Depression in freezing point of 0.01 mol...

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.

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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 :

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

The mole fraction of solvent in 0.1 molal aqueous solution is

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)) _______________________.

Mole fraction of the solute in a 1.0 molal aqueous solution is:

Depression in freezing point of 0.1 molal solution of HF is -0.201^(@)C . Calculate percentage degree of dissociation of HF. (K_(f)=1.86 K kg mol^(-1)) .

What is the boiling point of 1 molal aqueous solution of NaCl (K_b)=0.52 K molal^-1]

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