An electrode was constructed in lab that measures equilibrium silver ion concentrations in solutions saturated with particular insoluble silver salts such as AgCl(s). Effective measurement of the silver ion at these trace levels requires that the ionic strength of the solutions in which Ag+ is measured be held constant. a) b) In Step 1 of the experiment, 10.0 mL of a solution containing 0.0010 M AgNO3 and 0.100 M NH4NO3 is diluted to 100.00 mL in a volumetric flask. What is the resulting ionic strength of this solution? To the 100.00 mL solution made in Step 1,10.00 mL of a solution containing 0.0100 M NH4 acting as the limiting reagent. Cl is added. Verify that the ionic strength has in fact been kept constant, assuming that stoichiometric amounts of AgCl are formed with Ag+ acting as the limiting reagent.
An electrode was constructed in lab that measures equilibrium silver ion concentrations in solutions saturated with particular insoluble silver salts such as AgCl(s). Effective measurement of the silver ion at these trace levels requires that the ionic strength of the solutions in which Ag+ is measured be held constant. a) b) In Step 1 of the experiment, 10.0 mL of a solution containing 0.0010 M AgNO3 and 0.100 M NH4NO3 is diluted to 100.00 mL in a volumetric flask. What is the resulting ionic strength of this solution? To the 100.00 mL solution made in Step 1,10.00 mL of a solution containing 0.0100 M NH4 acting as the limiting reagent. Cl is added. Verify that the ionic strength has in fact been kept constant, assuming that stoichiometric amounts of AgCl are formed with Ag+ acting as the limiting reagent.
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