Betermine the concentration of hydroxide ion, OH-, in a particular solution of Bro- by constructing an ICE table, writing the equilibrium constant expression, and using this information to determine the concentration of hydroxide ion. The Kb for BrO- is 4.0 × 10-6. Complete Parts 1-3 before submitting your answer. 1 2 3 NEXT > A 0.724 M aqueous solution of BrO- was prepared. Fill in the ICE table with the appropriate value for each involved species to determine concentrations of all reactants and products. BrO-(aq) + H₂O(1) Initial (M) Change (M) Equilibrium (M) = OH-(aq) + HBrO(aq)
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.
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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.
![< PREV
2
3
NEXT >
Based on your ICE table and the definition of Kb, set up the expression for Kb in order to
determine the unknown concentration. Each reaction participant must be represented by
one tile. Do not combine terms.
Kb
[0]
[0.724]
[4.0 × 10-9]
[0.362]
[x]
[0.724 - x]
[0.724 + 2x]
[0.724 - 2x]
[4.0 × 10€+x]
[4.0 × 10-x]
< PREV
1
2
=
4.0 × 10-6
[2x]
[2x]²
[4.0 x 10 + 2x] [4.0 × 10 - 2x]
3
RESET
[0.724 + x]
Based on your ICE table and equilibrium expression for Kb, determine the concentration
of hydroxide ion, OH- in this solution.
[OH-]
=
RESET
0
5.9 × 10-12
2.8
11.2
1.7 × 10-3
6.4
x
2.9 × 10-*
3.5 x 10-5](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff922ab2d-c754-4c9c-9d3b-bd784fecfd89%2F7529cd3b-b1c9-4a57-a181-a611e22ff2b3%2F9ohjepi_processed.png&w=3840&q=75)
![Determine the concentration of hydroxide ion, OH-, in a particular
solution of BrO by constructing an ICE table, writing the equilibrium
constant expression, and using this information to determine the
concentration of hydroxide ion. The Kb for BrO¯ is 4.0 × 10−6. Complete
Parts 1-3 before submitting your answer.
1
2
3
NEXT >
A 0.724 M aqueous solution of BrO¯ was prepared. Fill in the ICE table with the
appropriate value for each involved species to determine concentrations of all reactants
and products.
BrO-(aq)
+
H₂O(1)
=
OH-(aq)
+
HBrO(aq)
Initial (M)
Change (M)
Equilibrium (M)
-2x
4.0 × 10-6 -2x
0
0.724
4.0 × 10-6
0.362
+x
-x
RESET
+2x
0.724 + x
0.724 - x
0.724 + 2x
0.724 - 2x
4.0 × 10-6 + x
4.0 × 10-6-x
4.0 × 10-6 + 2x](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff922ab2d-c754-4c9c-9d3b-bd784fecfd89%2F7529cd3b-b1c9-4a57-a181-a611e22ff2b3%2F5o5l46_processed.png&w=3840&q=75)
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