Chriselc03idn
Answered

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What is the Freezing Point of a solution that contains 1.25 mol of CaCl2 ( Cl = 35.5 ) in 1400 g of water?

a. -5 deg. celsius
b. 5 deg. celsius
c. 105.5 deg. celsius

Sagot :

Indrawboyidn

The freezing Point of a solution : -1.661 °C(no option)

Further explanation  

Solution properties are the properties of a solution that don't depend on the type of solute but only on the concentration of the solute.  

The term is used in the Solution properties  

1. molal  

that is, the number of moles of solute in 1 kg of solvent  

[tex]\tt m=\dfrac{mol~solute}{mass~1~kg~solvent}[/tex]

2. freezing point  

Solutions from volatile substances have a higher boiling point and lower freezing points than the solvent  

[tex]\tt \Delta Tf=Kf\times m[/tex]

ΔTf = Tf solvent - Tf solution

Kf = The molal freezing point depression constant

m = molal solution  

Given

1.25 mol CaCl₂

1400 g water = 1.4 kg

Required

The freezing point

Solution

molal of the solution :

= mol : kg solvent(water)

= 1.25 mol : 1.4 kg

= 0.893

The freezing point :

Tf solvent = 0 °C(for water)

Kf water = 1.86 °C/m

Input the value :

ΔTf = Tf solvent - Tf solution  = Kf . m

0 - Tf solution = 1.86 °C/m . 0.893

0 - Tf solution = 1.661

Tf solution = - 1.661 °C

Learn more  

the vapor pressure of the glucose solution  

https://brainly.ph/question/2746258  

The molecular mass of organic compound  

https://brainly.ph/question/2741540  

The molecular weight of nonvolatile nonelectrolyte substance  

https://brainly.ph/question/2740419  

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