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Define cryoscopic constant....

Define cryoscopic constant.

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Depression of freezing point of which of the following solutions does represent the cryoscopic constant of water ?

Assertion (A): Larger the value of cryoscopic constant of the solvent, lesser will be the freezing point of the solution. Reason (R ): Depression in the freezing point depends on the nature of the solvent.

The freezing point of cyclohexane is 6.5^(@)C . A solution of 0.65g of naphthalene in 19.2g of cyclohexane froze at 1.2^(@)C . What is the molecular mass of naphthalene? The cryoscopic constant for cyclohexane is 20.1 K "mol"^(-1) kg.

Write the units of cryoscopic constant and ebullioscopic constant?

The cryoscopic constant value depends upon:

The cryoscopic constant of water is 1.86 K "mol"^(-1) kg. An aqueous solution of cane sugar freezes at -0.372^(@)C . Calculate the molality of the solution.

A weak electrolyte XY is 5% dissociated in water. What is the freezing point of a 0.01 molal aqueous solution of XY ? The cryoscopic constant of water is 1.86 K/m.

What is the percent by mass of iodine needed to reduce the freezing point of benzene to 3.5^(@)"C" ? The freezing point and cryoscopic constant of pure benzene are 5.5^(@)"C" and 5.12K/m respectively.

0.1 molal solution of Hg(NO_(3))_(2) freezes at 0.558^(@) C. The cryoscopic constant for water is 1.86 KKg mol^(-1) then what will be the percentage ionisation of salt ?

(a) Define dielectric constant. (b) How does dielectric constant affect SN^1 rates ? (c) Explain why solvolyses are much faster in EtOH than in acetone even though both solvents have the same dielectric constants.