Acetic acid and propanoic acid have K_(a) value 1.75xx10^(-5) and 1.3xx10^(-5) respectively at a certain temperature. An equimolar solution of a mixture of the two acids is partially neutralised by NaOH . How is the ratio of the contents of acetate and propionate ions related to the K_(a) values and the molarity?

Acetic acid and propanoic acid have K_(a) value 1.75xx10^(-5) and 1.3x

1.	Acetic acid and propanoic acid have K_(a) value 1.75xx10^(-5) and 1.3xx10^(-5) respectively at a certain temperature. An equimolar solution of a mixture of the two acids is partially neutralised by NaOH . How is the ratio of the contents of acetate and propionate ions related to the K_(a) values and the molarity?
Answer» `((alpha)/(1-alpha))=(1.75)/(1.3)xx((beta)/(1-beta))` , where `alpha` (acetic ACID) and `beta` (propanic acid) are ionised fractions of their ACIDS. the RATIO is underlated to the `K_(a)` values The ratio is UNRELATED to the molarity of acid. The ratio is unrelated to the pH of the SOLUTION. Answer :a,c,d