c. [H+] = [A-]
The dissociation of weak acid in water occurs as shown by the equation;
HA → H+ + A-
The initial concentration of the weak acid is 0.10 M
Since you are dealing with a weak acid, all of it will not be dissociated to free H+.
Equal number of H+ and A- will be formed when HA dissociates. All the molecules will not be dissociated since it is a weak acid.
We have that for the Question "Which of the following statements is/are true for a 0.10 M solution of a weak acid HA?" it can be said that the statements is true for a 0.10 M solution of a weak acid HA is
[H+] = [A-]
From the question we are told
Which of the following statements is/are true for a 0.10 M solution of a weak acid HA?
(a) The pH is 1.00 M
(b) [H+ ] >> [A - ]
(c) [H+ ] = [A -]
Generally
HA = [H+] +[ A-]
Since
pH value of HA is not equal to 1
Being as it is a weak acid
Therefore
[H+] = [A-]
Hence
The statements is true for a 0.10 M solution of a weak acid HA is
[H+] = [A-]
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