Calculate the ratio of pH of a solution containing 1 mole of `CH_(3)COONa` + 1 mole of HCl per litre and of other solution containing 1 mole of HCl per litre and of other solution containing 1 mole `CH_(3)XCOoNa ` + 1 mole of acetic acid per litre .

Explanation

Case I : pH when 1 mole `CH_(3)COONa` and 1 mole HCl are present .
`{:(,CH_(3)COONa,+,HCl,to,CH_(3)COOH,+,NaCl),(" Before reaction",1,,1,,0,,0),("After reaction",0,,0,,1,,1):}`
` :. [ CH_(3)COOH] = 1 M `
` :. [H^(+)] = C .alpha = C sqrt(((K_(s))/(C))) = sqrt(K_(a).C) = sqrt((K_(s))) " " :. C = 1 `
` :. pH_(1) = -1/2 logK_(a)`
Case II . pH when 1 mole `CH_(3)COONa` and 1 mole mole of `CH_(3)COOH` , a buffer solution
` :. pH_(2) = - log K_(a)+log. (["salt"])/(["acid"])" ":.["Salt"]=1M`
` pH_(2) = -logK_(a) " ":. ["Acid"] = 1 M`
` :. (pH_(1))/(pH_(2))=1/2`