The pH of 0.05 M acetic acid is `(K_(a) = 2 xx 10^(-5))`

Calculate pH of 0.1 M acetic acid having K_(a)=1.8xx10^(-5)

0.2 M NaOH are added to 50 ml of 0.2 M acetic acid ( K_(a) = 1.8 xx 10^(-5)) . The volume of 0.2 M NaOH required to make the pH of solution 4.74 ( -log 1.8 xx 10^(-5) = 4.74 )

In the titration of 25.0 mL of 0.1 M aqueous acetic acid (K_(a) = 1.8 xx 10^(-5)) with 0.1 M NaOH (aq), the pH after addition of 10.0 mL of tirant is

Calculate PH Of 0.01 M acetic acid . K_a = 1.8 xx 10^-5 at 298 K.

The degree of ionization of 0.4 M acetic acid will be ( K _ a = 1.8 xx 10 ^( -5 ))

The pH of 0.5 M aqueous solution of HF (K_(a)=2xx10^(-4)) is

The pH of 0.5 M aqueous solution of HF (K_(a)=2xx10^(-4)) is

The [H^(+)] of a resulting solution that is 0.01 M acetic acid (K_(a)=1.8xx10^(-5)) and 0.01 M in benzoic acid (K_(a)=6.3xx10^(-5)) :