- ΔTf = freezing point depression- i = van 't Hoff factor (number of particles the solute dissociates into)- Kf = cryoscopic constant of the solvent (water in this case)- m = molality of the solution Step 2: Identify the known valuesFrom the question, we have:- ΔTf=0.372K- Kf...
Depression in freezing point for 1 M urea, 1 M NaCl and 1 MCaCl2are in the ratio of View Solution Equimolal solutions will have the same boiling point, provided they do not show View Solution Doubtnut is No.1 Study App and Learning App with Instant Video Solutions for NCERT Class 6, ...
To solve the question regarding which equimolar solution has the highest freezing point, we can follow these steps:Step 1: Understand the Freezing Point Depression The freezing point depression (\( \Delta Tf \)) is given by the
The molal elevation constant of water =0.52 K m^(-1). The boiling poin... 02:08 The ratio of freezing point depression values of 0.01 M solutions of u... 05:06 From a measurement of the freezing point depression of benzene, the mo... 01:36 An aqueous solution containing an ionic...
The freezing point depression constant for water is -1.86^(@)Cm^(-1).i... 03:22 Equal volumes of M/20 urea solution and M/20 glucose solution are mixe... 01:39 Assuming the salts to be unionised in solution, which of the following... 02:30 Pure benzne freezes at 5.3^(@)C....
The freezing point of one molal NaCl solution assuming NaCI to be 100% dissociated in water is (molal depression constant is 1.86)
The molal freezing point constant of water is 1.86Km−1. If 342g of cane sugar (C12H22O11) is dissolved in 1000g of water, the solution will freeze at A−1.86∘C B1.86∘ C−3.92∘C D2.42∘CSubmit The molar freezing point constant for water is 1.86∘C/ molal ...
The molal elevation constant of water is 0.51. The boiling point of 0.1 molal aqueous NaCl solution is nearly : A100.05∘C B100.1∘C C100.2∘C D101.0∘CSubmit The boiling point of 0.1 molal aqueous solution of urea is 100.18∘C atm. The molal elevation constant of water...
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The formula for depression in freezing point is:ΔTf=Kf⋅i⋅mWhere:- Kf is the freezing point depression constant (1.86°C kg/mol for water),- i is the van 't Hoff factor (number of particles the solute dissociates into),- m is the molality of the solution (0.2 molal). ...