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28 Sep 2019
25.00 mL of 0.100 M AgNO3 are mixed with 35.00 mL of 0.0500 MK2CrO4. Calculate the concentrations of each ionic specie (Ag + ,NO3 - , K + , CrO4 2- ) at equilibrium. Is the precipitation ofsilver chromate quantitative (we define quantitative for thisproblem when 99.9% or more has precipitated)? Ksp Ag2CrO4 = 1.1 x10 -12.
I'm not sure exactly how to do this question.
Am I suppose to find the concentrations for the ions in terms ofmoles? Then find the Qsp of silver nitrate and compare it to theKsp to determine whether the precipitate is quantitative?
25.00 mL of 0.100 M AgNO3 are mixed with 35.00 mL of 0.0500 MK2CrO4. Calculate the concentrations of each ionic specie (Ag + ,NO3 - , K + , CrO4 2- ) at equilibrium. Is the precipitation ofsilver chromate quantitative (we define quantitative for thisproblem when 99.9% or more has precipitated)? Ksp Ag2CrO4 = 1.1 x10 -12.
I'm not sure exactly how to do this question.
Am I suppose to find the concentrations for the ions in terms ofmoles? Then find the Qsp of silver nitrate and compare it to theKsp to determine whether the precipitate is quantitative?
I'm not sure exactly how to do this question.
Am I suppose to find the concentrations for the ions in terms ofmoles? Then find the Qsp of silver nitrate and compare it to theKsp to determine whether the precipitate is quantitative?
Nestor RutherfordLv2
28 Sep 2019
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