Question

Consider the reaction of 75.0 mL of 0.350 M C₅H₅N (Kb = 1.7 x 10⁻⁹) with 100.0 mL of 0.405 M HCl. a) Write the net ionic equation for the reaction that takes place. b) How many moles of C₅H₅N would be present before the reaction takes place. c) How many moles of H+ would be present if 100.00 mL of H+ were added?

Name: consider the reaction of 750 ml of 0350 m c5h5n kb 17 x 109 with 1000 ml of 0405 m hcl a write the net ionic equation for the reaction that takes place b how many moles of c5h5n would be pre 07937
Uploaded: 2022-11-01T19:36:01-08:00
Duration: 1 min 51 s
Channel: David Collins
Description: consider the reaction of 750 ml of 0350 m c5h5n kb 17 x 109 with 1000 ml of 0405 m hcl a write the net ionic equation for the reaction that takes place b how many moles of c5h5n would be pre 07937

          Consider the reaction of 75.0 mL of 0.350 M C₅H₅N (Kb = 1.7 x 10⁻⁹) with 100.0 mL of 0.405 M HCl.

a) Write the net ionic equation for the reaction that takes place.
b) How many moles of C₅H₅N would be present before the reaction takes place.
c) How many moles of H+ would be present if 100.00 mL of H+ were added?

Added by Sara B.

Chemistry: Structure and Properties

Nivaldo Tro 2nd Edition

Instant Answer

Solved by Expert David Collins

11/01/2022

Step 1

Step 1:** Write the net ionic equation for the reaction that takes place: \[C_5H_5N + HCl \rightarrow C_5H_5NH^+ + Cl^-\] ** Show more…

Show all steps

Thanks for your feedback!

Consider the reaction of 75.0 mL of 0.350 M C₅H₅N (Kb = 1.7 x 10⁻⁹) with 100.0 mL of 0.405 M HCl. a) Write the net ionic equation for the reaction that takes place. b) How many moles of C₅H₅N would be present before the reaction takes place. c) How many moles of H+ would be present if 100.00 mL of H+ were added?