Question

Gravimetry 325 mL of solution was prepared by dissolving a sample of 8.475 g of sample containing baryum nitrate (Ba(NO3)2) in water. The analysis of the barium content of an intake of 50.00 mL of the solution led to the formation of 0.2924 g of dried BaSO4. Calculate the mass fraction (%) in Ba(NO3)2 of the sample.

Name: gravimetry 325 ml of solution was prepared by dissolving a sample of 8475 g of sample containing baryum nitrate bano32 in water the analysis of the barium content of an intake of 5000 ml of 16255
Uploaded: 2024-07-29T19:20:38-08:00
Duration: 1 min 31 s
Channel: Adi S
Description: gravimetry 325 ml of solution was prepared by dissolving a sample of 8475 g of sample containing baryum nitrate bano32 in water the analysis of the barium content of an intake of 5000 ml of 16255

          Gravimetry
325 mL of solution was prepared by dissolving a sample of 8.475 g of sample containing baryum nitrate (Ba(NO3)2) in water. The analysis of the barium content of an intake of 50.00 mL of the solution led to the formation of 0.2924 g of dried BaSO4.
Calculate the mass fraction (%) in Ba(NO3)2 of the sample.

Added by Jes-S W.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert Adi S

07/29/2024

Step 1

- The molar mass of BaSO4 (Barium Sulfate) is calculated as follows: - Ba: 137.33 g/mol - S: 32.07 g/mol - O: 16.00 g/mol × 4 = 64.00 g/mol - Total = 137.33 + 32.07 + 64.00 = 233.40 g/mol - Now, calculate the moles of BaSO4 formed from 0.2924 g: \[ Show more…

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Gravimetry 325 mL of solution was prepared by dissolving a sample of 8.475 g of sample containing baryum nitrate (Ba(NO3)2) in water. The analysis of the barium content of an intake of 50.00 mL of the solution led to the formation of 0.2924 g of dried BaSO4. Calculate the mass fraction (%) in Ba(NO3)2 of the sample.