To carry out a particular reaction, you determine that you need 0.0500 moles of ammonium chloride. what volume of 0.876 M ammonium chloride will you need to complete the reaction without any left over?
Added by Kyle O.
Step 1
The formula is: \[ \text{Volume (L)} = \frac{\text{Moles}}{\text{Molarity (M)}} \] Show more…
Show all steps
Your feedback will help us improve your experience
Crystal Wang and 80 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
A reaction requires $70.6 \mathrm{~g}$ of $\mathrm{NH}_{4} \mathrm{Cl}$. What volume of the solution described in Exercise 59 do you need if you want to use a $20.0 \%$ excess of $\mathrm{NH}_{4} \mathrm{Cl}$ ?
A A reaction requires $65.6 \mathrm{~g}$ of $\mathrm{NH}_{4}$ Cl. What volume of the solution described in Exercise 59 do you need if you want to use a $25.0 \%$ excess of $\mathrm{NH}_{4} \mathrm{Cl} ?$
How many grams of Ammonium Chloride are required to prepare 500 mL of a 0.0750 mol/L solution of Ammonium Chloride, (NH4)Cl?
Jennifer H.
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