with 65.0 mL of 0.0150M AgNO3?
- write the double displacement to identify the slightly soluble salt (the precipitate)
- silver chloride in the example
- determine the concentration of the ions of the slightly soluble salt using c1V1=c2V2
- Cl and Ag in this example
- for Cl: (0.0350L)(0.0100M)=c2(0.100L*);
- * 35mL + 65mL = 100mL = 0.100L
- Write the llbm equation for the slightly soluble salt then the Ksp expression
- Use the calculated concentrations, sub into Ksp to determine a "trial K"
- compare "trial K" to real K (from Ksp chart)
- if trial K less than real K = no precipitate (not enough of the ions present to cause a ppt to form)
- if trial K greater than real K = ppt (too great of an amount of the ions in the solution - excess ppts out)
