Question
The density of a solution of sulfuric acid is $1.285 \mathrm{~g} / \mathrm{cm}^{3}$, and it is $38.08 \%$ acid by mass. Calculate the volume of the acid solution (in mL) you need to supply $125 \mathrm{~g}$ of sulfuric acid.
Step 1
Since the solution is 38.08% sulfuric acid by mass, we have $38.08g$ of $H_2SO_4$ in $100g$ of the solution. Show more…
Show all steps
Your feedback will help us improve your experience
Ronald Prasad 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
The density of a solution of sulfuric acid is $1.285 \mathrm{~g} / \mathrm{cm}^{3}$, and it is $38.08 \%$ acid by mass. Calculate the volume of solution (in $\mathrm{mL}$ ) that contains $125 \mathrm{~g}$ of sulfuric acid.
The density of a solution of sulfuric acid is $1.285 \mathrm{~g} / \mathrm{cm}^{3}$, and it is $38.08 \%$ acid by mass. What volume of the acid solution (in mL) do you need to supply $125 \mathrm{~g}$ of sulfuric acid?
The density of a solution of sulfuric acid is $1.285 \mathrm{~g} / \mathrm{cm}^{5}$, and it is $38.08 \%$ acid by mass. What volume of the acid solution (in $\mathrm{mL}$ ) do you need to supply $125 \mathrm{~g}$ of sulfuric acid?
Transcript
18,000,000+
Students on Numerade
Trusted by students at 8,000+ universities
Watch the video solution with this free unlock.
EMAIL
PASSWORD