# Freezing point and boiling relationship

### Melting Point, Freezing Point, Boiling Point

Solutes in the liquid phase also raise the equilibrium boiling temperature. Pressure also affects freezing temperature (a little) and boiling temperatures (a lot). Raoult's Law; boiling point elevation; freezing point depression This relationship can be useful for calculating the molecular weight of an unknown solid. Liquids have a characteristic temperature at which they turn into solids, known as their freezing point. In theory, the melting point of a solid should be the same.

The gain in disorder on evaporation is now less, because the liquid water in solution is more disordered. The energy effect is hardly changed, so the energy effect now dominates over a slightly larger range: So the boiling temperature is higher for a solution. Conversely, when we look at melting, the disorder effect is greater for a solution: So the disorder effect can dominate even at lower temperatures.

• Mixtures and solutions

So the freezing temperature is lower for a solution. I mentioned the equilibrium freezing and boiling temperatures above. If we add a little heat, some ice melts. Remove a little heat and some water freezes. We call this the equilibrium freezing temperature: More about supercooling and super heating below. An aqueous solution has a higher boiling point and a lower freezing point than does pure water. If the solution is not too concentrated, these two effects are approximately independent of what the dissolved substance is: So, provided you remember to count each ion separately, the effect of concentration on boiling point elevation or freezing point depression is much the same for all small solutes in water.

Macromolecules such as polymers behave differently because they have lots of neighbouring solvent molecules, and so affect the solvent much more than simple solutes. So, you might expect that the antifreeze in a radiator not only stops it freezing, but also helps stop it from boiling.

However, the real situation is more complicated: Ethylene glycol is one antifreeze. Salt is used to melt snow and ice on roads in cold countries, but it is not used in radiators because it is corrosive and crystallises readily. Sugar is not used in some applications, because concentrated sugar solutions are viscous, and because they support bugs. However, many organisms use sugars and other small organic molecules as antifreeze.

The concentration of solutes in blood is less than that in sea water, so the equilibrium freezing temperature of blood is usually higher than that of sea water.

Consequently, some Arctic and Antarctic fish live at temperatures below the equilibrium freezing temperature of normal blood. The bio-antifreeze in their blood is a protein that works in a way different from the anti-freeze used in car radiators: The effect of pressure Notice that above I've included the proviso "at atmospheric pressure" a few times.

The reason why the pressure is important is that, in the vapour phase, a given amount of a substance occupies a much larger volume than it does as a liquid.

### Freezing and Boiling

Some of the energy required to vapourise it goes towards 'pushing the air out of the way' to make room for the amount evaporated. So, at low pressure, it is easier to form the vapour phase and so the boiling point is lower. The dependence of the transition temperature on pressure is the Clausius-Clapeyron effect.

Again, being a bit technical, we note that this effect involves energy - the work done in displacing air - whereas the solute effect involves entropy - the disordering of the liquid phase. Water expands a lot when it boils: This means that even modest increases in altitude can measurably reduce the boiling temperature. Some people complain that this affects cooking and even the taste of tea at altitude.

Boiling Point of Water

It is also true that pressure changes the melting temperature. However, because the volume occupied by a kilogram of liquid is not much different from that occupied by a kilogram of solid, this effect is very small unless the pressures are very large. For most substances, the freezing point rises, though only very slightly, with increased pressure.

Water is one of the very rare substances that expands upon freezing which is why ice floats. Consequently, its melting temperature falls very slightly if pressure is increased.

## Freezing and Boiling Points

I have been asked: Does freezing point depression with pressure explain the low friction under an ice-skate? I'm writing this in Sydney, so you might guess correctly that I don't know much about skating, but let's try to be quantitative.

The Clausius-Clapeyron equation says that the ratio of the change in pressure times the change in specific volume to the latent heat of the phase change equals the ratio of the change in transition temperature to the absolute melting or boiling temperature.

As we might have guessed from dimensional considerations — i. The weight of the skater is say 1 kN. I'm not a skater, but let's start with an estimate of the skate-ice contact area as say mm2. The value depends on how far the skate cuts into the ice.

Say mm long by 0. A kg of water one litre freezes to give about 1. So, with this estimate for area and if this were the cause of the slipperiness, ice skating would be possible only at temperatures only one or a few degrees below freezing. Mixtures also tend to melt at temperatures below the melting points of the pure solids.

Boiling Point When a liquid is heated, it eventually reaches a temperature at which the vapor pressure is large enough that bubbles form inside the body of the liquid. This temperature is called the boiling point.

Once the liquid starts to boil, the temperature remains constant until all of the liquid has been converted to a gas.

The normal boiling point of water is oC. But if you try to cook an egg in boiling water while camping in the Rocky Mountains at an elevation of 10, feet, you will find that it takes longer for the egg to cook because water boils at only 90oC at this elevation. In theory, you shouldn't be able to heat a liquid to temperatures above its normal boiling point. Before microwave ovens became popular, however, pressure cookers were used to decrease the amount of time it took to cook food. In a typical pressure cooker, water can remain a liquid at temperatures as high as oC, and food cooks in as little as one-third the normal time.

To explain why water boils at 90oC in the mountains and oC in a pressure cooker, even though the normal boiling point of water is oC, we have to understand why a liquid boils. By definition, a liquid boils when the vapor pressure of the gas escaping from the liquid is equal to the pressure exerted on the liquid by its surroundings, as shown in the figure below. Liquids boil when their vapor pressure is equal to the pressure exerted on the liquid by its surroundings. The normal boiling point of water is oC because this is the temperature at which the vapor pressure of water is mmHg, or 1 atm.

Under normal conditions, when the pressure of the atmosphere is approximately mmHg, water boils at oC. At 10, feet above sea level, the pressure of the atmosphere is only mmHg. At these elevations, water boils when its vapor pressure is mmHg, which occurs at a temperature of 90oC. Pressure cookers are equipped with a valve that lets gas escape when the pressure inside the pot exceeds some fixed value. This valve is often set at 15 psi, which means that the water vapor inside the pot must reach a pressure of 2 atm before it can escape.

Because water doesn't reach a vapor pressure of 2 atm until the temperature is oC, it boils in this container at oC. Liquids often boil in an uneven fashion, or bump. They tend to bump when there aren't any scratches on the walls of the container where bubbles can form.