentration. This concentration is equivalent to the molar solubility of AgCl, which can then be converted to grams per liter of solution.

PREREQUISITES
  • Understanding of pH and its relation to hydrogen ion concentration
  • Knowledge of solubility product constants (Ksp)
  • Familiarity with equilibrium calculations in chemistry
  • Ability to perform unit conversions (molarity to grams per liter)
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  • Study the calculation of solubility product constants (Ksp) in detail
  • Learn about equilibrium expressions and their applications in solubility
  • Explore the relationship between pH and concentration of strong acids
  • Investigate the conversion methods between molarity and grams per liter
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Chemistry students, educators, and professionals involved in analytical chemistry or solubility calculations will benefit from this discussion.

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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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