Determine the pH of a buffer solution by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the pH. Complete Parts 1-3 before submitting your answer. Initial (M) Change (M) Equilibrium (M) 0.178 0.880 - x The buffer was prepared by dissolving 21.5 g HC7H5O₂ and 37.7 g of NaC-H5O₂ in 200.0 mL of solution. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products.. 0 0.888 1 HC7HsO₂(aq) + 1.31 + x 21.5 +X 0.178 + x 37.7 2 H₂O(l) 0.888 + x 0.176 21.5-x 3 H3O+ (aq) + 0.261 37.7 + x 0.880 NEXT > 0.176 - x C7H5O₂ (aq) RESET 1.31 0.261 + x
Ionic Equilibrium
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.
Arrhenius Acid
Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.
Bronsted Lowry Base In Inorganic Chemistry
Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
![Determine the pH of a buffer solution by constructing an ICE table, writing the
equilibrium constant expression, and using this information to determine the pH.
Complete Parts 1-3 before submitting your answer.
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The Ka for HC7H5O₂ is 6.3 × 10-5. Based on your ICE table (Part 1) and the definition of Ka, set up the
expression for Ka in order to determine the unknown. Each reaction participant must be represented by
one tile. Do not combine terms.
[0]
[0.888]
[1.31 + x]
[21.5]
[x]
[0.178 + x]
1
Ka
[37.7]
[2x]
[0.888 + x]
[0.176]
[21.5-x]
2
[0.261]
[37.7 + x]
= 6.3 × 10-5
[0.880]
3
[0.176 -x]
[1.31]
[0.261 + x]
RESET
[0.178]
[0.880 -x]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F53fad175-5b35-4951-b14a-e374468693f0%2Fb0d9c59d-4f80-49ff-936f-bd0a9e1e95c2%2Fh2hq6x_processed.png&w=3840&q=75)
![Determine the pH of a buffer solution by constructing an ICE table, writing the
equilibrium constant expression, and using this information to determine the pH.
Complete Parts 1-3 before submitting your answer.
3
NEXT >
The buffer was prepared by dissolving 21.5 g HC7H5O2 and 37.7 g of NaC7H5O₂ in 200.0 mL of solution.
Fill in the ICE table with the appropriate value for each involved species to determine concentrations of
all reactants and products..
Initial (M)
Change (M)
Equilibrium (M)
0.178
0.880 - x
0
0.888
1
HC7H5O₂(aq) +
1.31 + x
21.5
+X
0.178 + x
37.7
-X
H₂O(1)
0.888 + x
0.176
21.5-x
H3O+ (aq)
0.261
37.7 + x
+
0.880
0.176 - x
C7H5O₂ (aq)
RESET
1.31
0.261 + x](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F53fad175-5b35-4951-b14a-e374468693f0%2Fb0d9c59d-4f80-49ff-936f-bd0a9e1e95c2%2Fpe74gul_processed.png&w=3840&q=75)
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