Question
A bottle of 12.0 M hydrochloric acid has only 35.7 mL left in it. What will the HCl concentration be if the solution is diluted to 250.0 mL?
Step 1
The dilution equation is given by $C_1V_1 = C_2V_2$, where $C_1$ and $V_1$ are the initial concentration and volume, and $C_2$ and $V_2$ are the final concentration and volume after dilution. Show more…
Show all steps
Your feedback will help us improve your experience
Nadia Lara and 94 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
Concentrated hydrochloric acid is $12 \mathrm{M}$. What is the molarity of an $\mathrm{HCl}$ solution prepared by diluting $10.0 \mathrm{~mL}$ of concentrated acid to a total volume of $250.0 \mathrm{~mL}$ ?
You have $250 .$ mL of $0.136 \mathrm{M}$ HCl. Using a volumetric pipet, you take $25.00 \mathrm{mL}$ of that solution and dilute it to $100.00 \mathrm{mL}$ in a volumetric flask. Now you take $10.00 \mathrm{mL}$ of that solution, using a volumetric pipet, and dilute it to $100.00 \mathrm{mL}$ in a volumetric flask. What is the concentration of hydrochloric acid in the final solution?
Titration of a $12.0 \mathrm{~mL}$ solution of $\mathrm{HCl}$ requires $22.4 \mathrm{~mL}$ of $0.12 \mathrm{M} \mathrm{NaOH}$. What is the molarity of the HCl solution?
Transcript
18,000,000+
Students on Numerade
Trusted by students at 8,000+ universities
Watch the video solution with this free unlock.
EMAIL
PASSWORD