An aqueous solution of hydrofluoric acid is 30.0% HF, by mass, and has a density of 1.101 g/cm³. Compute the mole fraction of HF in the solution described above.
Added by Scott H.
Step 1
Assuming we have 100 g of the solution, then 30 g of it is HF (since it is 30% by mass). Show more…
Show all steps
Your feedback will help us improve your experience
Sri K and 81 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
An aqueous solution of HF (MM=20.01 g/mol) has a density of 0.99 g/mL and molarity of 28.9 M. What is the mole fraction of HF?
Adi S.
Calculate the mass of HF dissolved in 683.0 mL of 0.323 M hydrofluoric acid.
a) An aqueous solution is 30.0% hydrofluoric acid (HF, molar mass = 20.01 g/mol) by weight. If the density of a 30.0% HF solution in water is 1.101 g/mL, what is the molality of the solution (to 3 significant figures)? b) How many mL of 0.250 M Ba(OH) 2 is needed to completely neutralize a 12.0 mL of 1.00 M HCl? Report your volume in mL to 3 significant figures
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