Chemistry
Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Question

Consider the reaction of 66.5 mL of 0.310 M NaC₇H₅O₂ with 50.0 mL of 0.245 M HBr. (Ka of HC₇H₅O₂ = 6.3 x 10⁻⁵)

a)Write the net ionic equation for the reaction that takes place. (In terms of C, H2O, H3O+, O, H, H+, OH-)

b) How many moles of C7H5O2- would be present before the reaction takes place?

c) How many moles of H+ would be present before the reaction takes place?

d)What species would be left in the beaker after the reaction goes to completion?

e) How many moles of C7H5O2- would be left in the beaker after the reaction goes to completion?

f) How many moles of HC7H5O2 would have been produced after the reaction goes to completion?

g) What would be the pH of this soultion after the reaction goes to completion?

Expert Solution
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“Since you have posted a question with multiple sub-parts, we will solve the first three subparts for you. To get the remaining sub-part solved please repost the complete question and mention the sub-parts to be solved.”

 

 

According to the question we have,

The molarity of the NaC₇H₅O₂ is given by = 0.310 M = 0.310 mol/L

The volume of the NaC₇H₅O₂ is given by = 66.5 ml = 0.0665 L

The molarity of the HBr is given by = 0.245 M = 0.245 mol/L

The volume of the HBr is given by = 50.0 ml = 0.050 L

The Ka for the HC₇H₅O₂ is given by = 6.3 x 10⁻⁵

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