Wikipedia / Cooling bath
Wikipedia / Cooling bath
A cooling bath or ice bath, in laboratory chemistry practice, is a liquid mixture which is used to maintain low temperatures, typically between 13°C and −196°C. These low temperatures are used to collect liquids after distillation, to remove solvents using a rotary evaporator, or to perform a chemical reaction below room temperature (see Kinetic control).
Cooling baths are generally one of two types: (a) a cold fluid (particularly liquid nitrogen, water, or even air) — but most commonly the term refers to (b) a mixture of 3 components: (1) a cooling agent (such as dry ice or ice); (2) a liquid "carrier" (such as liquid water, ethylene glycol, acetone, etc.), which transfers heat between the bath and the vessel; (3) an additive to depress the melting point of the solid/liquid system.
A familiar example of this is the use of an ice/rock-salt mixture to freeze ice cream. Adding salt lowers the freezing temperature of water, lowering the minimum temperature attainable with only ice.
Mixed-solvent cooling baths
Mixing solvents creates cooling baths with variable freezing points. Temperatures between approximately −78°C and −17°C can be maintained by placing coolant into a mixture of ethylene glycol and ethanol, while mixtures of methanol and water span the −128°C to 0°C temperature range. Dry ice sublimes at −78°C, while liquid nitrogen is used for colder baths.
As water or ethylene glycol freeze out of the mixture, the concentration of ethanol/methanol increases. This leads to a new, lower freezing point. With dry ice, these baths will never freeze solid, as pure methanol and ethanol both freeze below −78°C (−98°C and −114°C respectively).
Relative to traditional cooling baths, solvent mixtures are adaptable for a wide temperature range. In addition, the solvents necessary are cheaper and less toxic than those used in traditional baths.
Traditional cooling baths
Water and ice baths
A bath of ice and water will maintain a temperature 0°C, since the melting point of water is 0°C. However, adding a salt such as sodium chloride will lower the temperature through the property of freezing-point depression. Although the exact temperature can be hard to control, the weight ratio of salt to ice influences the temperature:
−10°C can be achieved with a 1:2.5 mass ratio of calcium chloride hemihydrate to ice.
−20°C can be achieved with a 1:3 mass ratio of sodium chloride to ice.
Dry ice baths at −78 °C
Since dry ice will sublime at −78°C, a mixture such as acetone/dry ice will maintain −78°C. Also, the solution will not freeze because acetone requires a temperature of about −93°C to begin freezing.
Safety recommendations
The American Chemical Society notes that the ideal organic solvents to use in a cooling bath have the following characteristics:
Nontoxic vapors.
Low viscosity.
Nonflammability.
Low volatility.
Suitable freezing point.
In some cases, a simple substitution can give nearly identical results while lowering risks. For example, using dry ice in 2-propanol rather than acetone yields a nearly identical temperature but avoids the volatility of acetone (see below).
See also
References
Further reading
External links