What is the alpha of 0.1M acitic acid?
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Acetic acid is a weak monoprotic acid. In aqueous solution, it has a pKa value of 4.76. Its conjugate base is acetate (CH3COO−). A 1.0 M solution has a pH of 2.4, indicating that merely 0.4% of the acetic acid molecules are dissociated.
For acetic acid pKa =4.76 and –log(10)[H+] = pH
4.76 = log(10)(0.1) + 2*pH
=>2*pH=4.76 + 1
=> pH = 5.76/2
=> pH = 2.88
The required pH of 0.1 M solution of acetic acid is 2.88.
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Answer:
The pH of 0.1M acetic acid solution is closest to[Dissociation constant of the acid, Ka=1.8× 10−5]. A ... On solving we get α=0.0134.
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