Questions tagged [colligative-properties]
Colligative properties of solutions are properties that depend upon the concentration of solute molecules or ions, but not upon the chemical identity of the solute.
23
questions
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1answer
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Relative lowering of vapour pressure
Why is lowering of vapour pressure (Po - Ps) temperature dependent? And why is relative lowering of vapour pressure (1 - Ps/Po) independant of temperature?
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3answers
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How much salt (or any other substance one can find in a kitchen) do I need to add to make water boil at 104 °C? [closed]
I've seen some formulas around in other questions and Google searches, but my chemistry is pretty much dead so I have no clue where to find the relevant values to calculate it myself. I just need to ...
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1answer
34 views
Is vapour pressure a surface phenomenon?
As a fact, I know that vapour pressure doesn't depend on surface area.
Does this imply it is not a surface phenomenon also?
It shouldn't be as then it would depend on surface area of molecules and ...
1
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0answers
23 views
Freezing point lowering for a mixture of many liquids
I have been taught that if I have a solute of molality $m$ mixed with a liquid, the freezing point in lowered by an amount $K_\mathrm{f}\cdot m$ where $K_\mathrm{f}$ is the molal freezing depression ...
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0answers
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Does the mole fraction of a solution change with Vant Hoff factor?
I reason that as mole fraction is a measure of colligative properties, increase in the Vant Hoff factor ( and hence increase in the value of colligative properties) should also leave a mark on the ...
2
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3answers
990 views
Why do colligative properties depend only on number of solute particles?
Colligative properties depend solely on the number of even though the interactive forces are different for different solute-solvent pairs. So why is the dependence only on the number of solute?
2
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1answer
561 views
Is there any difference between isotonic and isosmotic solution?
Is there any difference between isotonic and isosmotic solution? Can we say isotonic solution do not show osmosis because they have same osmotic pressure?
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1answer
50 views
What happens to depression when two solutions are mixed? [closed]
Equal volumes of $\pu{1.0 M}$ $\ce{KCl (aq)}$ and $\pu{1.0 M}$ $\ce{AgNO3 (aq)}$ solutions are mixed. The depression of freezing point of the resulting solution (with respect to water) will be (assume ...
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2answers
63 views
Intuitive explanation for depression of freezing point
Why does depression of freezing point takes place if a non-volatile solute is added to the solution?
For more details about the question checkout this link below
Depression of freezing point
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1answer
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Why it is very rare to find a compound that lacks carbon to be liquid at standard temperatures and pressures?
It is the first time I heard such a generalization, I had no idea. Why being liquid in standard conditions is special to compounds which contain carbon atom? Which property of carbon cause this?
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1answer
99 views
Proper explanation for depression of freezing point [closed]
Why does depression of freezing point takes place if a non-volatile solute is added to the solution?
Depression of freezing point
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1answer
136 views
Depression of freezing point [closed]
Recently, I learnt that by adding a non-volatile solute to a solvent, the vapour pressure of the solution is decreased and consequently its boiling point.
Facts and definitions
freezing point: "The ...
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votes
1answer
345 views
Why does freezing point decrease when vapour pressure decreases in dilute solutions?
I was studying colligative properties of dilute solutions, and one of the properties was freezing point depression. The confusion I had was that, if vapour pressure decreases, it should be easier to ...
0
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1answer
80 views
What happens to the gas inside cold drinks as the cold drink is frozen?
According to Henry's law the amount of gas dissolved is directly proportional to the pressure exerted by a gas on the surface of the liquid.
And we know if we increase the temperature, the amount of ...
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1answer
294 views
Finding molar mass of naphthalene using the freezing point of a solution?
Naphthalene is the main ingredient in some mothballs. The freezing
point of a solution made by dissolving $\pu{7.01 g}$ of naphthalene in $\pu{200 g}$
of benzene is $4.20 \pu{^\circ C}$ . What is ...
2
votes
0answers
4k views
Why is osmotic pressure the best colligative property? [closed]
The osmotic pressure method has the advantage over
other methods as pressure measurement is around the room
temperature and the molarity of the solution is used instead of molality.
As compared ...
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0answers
90 views
How does dry air get saturated in the Ostwald-Walker Method?
This question was already asked and this was the answer that was posted:
"So basically, before you start the experiment the vapors have already formed, meaning that thermodynamic equilibrium has been ...
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0answers
204 views
Is my proof valid for the formula of elevation in boiling point? [closed]
Is my proof valid for the formula of elevation in boiling point?
proof
By Clausius clayperon equation,
$$\ln(P)=-\frac{∆H_v}{RT}+c$$
Differentiating,
$$\frac{dP}{...
2
votes
0answers
106 views
Why does only a single azeotropic composition exist for a mixture of two given substances?
In the image below, which represents a generic composition vs. temperature plot for a mixture, there is a single intersection point between the vapor and liquid curves. This is due to the fact that ...
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1answer
3k views
How to determine the highest freezing point by van't hoff factor when concentration is same? [closed]
Whch of the following will have the highest freezing point?
a) 0.1M KCl
b) 0.1M glucose
c) 0.1M BaCl2
d) 0.1M AlCl3
3
votes
1answer
126 views
How do repulsive solute interactions affect the van't Hoff factor?
Context. Consider an ideal solution, one in which the intermolecular solvent-solvent, solute-solute, and solute-solvent interactions are all equal. The presence of a solute therefore produces (solely) ...
4
votes
1answer
994 views
Relationship between freezing point depression and hydrogen bonds
Freezing point of a solvent is decreased due to the added solute particles in it. e.g. ions. Therefore electrolytes contribute to lowering freezing point (say for physiological conditions).
If a ...
2
votes
1answer
101 views
Order of molecular mass of solvent; given boiling point [closed]
Given three solvents X, Y, Z. Order of boiling point of pure solvent X < Y < Z and same order of molal elevation constant ($K_\mathrm{b}$). Find the order of molecular mass.
So I got this ...
