The mass of acetic acid present in `500 ml` of solution in which it is `1%` ionides (Ka of ` CH_(3)COOH = 1.8 xx 10^(-4)`)

The mass of acetic acid present in 500 ml solution in which it is 1% ionised ( K_(a) of CH_(3) COOH = 1.8 xx 10^(-5) )

Calculate the amount of acetic acid present in 1L of solution having alpha = 1% and K_(a) = 1.8 xx 10^(-5) .

Calculate the amount of acetic acid presnt in 1L of solution having alpha = 1% and K_(a) = 1.8 xx 10^(-5) .

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

Calculate the amount of acetic acid present in one litre, having degree of dissociation equal 1% and K_(a) = 1.8 xx 10^(-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: 10^(-8)M CH_(3)COOH (K_(a)=1.8 xx 10^(-5))

How many times of the acetic acid concentration, acetate salt should be added to a given acetic acid solution to obtain a solution of pH = 7.0 ( K_a for CH_3COOH=1.8xx10^(-5) ) .