What is the `pH` of a `1 M CH_(3)COOH` a solution `K_(a)` of acetic acid `=1.8xx10^(-5)`?
`K=10^(-14)mol^(2) litre^(-2)`

What is the pH of a 1 M CH_3COONa solution? K_2 of acetic acid = 1.8 xx 10^-5 and K_w = 10^-14 mol^2 litre^-2:

Calculate the pH value of 0.15 M solution of acetic acid. K_(CH_3COOH)=1.8xx10^(-5)

What is the pH at equivalence point in the titration of 0.1 M CH_(3)COOH and 0.1 NaOH? ( K_(a) for acetic acid is 1.8 xx 10^(-5) )

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