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Alekssandra [29.7K]
2 years ago
6

The freezing point of a 1.00 molal aqueous solution of calcium chloride (CaCl2) is lower than the freezing point of a 1.00 molal

aqueous solution of ethylene glycol (C2H6O2). Why are the freezing points of the two solutions different?
Chemistry
1 answer:
chubhunter [2.5K]2 years ago
7 0

Answer:

The calcium chloride is an electrolyte salt, so the frezzing point of solution must be higher than ethylene glycol.

Explanation:

This is the colligative property for this question: Frezzing point depression

ΔTf = Kf · molal · i

ΔTf = T° fussion solvent pure - T° fussion solution

As both solutions are the same in molality and the solvent is water, the formula stands the same but the Calcium Chloride is a salt which is dissociated in water like this:

CaCl₂ → Ca²⁺  + 2Cl⁻

We have 3 moles of ions, so this value modiffy the formula with the Van't Hoff Factor (number of ion particles per individual molecule of solute).

Ethyleneglycol  is a non-electrolytic organic compound (It is often used 1 as the i).

Let's see the formula in both:

0° - T° fussion solution = Kf · molal · 3 → CaCl2

0° - T° fussion solution = Kf · molal · 1 → C2H6O2

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scZoUnD [109]
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A 1.00 liter solution contains 0.24 M hypochlorous acid and 0.31 M sodium hypochlorite. If 0.160 moles of potassium hydroxide ar
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Explanation:

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since water is formed, this maintains the pH.  Thus ...

A. The number of moles of HClO will decrease. - TRUE

B. The number of moles of ClO- will increase. - TRUE

C. The equilibrium concentration of H3O+ will remain the same. - TRUE

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Answer:

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Explanation:

Hello!

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We can see there is a 2:1 mole ratio between the acid and the base; thus, at the equivalent point we can write:

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