Consider the reaction of 50.7 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?
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Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
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Consider the reaction of 50.7 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?
![**Chemical Reaction Analysis and Calculation**
Consider the reaction of 50.7 mL of 0.310 M NaC₂H₅O₂ with 50.0 mL of 0.245 M HBr. (Ka of HC₂H₅O₂ = 6.3 × 10⁻⁵)
**Questions and Requirements:**
a) Write the net ionic equation for the reaction that takes place.
b) How many moles of C₂H₅O₂⁻ 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 C₂H₅O₂⁻ would be left in the beaker after the reaction goes to completion?
f) How many moles of HC₂H₅O₂ would have been produced after the reaction goes to completion?
g) What would be the pH of this solution after the reaction goes to completion?
**Solutions and Steps:**
**a) Net Ionic Equation:**
\[ \text{C}_2\text{H}_5\text{O}_2^- (aq) + \text{H}^+ (aq) \rightarrow \text{HC}_2\text{H}_5\text{O}_2 (aq) \]
**b) Calculation of Moles of C₂H₅O₂⁻:**
\[ \text{Moles of C}_2\text{H}_5\text{O}_2^- = \text{Volume (L)} \times \text{Molarity (M)} \]
\[ = 0.0507 \, \text{L} \times 0.310 \, \text{M} \]
\[ = 0.015717 \, \text{mol} \]
**c) Calculation of Moles of H⁺:**
\[ \text{Moles of H}^+ = \text{Volume (L)} \times \text{Molarity (M)} \]
\[ = 0.0500 \, \text{L} \times 0.245 \, \text{M} \]
\[ = 0.01225 \, \text{mol} \]
**d) Species](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7ac8288c-ae85-467f-b87f-b54a8edd702d%2F6d55877c-9059-4f99-84e2-870a00332f6c%2Fg3t4dn7.jpeg&w=3840&q=75)
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