What is the `OH^(-)` concentration of a 0.08 M solution of `[K_(a)(CH_(3)COOH)=1.8 xx 10^(-5)]`

What is the [OH^(-)] concentration of a 0.04 M solution of CH_(3)COONa? [K_(a)" of "CH_(3)COOH=2xx10^(-5),log2=.30]

What is the [OH^(-)] concentration of a 0.04 M solution of CH_(3)COONa? [K_(a)" of "CH_(3)COOH=2xx10^(-5),log2=20]

0.05 M ammonium hydroxide solution is dissolved in 0.001 M ammonium chloride solution. What will be the OH^(-) ion concentration of this solution ? (K_(b) (NH_(4) OH) = 1.8 xx 10^(-5)

0.05 M ammonium hydroxide solution is dissolved in 0.001 M ammonium chloride solution. What will be the OH^(-) ion concentration of this solution ? (K_(b) (NH_(4) OH) = 1.8 xx 10^(-5)

Calculate the concentration of H^+ ions in 0.2 M solution of CH_3COOH . K_a for CH_3COOH=1.8xx10^(-5)

What is the pH of 7.0 xx 10^(-8)M acetic acid. What is the concentration of un-ionsed acetic acid. K_(a) of CH_(3)COOH = 1.8 xx 10^(-5) .

What is pH of 7.0 xx 10^(-8)M acetic acid. What is the concentration of un-ionsed acetic acid. K_(a) of CH_(3)COOH = 1.8 xx 10^(-5) .

Calculate pH solution: 0.1 M CH_(3)COOH (K_a=1.8 xx 10^(-5))

Calculate pH of 0.05 M Acetic acid solution , if K_(a)(CH_(3)COOH) = 1.74 xx 10^(-5) .