Excess (NH4)2SO4 was added to a 55.0 mL solution containing BaCl2 (MW=208.23 g/mol). The resulting BaSO4 (MW=233.43 g/mol) precipitate had a mass of 0.3863 g after it was filtered and dried. What is the molarity of BaCl2 in the solution?
Added by David C.
Step 1
Given: - Mass of BaSO4 precipitate = 0.3863 g - Molar mass of BaSO4 = 233.43 g/mol Number of moles of BaSO4 = Mass / Molar mass Number of moles of BaSO4 = 0.3863 g / 233.43 g/mol Number of moles of BaSO4 = 0.001655 moles Show more…
Show all steps
Your feedback will help us improve your experience
Ronald Prasad and 95 other Chemistry 101 educators are ready to help you.
Ask a new question
Labs
Want to see this concept in action?
Explore this concept interactively to see how it behaves as you change inputs.
Key Concepts
Recommended Videos
Excess (NH4)2SO4 was added to a 65.0 mL solution containing BaCl2 (MW=208.23 g/mol). The resulting BaSO4 (MW=233.43 g/mol) precipitate had a mass of 0.2791 g after it was filtered and dried. What is the molarity of BaCl2 in the solution?
Sri K.
What is the molarity of an aqueous solution prepared by adding 36.5 g of barium chloride to enough water to make 750.0 mL of solution? (Molar mass of BaCl2 is 208.2 g/mol)
Adi S.
A salt contains only barium and one of the halide ions. A 0.158-$\mathrm{g}$ sample of the salt was dissolved in water, and an excess of sulfuric acid was added to form barium sulfate $\left(\mathrm{BaSO}_{4}\right),$ which was filtered, dried, and weighed. Its mass was found to be $0.124 \mathrm{g} .$ What is the formula of the barium halide?
Recommended Textbooks
Chemistry: Structure and Properties
Chemistry The Central Science
Chemistry
Transcript
Watch the video solution with this free unlock.
EMAIL
PASSWORD