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log 10 of Acetonitrile vapor pressure. Uses formula log e P m m H g = {\displaystyle \scriptstyle \log _{e}P_{mmHg}=} log e ( 760 101.325 ) − 3.881710 log e ( T + 273.15 ) − 4999.618 T + 273.15 + 41.05901 + 3.515956 × 10 − 06 ( T + 273.15 ) 2 {\displaystyle \scriptstyle \log _{e}({\frac {760}{101.325}})-3.881710\log _{e}(T+ ...
2.79 6.55 –20.2 Diethyl ether: 0.713 34.5 2.16 –116.3 –1.79 K b & K f [1] Methanol [4] 0.79 64.7 Ethanol: 0.78 78.4 1.22 –114.6 –1.99 K b [2] Ethylene bromide: 2.18 133 6.43 9.974 –12.5 K b & K f [1] Ethylene glycol: 1.11 197.3 2.26 −12.9 –3.11 K b & K f [1] Formic acid: 101.0 2.4 8.0 –2.77 K b & K f [1] Naphthalene: 217.9 78. ...
The hydride surface can also be functionalized with carboxylic acids [2] and long-chain alkyl groups. [2] Mobile phases for ANPC are based on organic solvents as bulk solvents (such as methanol or acetonitrile) with a small amount of water as a modifier of polarity; thus, the mobile phase is both "aqueous" (water is present) and "normal phase ...
Polar aprotic solvents: acetone (CH 3) 2 CO 56.1 °C 21.8 0.785 g/cm 3: 2.91 reacts with strong acids and bases acetonitrile : CH 3 CN 82 °C 38.3 0.776 g/cm 3: 3.20 reacts with strong acids and bases dichloromethane: CH 2 Cl 2: 39.6 °C 9.08 1.327 g/cm 3: 1.6 low boiling point dimethylacetamide (CH 3) 2 NCOCH 3: 165 °C 37.8 0.94 g/cm 3: 3.72 ...
In the table above, it can be seen that water is the most polar-solvent, followed by DMSO, and then acetonitrile. Consider the following acid dissociation equilibrium: HA ⇌ A − + H + Water, being the most polar-solvent listed above, stabilizes the ionized species to a greater extent than does DMSO or Acetonitrile.
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 (in binary azeotropes, when only one fraction is given, it is the fraction of the second component), the boiling point (b.p.) of a component, the boiling point of a mixture, and the specific gravity of the mixture.
The following table lists the Van der Waals constants (from the Van der Waals equation) for a number of common gases and volatile liquids. [ 1 ] To convert from L 2 b a r / m o l 2 {\displaystyle \mathrm {L^{2}bar/mol^{2}} } to L 2 k P a / m o l 2 {\displaystyle \mathrm {L^{2}kPa/mol^{2}} } , multiply by 100.
Here is a similar formula from the 67th edition of the CRC handbook. Note that the form of this formula as given is a fit to the Clausius–Clapeyron equation, which is a good theoretical starting point for calculating saturation vapor pressures: