Question

Question 10 of 13 Calculate the pH when 41.0 mL of 0.200 M HBr is mixed with 30.0 mL of 0.400 M $CH_3NH_2$ ($K_b = 4.4 \times 10^{-4}$).

          Question 10 of 13
Calculate the pH when 41.0 mL of 0.200 M HBr is mixed with 30.0 mL of 0.400 M $CH_3NH_2$ ($K_b = 4.4 \times 10^{-4}$).

Question 10 of 13
Calculate the pH when 41.0 mL of 0.200 M HBr is mixed with 30.0 mL of 0.400 M CH3NH2 (Kb = 4.4 × 10^-4).

Added by Lindsey R.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert David Collins

07/04/2023

Step 1

For HBr: moles of HBr = (0.200 mol/L) * (0.041 L) = 0.0082 mol For CH3NH2: moles of CH3NH2 = (0.400 mol/L) * (0.030 L) = 0.012 mol Show more…

Show all steps

Thanks for your feedback!

Question 10 of 13 Calculate the pH when 41.0mL of 0.200MHBr is mixed with 30.0mL of Question 10 of 13 Calculate the pH when 41.0 mL of 0.200 M HBr is mixed with 30.0 mL of 0.400M CHNH Kb=4.4 10-) 2 5 8 +/-

Play audio

Feedback

David Collins and 88 other subject Chemistry 101 educators are ready to help you.

Ask a new question

Labs

Want to see this concept in action?

NEW

Explore this concept interactively to see how it behaves as you change inputs.

View Labs

Key Concepts

Recommended Videos

Recommended Textbooks

Transcript

Ace is your personal tutor. It breaks down any question with clear steps so you can learn.

Start Using Ace

Continue solving this problem

Create a free account to:

View full step-by-step solution
Ask follow-up questions with Ace AI
Save progress and study later

Question

Question 10 of 13 Calculate the pH when 41.0 mL of 0.200 M HBr is mixed with 30.0 mL of 0.400 M $CH_3NH_2$ ($K_b = 4.4 \times 10^{-4}$).

Please give Ace some feedback