According to Le Chatelier's principle, if you add more A to the following solution at pH 5.00, what will happen. ASsume HA is a weak acid. Watch equilibrium video posted on module 2 learning objectives page if you are not familiar with Le Chatelier's principle. H A(aq) + H2O«) + H3OTag) + A(aq) (ад) a. pH will increase but not much b. pH will decrease but not much c. amount of A- will decrease (than in the initial solution) d. amount of HA will increase (than in the initial solution) e. pH will still be 5.00

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Why is the answer a & d? 

According to Le Chatelier's principle, if you add more A to the following solution at pH 5.00, what
will happen. ASsume HA is a weak acid. Watch equilibrium video posted on module 2 learning
objectives page if you are not familiar with Le Chatelier's principle.
HA(aq) + H2O(1)
H3O* + A(ag)
(aq)
a. pH will increase but not much
b. pH will decrease but not much
C. amount of A- will decrease (than in the initial solution)
d. amount of HA will increase (than in the initial solution)
e. pH will still be 5.00
Transcribed Image Text:According to Le Chatelier's principle, if you add more A to the following solution at pH 5.00, what will happen. ASsume HA is a weak acid. Watch equilibrium video posted on module 2 learning objectives page if you are not familiar with Le Chatelier's principle. HA(aq) + H2O(1) H3O* + A(ag) (aq) a. pH will increase but not much b. pH will decrease but not much C. amount of A- will decrease (than in the initial solution) d. amount of HA will increase (than in the initial solution) e. pH will still be 5.00
Expert Solution
Step 1

The equilibrium reaction given is,

=> HA(aq) + H2O (l)  H3O+ (aq)+ A- (aq)

Given: More A- is added in the solution.

 

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