What is the $pH$ of acetic acid at equilibrium,given that acetic acid concentration is $0.1 \ M$ and it is $30 \%$ dissociated at equilibrium? $(\log 3=0.47)$
- A$2$
- B$1.53$
- C$3.53$
- D$3$
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Similar Questions
The $pH$ of a $0.1 \ M$ solution of acetic acid will be (degree of dissociation of acetic acid is $0.0132$).
An acid solution of $pH=6$ is diluted $1000$ times,the $pH$ of the final solution becomes
DifficultMHT CET 2011
View SolutionWhen a $1$ deci-normal solution of acetic acid is $1.3\%$ ionized,what is the value of the ionization constant $(K_a)$?
Difficult
View SolutionAt $298 \ K$,$0.1 \ M$ solution of acetic acid is $1.34 \ \%$ ionized. What is the dissociation constant of acetic acid?
The $pH$ of $0.05 \ M$ acetic acid is $(K_a = 2 \times 10^{-5})$.
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