Nhen a 100.0-mL portion of a solution containing 0.500 g of AGNO3 is mixed with 100.0 mL of a solution containing 0.300 g of K2CrO4, a bright red precipitate of Ag2CrO4 forms. (a) Assuming that the solubility of Ag2CrO4 is negligible, calculate the mass of the precipitate. Ans. The limiting reagent is the mass of the precipitate is g. (b) Calculate the mass of the unreacted component that remains in solution. Ans. The mass of the unreacted component is Submit tl

Fundamentals Of Analytical Chemistry
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Author:Skoog
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Chapter12: Gravimetric Methods Of Analysis
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When a 100.0-mL portion of a solution containing 0.500 g of AgNO3 is mixed with 100.0 mL of
a solution containing 0.300 g of K2CrO4, a bright red precipitate of Ag2CrO4 forms.
(a) Assuming that the solubility of Ag2CrO, is negligible, calculate the mass of the precipitate.
Ans. The limiting reagent is
the mass of the precipitate is
g.
(b) Calculate the mass of the unreacted component that remains in solution.
Ans. The mass of the unreacted component is
Transcribed Image Text:When a 100.0-mL portion of a solution containing 0.500 g of AgNO3 is mixed with 100.0 mL of a solution containing 0.300 g of K2CrO4, a bright red precipitate of Ag2CrO4 forms. (a) Assuming that the solubility of Ag2CrO, is negligible, calculate the mass of the precipitate. Ans. The limiting reagent is the mass of the precipitate is g. (b) Calculate the mass of the unreacted component that remains in solution. Ans. The mass of the unreacted component is
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