When 200.0 mL of a solution containing 0.4522 g of AgNO3 is mixed with 100.0 mL of a solution containing 0.1668 g of K2CRO4, a bright red Ag2CrO4 precipitates. a. Identify the limiting reagent. b. Calculate the mass of the precipitate. c. Calculate the mass of the unreacted AgNO3 or K2CrO4 that remains in solution.
When 200.0 mL of a solution containing 0.4522 g of AgNO3 is mixed with 100.0 mL of a solution containing 0.1668 g of K2CRO4, a bright red Ag2CrO4 precipitates. a. Identify the limiting reagent. b. Calculate the mass of the precipitate. c. Calculate the mass of the unreacted AgNO3 or K2CrO4 that remains in solution.
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Transcribed Image Text:When 200.0 mL of a solution containing 0.4522 g of AgNO3 is mixed with 100.0 mL
of a solution containing 0.1668 g of K2CRO4, a bright red Ag2CrO4 precipitates.
a. Identify the limiting reagent.
b. Calculate the mass of the precipitate.
c. Calculate the mass of the unreacted AgNO3 or K2CrO4 that remains in solution.
5. A series of sulfate samples is to be analyzed by precipitation as BaSO4. To obtain
four significant digits at least 0.1000 g BaSO4 should be obtained.
a. If the sample contains at least 10% sulfate by weight, what is the minimum
sample mass that can be used?
b. If this amount is used and the sample turns out to actually contain 42% sulfate,
what mass of precipitate would be obtained?
Expert Solution
4. Sol :- Step 1
Mass of AgNO3 = 0.4522 g
Volume = 200 mL
Mass of K2CrO4 = 0.1668 g
Volume = 100 mL
Precipitates of Ag2CrO4 will formed
Then find :
a). Identify the limiting reactant
b). Calculate the mass of precipitates formed = ?
c). Calculate the mass of unreacted AgNO3 or K2CrO4 that remains in the solution = ?
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