Aluminum sulfate, Al2(SO4)3, is an ionic compound that is used in the manufacture of paper and in various water purification processes. What is the formula mass (amu) of this compound?
Added by Cesar G.
Step 1
98 g/mol - Sulfur (S): 32.07 g/mol - Oxygen (O): 16.00 g/mol Now, we need to multiply the molar mass of each element by the number of atoms of that element in the compound: - Aluminum: 2 atoms × 26.98 g/mol = 53.96 g/mol - Sulfur: 3 atoms × 32.07 g/mol = 96.21 Show more…
Show all steps
Your feedback will help us improve your experience
Adi S and 100 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
what is the molar mass of Aluminum Sulfate Penta Hydrate (Al2(SO4)3) 5H2O
Madhur L.
calculate the mass percent of aluminum in AL2(SO4)3
Chareen G.
Aluminum sulfate, Al2(SO4)3, is a compound used in sewage treatment plants. 1. Select a pair of conversion factors that relate moles of Al to moles of S. 2. Construct a pair of conversion factors that relate moles of S to moles of Al2(SO4)3. 3. How many moles of Al are in a sample of this compound if the sample also contains 0.969 mol S? 4. How many moles of S are in 1.38 mol Al2(SO4)3?
Sri K.
Recommended Textbooks
Chemistry: Structure and Properties
Chemistry The Central Science
Chemistry
Transcript
18,000,000+
Students on Numerade
Trusted by students at 8,000+ universities
Watch the video solution with this free unlock.
EMAIL
PASSWORD