A silver nitrate soln was standardized by dissolving 0.54 grams of NaCl (MW=58.4

Question

A silver nitrate soln was standardized by dissolving 0.54 grams of NaCl (MW=58.45) into 120 mL of soln using 1.0M K2CrO4 for an indicator (1mL=20 drops) Upon titration with 43.6 mL of AgNO3, the AgCrO4 just began to precipitate. At this point in the titration the system reches equilibrium and therefore Qsp for silver chromate is equal to Ksp of silver chromate and Qsp for silver chloride is equal to Ksp for AgCl.

1. Cal the equilibrium concentration for the chromate ion [CrO4^2-] , [Ag+] , [Cl-]

2. Cal the percent Cl- remaining in soln.

3. Cal the molarity of the AgNO3 soln used.

Explanation / Answer

Because of the precipitating titration based upon utilizing silver nitrate

(AgNO3

) as a precipitating agent, then it called " argentimetric

processes ".

molarity of nacl=0.07

KSP =[Ag

+

]

2

[CrO

4

-2

]

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