9. Finally, you add 200 mL of 0.2 M sodium acetate to a final 200 mL aliquot of 0.100 M HCl. What is the final pH? Kb of acetate is 5.56 x 10-10 and Ka of acetic acid is 1.8 x 10^-5
Added by Em D.
Step 1
• Volume of HCl = 200 mL = 0.200 L • Molarity of HCl = 0.100 M • Moles of HCl = 0.200 L × 0.100 mol/L = 0.0200 moles Show more…
Show all steps
Close
Your feedback will help us improve your experience
Aparna Shakti and 60 other Chemistry 102 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
300 mL of 0.26 M acetic acid solution (CH3CO2H; Ka = 1.8 x 10-5) is mixed with an equal volume of 0.32 M sodium acetate solution (CH3CO2Na). If a 100 mL sample of the resulting solution is add 5 mL of 0.5 N KOH solution, calculate the pH variation in the sample.
Adi S.
What is the pH of a solution made by adding 0.30 mol of acetic acid and 0.30 mol of sodium acetate to enough water to make 1.0 L of solution? Ka = 1.8 x 10^-5 a. Calculate using ICE charts b. Calculate using Henderson-Hasselbalch equation
Dinesh S.
A solution is prepared by dissolving 1.700 g of sodium acetate (CH3COONa) into 100.00 mL of a 0.170 M solution of acetic acid. The Ka of acetic acid is 1.8 x 10^-5. What is the pH of the solution? pH =
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