List of boiling and freezing information of solvents

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SolventDensity (g cm-3)Boiling point (°C) Kb (°C⋅kg/mol)Freezing point (°C) Kf (°C⋅kg/mol)Data source
Aniline 184.33.69–5.96–5.87Kb & Kf [1]
Lauric acid 298.944–3.9
Acetic acid 1.04117.93.1416.6–3.90Kb [1] Kf [2]
Acetone 0.7856.21.67–94.8Kb [3]
Benzene 0.8780.12.655.5–5.12Kb & Kf [2]
Bromobenzene 1.49156.06.26–30.6
Camphor 204.05.95179–40Kf [2]
Carbon disulfide 1.2946.22.34–111.5–3.83
Carbon tetrachloride 1.5876.84.88–22.8–29.8Kb & Kf [1]
Chloroform 1.4861.23.88–63.5–4.90Kb & Kf [1]
Cyclohexane 80.742.796.55–20.2
Diethyl ether 0.71334.52.16–116.3–1.79Kb & Kf [1]
Methanol [4] 0.7964.7
Ethanol 0.7878.41.22–114.6–1.99Kb [2]
Ethylene bromide 2.181336.439.974–12.5Kb & Kf [1]
Ethylene glycol 1.11197.32.26−12.9–3.11Kb & Kf [1]
Formic acid 101.02.48.0–2.77Kb & Kf [1]
Naphthalene 217.978.2–6.80
Nitrobenzene 210.85.245.7–7.00
Phenol 181.753.6043.0–7.27Kf [2] Kb [1]
Water 100.000.5120.00–1.86Kb & Kf [2]
Ethyl Acetate 77.1 [5]
Acetic Anhydride 139.0 [6]
Ethylene Dichloride 1.2583.5−35 [7]
Acetonitrile 0.7881.6−45 [8]
Heptane 98.4 [9]
Isobutanol 107.7 [10]
n-Hexane 0.6668.7 [11]
n-Butanol 117.7 [12]
Hydrochloric Acid 84.8 [13]
tert-Butanol 82.5 [14]
Chlorobenzene 131.7 [15]
p-chlorobenzotrifluoride 1.34136–36.1 [16]
MTBE 55.2 [17]
Pentane 36.1 [18]
Petroleum Ether 35.0-60.0 [19]
Cyclopentane 49.3 [20]
Isopropanol 82.3 [21]
Dichloromethane 1.3339.8 [22]
n-Propanol 97.2 [23]
Pyridine 115.3 [24]
Dimethylacetamide 166.1 [25]
Tetrahydrofuran 66.0 [26]
Dimethylformamide 153.0 [27]
Toluene 0.82110.6 [28]
Dimethyl Sulfoxide 189.0 [29]
Trifluoroacetic Acid 71.8 [30]
Dioxane 1.03101.011.8 [31]
Xylene 140.0 [32]

See also

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<span class="mw-page-title-main">Boiling point</span> Temperature at which a substance changes from liquid into vapor

The boiling point of a substance is the temperature at which the vapor pressure of a liquid equals the pressure surrounding the liquid and the liquid changes into a vapor.

<i>Cis</i>–<i>trans</i> isomerism Pairs of molecules with same chemical formula showing different spatial orientations

Cis–trans isomerism, also known as geometric isomerism, describes certain arrangements of atoms within molecules. The prefixes "cis" and "trans" are from Latin: "this side of" and "the other side of", respectively. In the context of chemistry, cis indicates that the functional groups (substituents) are on the same side of some plane, while trans conveys that they are on opposing (transverse) sides. Cis–trans isomers are stereoisomers, that is, pairs of molecules which have the same formula but whose functional groups are in different orientations in three-dimensional space. Cis and trans isomers occur both in organic molecules and in inorganic coordination complexes. Cis and trans descriptors are not used for cases of conformational isomerism where the two geometric forms easily interconvert, such as most open-chain single-bonded structures; instead, the terms "syn" and "anti" are used.

<span class="mw-page-title-main">Paraffin wax</span> Soft colorless solid derived from petroleum, coal or shale oil

Paraffin wax is a soft colorless solid derived from petroleum, coal, or oil shale that consists of a mixture of hydrocarbon molecules containing between 20 and 40 carbon atoms. It is solid at room temperature and begins to melt above approximately 37 °C (99 °F), and its boiling point is above 370 °C (698 °F). Common applications for paraffin wax include lubrication, electrical insulation, and candles; dyed paraffin wax can be made into crayons.

<span class="mw-page-title-main">Solution (chemistry)</span> Homogeneous mixture of a solute and a solvent

In chemistry, a solution is defined by IUPAC as "A liquid or solid phase containing more than one substance, when for convenience one substance, which is called the solvent, is treated differently from the other substances, which are called solutes. When, as is often but not necessarily the case, the sum of the mole fractions of solutes is small compared with unity, the solution is called a dilute solution. A superscript attached to the ∞ symbol for a property of a solution denotes the property in the limit of infinite dilution." One important parameter of a solution is the concentration, which is a measure of the amount of solute in a given amount of solution or solvent. The term "aqueous solution" is used when one of the solvents is water.

<span class="mw-page-title-main">Solvent</span> Substance dissolving a solute resulting in a solution

A solvent is a substance that dissolves a solute, resulting in a solution. A solvent is usually a liquid but can also be a solid, a gas, or a supercritical fluid. Water is a solvent for polar molecules, and the most common solvent used by living things; all the ions and proteins in a cell are dissolved in water within the cell.

<span class="mw-page-title-main">Azeotrope</span> A mixture of two or more liquids whose proportions do not change when the mixture is distilled

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<span class="mw-page-title-main">Colligative properties</span> Properties of solutions that depend only on the number of solute particles

In chemistry, colligative properties are those properties of solutions that depend on the ratio of the number of solute particles to the number of solvent particles in a solution, and not on the nature of the chemical species present. The number ratio can be related to the various units for concentration of a solution such as molarity, molality, normality (chemistry), etc. The assumption that solution properties are independent of nature of solute particles is exact only for ideal solutions, which are solutions that exhibit thermodynamic properties analogous to those of an ideal gas, and is approximate for dilute real solutions. In other words, colligative properties are a set of solution properties that can be reasonably approximated by the assumption that the solution is ideal.

<span class="mw-page-title-main">Freezing-point depression</span> Drop in freezing temperature of a solvent due to the addition of solute

Freezing-point depression is a drop in the maximum temperature at which a substance freezes, caused when a smaller amount of another, non-volatile substance is added. Examples include adding salt into water, alcohol in water, ethylene or propylene glycol in water, adding copper to molten silver, or the mixing of two solids such as impurities into a finely powdered drug.

<span class="mw-page-title-main">Pentane</span> Alkane with 5 carbon atoms

Pentane is an organic compound with the formula C5H12—that is, an alkane with five carbon atoms. The term may refer to any of three structural isomers, or to a mixture of them: in the IUPAC nomenclature, however, pentane means exclusively the n-pentane isomer, in which case pentanes refers to a mixture of them; the other two are called isopentane (methylbutane) and neopentane (dimethylpropane). Cyclopentane is not an isomer of pentane because it has only 10 hydrogen atoms where pentane has 12.

<span class="mw-page-title-main">Rotary evaporator</span> Device used in chemical laboratories

A rotary evaporator (rotovap) is a device used in chemical laboratories for the efficient and gentle removal of solvents from samples by evaporation. When referenced in the chemistry research literature, description of the use of this technique and equipment may include the phrase "rotary evaporator", though use is often rather signaled by other language.

Petroleum ether is the petroleum fraction consisting of aliphatic hydrocarbons and boiling in the range 35–60 °C, and commonly used as a laboratory solvent. Despite the name, petroleum ether is not an ether; the term is used only figuratively, signifying extreme lightness and volatility.

This is a list of the various reported boiling points for the elements, with recommended values to be used elsewhere on Wikipedia.

<span class="mw-page-title-main">Hydrogen halide</span> Chemical compound consisting of hydrogen bonded to a halogen element

In chemistry, hydrogen halides are diatomic, inorganic compounds that function as Arrhenius acids. The formula is HX where X is one of the halogens: fluorine, chlorine, bromine, iodine, astatine, or tennessine. All known hydrogen halides are gases at standard temperature and pressure.

<span class="mw-page-title-main">Critical point (thermodynamics)</span> Temperature and pressure point where phase boundaries disappear

In thermodynamics, a critical point is the end point of a phase equilibrium curve. One example is the liquid–vapor critical point, the end point of the pressure–temperature curve that designates conditions under which a liquid and its vapor can coexist. At higher temperatures, the gas comes into a supercritical phase, and so cannot be liquefied by pressure alone. At the critical point, defined by a critical temperatureTc and a critical pressurepc, phase boundaries vanish. Other examples include the liquid–liquid critical points in mixtures, and the ferromagnet–paramagnet transition in the absence of an external magnetic field.

Boiling-point elevation is the phenomenon whereby the boiling point of a liquid will be higher when another compound is added, meaning that a solution has a higher boiling point than a pure solvent. This happens whenever a non-volatile solute, such as a salt, is added to a pure solvent, such as water. The boiling point can be measured accurately using an ebullioscope.

<span class="mw-page-title-main">François-Marie Raoult</span> French physical chemist (1830–1901)

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In thermodynamics, the ebullioscopic constantKb relates molality b to boiling point elevation. It is the ratio of the latter to the former:

This page contains tables of azeotrope data for various binary and ternary mixtures of solvents. The data include the composition of a mixture by weight, the boiling point (b.p.) of a component, the boiling point of a mixture, and the specific gravity of the mixture. Boiling points are reported at a pressure of 760 mm Hg unless otherwise stated. Where the mixture separates into layers, values are shown for upper (U) and lower (L) layers.

<span class="mw-page-title-main">Condenser (laboratory)</span> Laboratory apparatus used to condense vapors

In chemistry, a condenser is laboratory apparatus used to condense vapors – that is, turn them into liquids – by cooling them down.

References

  1. 1 2 3 4 5 6 7 8 9 Eastman. E.D. and Rollefson, G.K. Physical Chemistry 1947 ed. McGraw-Hill p307
  2. 1 2 3 4 5 6 Pauling, Linus: General Chemistry 1970 ed. Dover Publications pp459-460
  3. ↑ Moore, Walter J. Physical Chemistry 1962 ed. Prentice Hall p132
  4. ↑ "Boiling Point of Gases, Liquids & Solids | Toolbox | AMERICAN ELEMENTS ®".
  5. ↑ "Solvent Boiling Points Chart -".
  6. ↑ "Solvent Boiling Points Chart -".
  7. ↑ "Solvent Boiling Points Chart -".
  8. ↑ "Solvent Boiling Points Chart -".
  9. ↑ "Solvent Boiling Points Chart -".
  10. ↑ "Solvent Boiling Points Chart -".
  11. ↑ "Solvent Boiling Points Chart -".
  12. ↑ "Solvent Boiling Points Chart -".
  13. ↑ "Solvent Boiling Points Chart -".
  14. ↑ "Solvent Boiling Points Chart -".
  15. ↑ "Solvent Boiling Points Chart -".
  16. ↑ "P-CHLOROBENZOTRIFLUORIDE".
  17. ↑ "Solvent Boiling Points Chart -".
  18. ↑ "Solvent Boiling Points Chart -".
  19. ↑ "Solvent Boiling Points Chart -".
  20. ↑ "Solvent Boiling Points Chart -".
  21. ↑ "Solvent Boiling Points Chart -".
  22. ↑ "Solvent Boiling Points Chart -".
  23. ↑ "Solvent Boiling Points Chart -".
  24. ↑ "Solvent Boiling Points Chart -".
  25. ↑ "Solvent Boiling Points Chart -".
  26. ↑ "Solvent Boiling Points Chart -".
  27. ↑ "Solvent Boiling Points Chart -".
  28. ↑ "Solvent Boiling Points Chart -".
  29. ↑ "Solvent Boiling Points Chart -".
  30. ↑ "Solvent Boiling Points Chart -".
  31. ↑ "Solvent Boiling Points Chart -".
  32. ↑ "Solvent Boiling Points Chart -".
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