What law or formula discusses the relationship between pressure and dew point? A lot of times, dew point is focused primarily upon temperature and relative humidity. However, that same point of saturation is affected by the pressure, but I can't find a formula, or law even, that discusses this. 
It's possible that my premise of the relationship between dew point and pressure may be inaccurate, but if so, how can we then explain that a refrigerant may be a vapor at 210°F in a 280psi container, have a dew point of 125°F, but also be a vapor at 75°F in a 70psi container. 
Whether the substance is water, freon, or any liquid, there should be relationships between pressure and dew points (saturation points, condensation points, etc - they're all meaning the same thing). We can clearly see with freon there's some relationship between pressure and temperatures where the rate of condensation is greater than that of the evaporation, but I can't seem to find any laws/formulas for this.
 A: For single-component liquids, boiling point = condensation point. Both are the same temperature for a given pressure. Let's talk boiling.
Liquids boil when the vapor pressure of the liquid equals the pressure of the surrounding gas (e.g. 1 atm for open containers at sea level). As you raise the temperature of a liquid, the vapor pressure increases until it equals the pressure of the surrounding gas at which point it boils. If you reduce the pressure of the surrounding gas, then you do not need to raise the temperature of the liquid as much anymore. This is why water boils at 82 C instead of 100 C on Everest-- because the atmospheric pressure is lower:

If you have the vapor pressure $P_1$ of a pure substance at one temperature $T_1$ you can calculate the vapor pressure $P_2$ at a second temperature $T_2$ using the Clausius-Clapeyron equation:
$$
\ln\frac{P_2}{P_1} = \frac{-\Delta H_{vap}}{R}\left(\frac{1}{T_2} - \frac{1}{T_1}\right)
$$
where 
$P$ = vapor pressure  
$\Delta H_{vap}$ = enthalpy of vaporization in $J/mol$ 
$R$ = the gas constant = $8.3145\ J/mol \cdot K$ 
$T$ = temperature in $K$ 
A: Even though I am not an expert on this, I found some information that can help. Check out this website
https://www.vaisala.com/sites/default/files/documents/Dew-point-compressed-air-Application-note-B210991EN-B-LOW-v1.pdf
and this website 
https://en.wikipedia.org/wiki/File:Dewpoint.jpg
A: The common use of the term "dew point" is actually the "Atmospheric Dew Point" which doesn't take account the pressure of a system, as it's presumed to be at 1 atm. Many readily found formulas on dew point are formulas for atmospheric dew point, as they focus solely on temperature and the amount of gas (eg. water vapor) trapped the air. 
The other important variable in what affects dew point is the pressure, which is where Pressure Dew Point (PDP) comes into play. 
As a rule of thumb (without the use of complex equations), compression increases/raises the dew point temperature and expansion/decompression lowers the dew point. 
This makes sense considering if you have a fixed amount of vapor in the air, and expand/decompress that vapor, the overall percentage of moisture in the air will be smaller, meaning the relative humidity percentage will decrease, and therefore lower the dew point. 
At this point, the standard atmospheric dew point formulas can then be applied to find dew points at different levels of pressure.
As an actual example, the dew point for a parcel of air at 200 PSIg would have a dew point at -40°F, whereas the same parcel at 5 PSIg, significantly less compressed than the 200 PSIg parcel, would have a dew point of -77°F.
This has important applications in really understanding how things fully work like heat pumps, air dryers, food processing plants, electronics manufacturing, and more.
