Introduction to Elevation of Boiling Point
The elevation of the boiling point refers to the rise of a solvent's boiling point upon the addition of a solute. The resulting solution has a higher boiling point when a non-volatile solute is applied to a solvent than that of the pure solvent. The boiling point of sodium chloride (salt) solution and water, for example, is higher than that of pure water.
The elevation of boiling points is a colligative property of matter, i.e., it depends on the solvent-to-solvent ratio but not on the identity of the solute. This means that the elevation of a solution's boiling point depends on the amount of solution applied to it. The higher the solute concentration in the solution, the greater the elevation of the boiling point.
Boiling Point Elevation
The vapor pressure of a solvent can decrease when a solution is applied. This occurs because of the solute displacement of solvent molecules. This means that some of the solvent molecules on the liquid's surface are replaced by the solvent; both electrolytic and non-electrolytic solutions will occur. The lower number of solvent molecules on the surface means that less can evaporate, thus reducing the vapor pressure. A higher temperature is needed for the vapor pressure to equal the ambient pressure, and a higher boiling point is observed.
A graph describing the elevation at the boiling point of water when sucrose is added is given above. At a pressure of 1atm, pure water boils at 100\[^{\circ}C\]. However, in water, a 10-molal solution of sucrose boils at around 105\[^{\circ}C\].
Why Does Boiling Point Elevation Occur?
The temperature at which its vapor pressure is equal to the pressure of its surrounding atmosphere is the boiling point of a liquid. Non-volatile liquids do not evaporate quickly and have very low vapor pressures (assumed to be zero). The vapor pressure of the resulting solution is lower than that of the pure solvent when a non-volatile solute is applied to the solvent.
Therefore the solution must be supplied with a larger amount of heat for it to boil. The boiling point elevation is this rise in the solution's boiling point. A rise in the concentration of the added solution is followed by a further decrease in the solution's vapor pressure and a further increase in the solution's boiling point.
A temperature graph of pressure v/s detailing the boiling point elevation of a solution is given below.
Here, ΔTb represents the elevation of the solution's boiling point. It can be observed from the graph that:
The solution's freezing point is lower than that of the pure solvent (freezing point depression).
The solution's boiling point is higher than that of the pure solvent.
Note: The liquid's boiling point often depends on the pressure of its surroundings (which is why water boils at temperatures lower than 100\[^{\circ}C\] at high altitudes, where the surrounding pressure is low).
Boiling Point Elevation Formula
The boiling point of a non-volatile solute containing solution can be expressed as follows:
Boiling point of solution = pure solvent boiling point + elevation of the boiling point.
The boiling point elevation (ΔTb) is proportional to the solute concentration in the solution. The following equation allows it to be measured.
ΔTb = i*Kb*m
Where,
It is the Van’t Hoff factor.
Kb is the ebullioscopic constant.
m is the molality of the solute.
It is important to remember that when the solute concentration is very high, this formula becomes less accurate. Also, this formula for volatile solvents does not hold true.
In terms of\[^{\circ}C\] /molal, or\[^{\circ}C\].kg.mol-1, the ebullioscopic constant (Kb) is also expressed. Below the Kb values for some common solvents are tabulated.
Kb Values for Some Common Solvents
With the support of the boiling point elevation formula, the degree of dissociation of the solute and the molar mass of the solute can be measured.
The Relationship Between Boiling Point Elevation and Vapor Pressure
In terms of vapor pressure, boiling point elevation can be clarified. Vapor pressure is defined as the pressure exerted at a given temperature by a vapor in thermodynamic equilibrium with its condensed phases. It is simply a measure of the ability of the solvent molecules, in layman's words, to escape by entering the gas phase. When the vapor pressure is equal to the air pressure, a liquid boils.
Boiling Point - The boiling point of a liquid in its purest form. The liquid can boil when the vapor pressure of the liquid equals the ambient pressure.
What do we Mean by Boiling Point Elevation?
By the term boiling point elevation we mean the increase in the boiling point of a solvent after a solute is added. So when any non volatile solute is added to the solvent then the result solution has a higher boiling point that the pure solvent. Like for instance the boiling point of the solution chloride that is salt coupled with water is prominent than the pure water. However the boiling point elevation is a colligative property of matter as it depends on the solute to solvent ratio and not on the identity of the solute. This means that the elevation in the boiling point of solution is dependent on the amount of solute that gets added. Hence the greater the concentration of solute is there in the solution then greater will be the boiling point elevation.
Why does Boiling Point Elevation happen?
However the boiling point of a liquid is perhaps the temperature at which the vapour pressure is equal to the pressure of its nearby environment. Moreover non-volatile substances do not actually undergo evaporation and have low vapour pressures which we can assume to be at 0. However when the non-volatile solute is given to the solvent then the vapor pressure of the resulting solution is lower than the pure solvent. Henc the increased amount of heat should be supplied to the solution so that it can boil. This increase in the boiling point of the solution is known as boiling point elevation.
However if this is put in vapour pressure terms the liquid boils at the temperature when the vapor pressure becomes equal to the surrounding pressure. However for the solvent if the solute is present it will decrease its vapor pressure by dilution.
What is the Use of Boiling Point Elevation?
The boiling point election and formulas used for boiling point elevation can be used to weigh the degree of dissociation or the molar mass of the solute. However this type of measurement is known as ebullioscopy which is a Greek term for boiling viewing. However the cryoscopic constant which says that the freezing point depression is larger than the ebullioscopic constant. But the freezing point is easy to measure with accuracy and is commonly used in cryoscopy.
FAQs on Elevation Boiling Point
1. Explain boiling point elevation with examples?
Salted water's boiling point is higher than pure water's boiling point. Salt is an electrolyte that dissociates into solution ions, thereby having a relatively significant effect on the point of boiling. Remember that non-electrolytes, including sugar, often raise the boiling point. However, since a nonelectrolyte does not dissociate to form several particles, the effect per mass is less than that of a soluble electrolyte.
Boiling Point Elevation Equation -
A combination of the Clausius-Clapeyron equation and Raoult's law is the formula used for measuring boiling point elevation. It is believed that the solvent is non-volatile.
ΔTb = Kb · bB
where,
ΔTb is the boiling point elevation.
Kb is the ebullioscopic constant, which depends on the solvent.
bB is the molality of the solution (typically found in a table).
Thus, boiling point elevation is directly proportional to a chemical solution's molal concentration.
2. 10 grams of a non-volatile and non-dissociating solute is dissolved in 200 grams of benzene. the resulting solution boils at a temperature of 81.2℃. find the molar mass of the solute.
Let x = number of moles of solute. The boiling point of pure benzene is 80.1\[^{\circ}C\] and its ebullioscopic constant is 2.53\[^{\circ}C\]/molal. From the boiling point elevation formula, the following relationship can be obtained:
(81.2\[^{\circ}C\] – 80.1\[^{\circ}C\]) = (1)\[\times\](2.53\[^{\circ}C\].kg.mol-1)(x/0.2 kg).
x = \[\frac{(1.1^{\circ}C \times 0.2kg)}{(2.53^{\circ}C.kg.mol^{-1})}.\]
x = 0.0869 moles.
Since 0.0869 moles of the solute has a mass of 10 grams, 1 mole of the solute will have a mass of 10/0.0869 grams, which is equal to 115.07 grams. Therefore, the molar mass of the solute is 115.07 grams per mole.
3. What do you understand by colligative properties and boiling point elevation?
However there is one category of property which we can apply to solutions this is called as colligative properties. Moreover these properties are known colligative only if these are dependent on the amount of solute that is present in the solution irrespective of the identity of the solution. Likewise the boiling point of the solvent will help be increased when the solute is broken down in it. This is what we call a boiling point elevation.
4. Define the relationship between vapor pressure and boiling point elevation.
However we can explain the boiling point elevation in terms of vapor pressure. Moreover the vapor pressure is known to be the pressure that is applied by the vapor in thermodynamic equilibrium with its liquid phases at any given temperature. To put it in simple words it is the tendency of the solution molecules to escape by entering the gas phase. Hence a liquid boils only when its vapor pressure is equal to the air pressure. The boiling point of a pure liquid is when the vapour pressure of the liquid is equal to the atmospheric pressure then the liquid will boil.
5. How can we use boiling point elevation in real life?
However one area that we can apply the boiling point elevation is cooking. There are many recipes where the salt needs to be added to water before it boils for the purpose of seasoning the water which is not necessary. Hence if you salt the water it will increase its boiling point and it will take more time for the water to boil then the usual time it takes.
6. Why do you think the boiling point elevation is important?
If you raise the boiling point then it will help to protect it against the boil overs. You will see there are many brands of antifreeze that will tell you about the amount of protection of boil-over and the freeze up protection that it offers. The antifreeze will help to avoid the water in your vehicle’s radiator to keep away from freezing through the freezing point depression.
7. Why do you think molality is used for colligative properties?
Colligative properties are the physical properties of the solution like the boiling point elevation and the freezing point depression. However in these calculations as we add more solute to the solvent the temperature of the solution changes which means the volume of the solution changes. As molarity is moles solute per liter of solution hence molarity cannot be used as a concentration unit.
