Determine the resulting pH when 0.0015 of solid Ba(OH)2 is added to a 0.350 L but containing 0.110 M weak acid, HA, and 0.2 M of its conjugate base, A. The value of K HA is 3.2 x 10-º. 1 3 4 Use the table below to determine the mol reactant and product after the reaction of acid and base. You can ignore the amoun
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 is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
Find kb ?
find Ph?
![Determine the resulting pH when 0.0015 mol
of solid Ba(OH)2 is added to a 0.350 L buffer
containing 0.110M weak acid, HA, and 0.220
M of its conjugate base, A. The value of Ka for
HA is 3.2 x 10-9.
1
2
3
4
Based on the result of the acid-base reaction,
set up the ICE table in order to determine the
unknown.
HA(aq) + H2O(1) =H;0*(aq) + A´(aq)
Initial (M)
Change (M)
Equilibrium
(M)
5 RESET
0.110
0.220
0.101
0.229
0.106
+x
0.110 + x
0.110 - x
0.220 + x
-X
0.220 - x
0.101 + x
0.101 - x
0.229 + x
0.229 - x
0.106 + x
0.106 - x
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![Determine the resulting pH when 0.0015 mol
of solid Ba(OH)2 is added to a 0.350 L buffer
containing 0.110M weak acid, HA, and 0.220
M of its conjugate base, A. The value of Ka for
HA is 3.2 x 10-9.
1
2
4
Use the table below to determine the moles of
reactant and product after the reaction of the
acid and base. You can ignore the amount of
liquid water in the reaction.
HA(aq) + OH (aq) → H20(1) + A(aq)
Before (mol)
Change (mol)
After (mol)
5 RESET
0.110
0.220
0.0015
-0.0015
0.0030
-0.0030
0.0385
0.0770
0.0370
0.0355
0.0750
0.0800
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