The ionization constant of acetic acid `1.74xx10^(-5)`. Calculate the degree of dissociation of acetic acid in its `0.05 M` solution. Calculate the concentration of acetate ion in the solution and its `pH`.

Options

A. `54.95`
B. `9.6`
C. `4.6`
D. `42.3454`

Answer

A

Explanation

Aniline acetate is state of weak acid and weak base , its degree of hydrolysis may be calculated using following formula
`alpha= sqrt((K_(h)))= sqrt(((K_(w))/(K_(a)xxK_(b))))......(i)`
where `K_(w)=10^(-14)`
`K_(a)=1.75xx10^(-5), K_(b)3.8.x10^(-10)`
Hence from equation (i) we have
`alphasqrt(((10^(-14))/(1.75xx10^(-5)xx3.83xx10^(-10))))=1.22`
Which is not possibel because, degree of hydrolysis may not be greater than 1.
Thus, we have to avoid the approximation
`((alpha)/(1-alpha))= sqrt((K_(h)))=1.22, alpha=(1.22)/(2.22))=0.5495`
`%` hydrolysis `alphax100`
`=0.5495x100=54.95%`