The depression in freezing point of `0.01 m` aqueous `CH_(3)CooH` solution is `0.02046^(@)`, `1 m` urea solution freezes at `-1.86^(@)C`. Assuming molality equal to molarity, `pH` of `CH_(3)COOH` solution is

Depression of freezing point of 0.01 molal aq. CH_(3)COOH solution is 0.02046^(@) . 1 molal urea solution freezes at -1.86^(@) C . Assuming molarity equal to molarity , pH of CH_(3)COOH solution is :

Depression in freezing point of 0.01 molal aqueous HCOOH solution is 0.02046. one molal aqueous urea solution freezes at -1.86^(@)C , assuming molality equal to molari ty, pH of HCOOH solution is :

Depression in freezing point of 0.01 molal aqueous HCOOH solution is 0.02046^(@)C . 1 molal aqueous urea solution freezes at -1.86^@ C . Assuming molality equal to molarity , calculate the pH of HCOOH solution.

depression in freezing point of 0.01 molal aqueous CH_(3)COOH solution is 0.02046^(@)C . Assuming molality equal to molarity. pH of CH_(3)COOH solution is (K_(f)=1.86K Kg "mol"^(-1)) _______________________.

The depression in freezing point of 0.01 m aqueous solution of urea, sodium chloride and sodium sulphate is in the ratio

If the freezing point of 0.1 M HA(aq) solution is -0.2046^(@)C then pH of solution is ( If K_(f) water =1.86mol^(-1)kg^(-1))

If the freezing point of 0.1 M HA(aq) solution is -0.2046^(@)C then pH of solution is ( If K_(f) water =1.86mol^(-1)kg^(-1))

The measured freezing point depression for a 0.1m aqueous CH_(3)COOH solution is 0.19""^(@)C . The acid dissociation constant K_(e) at this concentration will be (Given K_(f) , the molal cryoscopic constant = 1.86 K kg mol^(-1) )