How much water must be added to 300mL of 0.2M solution of `CH_(3)COOHKa=1.8xx10^(-5)` for the degree of dissociation to double ?

How much water must be added to 300 mL of a 0.2M solution of CH_(3)COOH for the degree of dissociation of the acid to double ? ( Assume K_(a) of acetic is of order of 10^(-5)M)

How much water must be added to 300 mL of a 0.2M solution of CH_(3)COOH for the degree of dissociation of the acid to double ? ( Assume K_(a) of acetic is of order of 10^(-5)M)

How much water must be added to 300 mL of a 0.2M solution of CH_(3)COOH for the degree of dissociation of the acid to double ? ( Assume K_(a) of acetic is of order of 10^(-5)M)

How much water must be added to 300 mL of a 0.2M solution of CH_(3)COOH for the degree of dissociation of the acid to double ? ( Assume K_(a) of acetic is of order of 10^(-5)M)

How much water (in ml) must be added to 300 mL of a 0.2 M solution of CH_(3)COOH for the degree of dissociation of the acid to double ? [Assume K_(a) of acetic acid is of the order of 10^(-5)M]

How much water must be added to 100ml of 0.5M NaOH to get 0.2M NaOH solution.

A monoprotic acid in 0.1 M solution has K_(a)=1.0xx10^(-5) . The degree of dissociation for acid is

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