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Consider 2.0 L of a solution that is 0.11 M NH3 and 0.13 M NH4Cl. Then 0.015 moles of NaOH is added to the solution (assume no volume change). What is the resulting pH? Kb(NH3) = 1.8 x 10-5 Select one: OA. 5.13 O B. 4.76 O C. 9.23 OD. 8.38

Consider 2.0 L of a solution that is 0.11 M NH3 and 0.13 M NH4Cl. Then 0.015 moles of NaOH is added to the solution (assume no volume change). What is the resulting pH? Kb(NH3) = 1.8 x 10-5 Select one: OA. 5.13 O B. 4.76 O C. 9.23 OD. 8.38

Chemistry by OpenStax (2015-05-04)
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter14: Acid-base Equilibria
Section: Chapter Questions
Problem 100E: What mass of NH4Cl must be added to 0.750 L of a 0.100-M solution of NH3 to give a buffer solution...
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Consider 2.0 L of a solution that is 0.11 M NH3 and 0.13 M NH4Cl. Then 0.015 moles of NaOH is added to the solution (assume no volume change). What is the resulting pH? Kb(NH3) = 1.8 x 10-5 Select one: OA. 5.13 O B. 4.76 O C. 9.23 OD. 8.38
Transcribed Image Text:Consider 2.0 L of a solution that is 0.11 M NH3 and 0.13 M NH4Cl. Then 0.015 moles of NaOH is added to the solution (assume no volume change). What is the resulting pH? Kb(NH3) = 1.8 x 10-5 Select one: OA. 5.13 O B. 4.76 O C. 9.23 OD. 8.38
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