An attempt is made to analyse barium gravimetrically by precipitating of BaF, with NaF2. Assuming that 200 mg sample of Ba2+ in 100 mL of solution is to be precipitated and the precipitation must be 99.9% completed. The solubility product of BaF, is 1.7 x 10-6. i. Determine the amount of Ba2+ that must remain in 100 mL of solution so that the precipitation 99.9% is completed (in mg mL-1). ii. Based on the following balanced chemical equation, calculate the concentration of F after the precipitation of BaF2. BaF, (s) == Ba?* (aq) + 2F¯(aq)
An attempt is made to analyse barium gravimetrically by precipitating of BaF, with NaF2. Assuming that 200 mg sample of Ba2+ in 100 mL of solution is to be precipitated and the precipitation must be 99.9% completed. The solubility product of BaF, is 1.7 x 10-6. i. Determine the amount of Ba2+ that must remain in 100 mL of solution so that the precipitation 99.9% is completed (in mg mL-1). ii. Based on the following balanced chemical equation, calculate the concentration of F after the precipitation of BaF2. BaF, (s) == Ba?* (aq) + 2F¯(aq)
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter15: Complex Ion And Precipitation Equilibria
Section: Chapter Questions
Problem 30QAP: Silver(I) sulfate (Ksp=1.2105) is used in the electroplating of silver. A 1.0-L solution is prepared...
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Transcribed Image Text:An attempt is made to analyse barium gravimetrically by precipitating
of BaF, with NaF,. Assuming that 200 mg sample of Ba2+ in 100 mL
of solution is to be precipitated and the precipitation must be 99.9%
completed. The solubility product of BaF, is 1.7 x 10-6.
i.
Determine the amount of Ba2+ that must remain in 100 mL
of solution so that the precipitation 99.9% is completed
(in mg mL-1).
ii.
Based on the following balanced chemical equation, calculate
the concentration of F after the precipitation of BaF2.
BaF, (s) = Ba?* (aq) + 2F¯ (aq)
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