Chapter 17, Problem 17.113QP

An analytical chemist has a solution containing chloride ion, Cl⁻. She decides to determine the amount of chloride ion in the solution by titrating 50.0 mL of this solution by 0.100 M AgNO₃. As a way to indicate the endpoint of the titration, she added 1.00 g of potassium chromate, K₂CrO₄ (see Figure 17.5). As she slowly added the silver nitrate to the solution, a white precipitate formed. She continued the titration, with more white precipitate forming. Finally, the solution turned red, from another precipitate. The volume of the solution at this point was 60.3 mL. How many moles of chloride ion were there in the original solution? How many moles of chloride ion were there in the final solution? You may make any reasonable approximations.