Solubility product by electrometric titration

To determine the solubility of silver chloride in aqueous potassium nitrate bv electrometric titration. 

Electromoti% e force measurements were made on the cells 

The solvent medium was 0.0286 M KNOs- The KCl was added in increments of 4.8440 x 10 moles. The number of increments is denoted by n and the e.m.f. of the cell by E. The volume of solution is taken as 0.338591. Actually its volume increases slightly during the titration, but the recorded values of E have been corrected to take account of this change. 

Ratios of the activity coefficients of KCl in aqueous solutions of various concentrations at 25 °C have been determined by Shedlovsky and Macinnes (J. Amer. Chem, Soc. 1937, 59, 503) by combining measurements of e.m.f. of concentration cdls with independent 

INTRODUCTION We use the following notation s the solubility of AgCl in the KNO3 solution, sx the initial concentration (not accurately known) of AgXOs, sxy the concentration of Ag in /S after addition of n increments of KCl, 

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