User:Michaelmok1010/Boiling-point elevation
 | This is the sandbox page where you will draft your initial Wikipedia contribution.
If you're starting a new article, you can develop it here until it's ready to go live. If you're working on improvements to an existing article, copy only one section at a time of the article to this sandbox to work on, and be sure to use an edit summary linking to the article you copied from. Do not copy over the entire article. You can find additional instructions here. Remember to save your work regularly using the "Publish page" button. (It just means 'save'; it will still be in the sandbox.) You can add bold formatting to your additions to differentiate them from existing content. |
Article Draft
Lead
Boiling-point elevation is the event in which the boiling point of a liquid (a solvent) increases when a non-volatile solute. This results in a pure solvent having a lower temperature than its solution. The boiling point can be measured accurately using an ebullioscope.
*Broke up the lead sentence as it was too long
Article body
- The boiling point elevation is a colligative property, which means that it is dependent on the number of dissolved particles, but not their identity.[1] **When integrated in the original text, will be 5**. It occurs when a solute dilutes the solvent. This phenomenon happens for all solutes in solutions, including ideal solutions, and is independent of specific solute–solvent interactions. Boiling point elevation occurs when a solution is both an electrolyte, like salts, and a nonelectrolyte which is explained by the Van't Hoff Factor. Due to this factor, the boiling point increases as electrolytes dissociate and contribute more particles while nonelectrolytes don't dissociate but increases solute concentration. In thermodynamic terms, boiling point elevation has an entropic origin and can be explained in terms of the vapor pressure or chemical potential. The vapor pressure affects the solute shown by Raoult's Law while the free energy change and chemical potential shown by Gibbs free energy. Most solutes remain in the liquid phase and do not enter the gas phase, except at very high temperatures.
In terms of vapor pressure, a liquid boils when its vapor pressure equals the surrounding pressure. A nonvolatile solute reduces the solvent’s vapor pressure, meaning a higher temperature is needed for the vapor pressure to reach the surrounding pressure, causing the boiling point to elevate.
In terms of chemical potential, at the boiling point, the liquid and gas phases have the same chemical potential. Adding a nonvolatile solute lowers the solvent’s chemical potential in the liquid phase, but the gas phase remains unaffected. This shifts the equilibrium between phases to a higher temperature, elevating the boiling point.[1] **Original text [1] Citation**
Freezing-point depression is analogous to boiling point elevation, though the magnitude of freezing-point depression is larger for the same solvent and solute concentration. These phenomena extend the liquid range of a solvent in the presence of a solute.
*Made changes with wording and changing some passive sentences to their active form to give a more concise text. (Major wording changes are in bold)
*Added relationship to Van't Hoff Factor and Raoult's Law
- will be changing title "The equation for calculations at dilute concentration" to "Equations for calculating Boiling Point Elevation"
- will be changing the image/diagram from LibreTexts Chemistry
- will be changing the equation from LibreTexts Chemistry
- at "Uses", Together with the formula above, the boiling-point elevation can in principle be used to measure the degree of dissociation or the molar mass of the solute. This kind of measurement is called ebullioscopy (Latin-Greek "boiling-viewing"). However, avoiding superheating would be challenging. Therefore, ΔTb would be hard to measure precisely even though superheating was partly overcome by the invention of the Beckmann thermometer. Since the freezing point is often easier to measure with precision, cryoscopy is used more often.
- Added a few changes based on peer review
References
- LibreTexts Chemistry. https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Introductory_Chemistry_(CK-12)/16%3A_Solutions/16.14%3A_Boiling_Point_Elevation (accessed 2024-11-01)
- Akhter, M., Alam, M.M. (2023). Colligative Properties. In: Physical Pharmacy and Instrumental Methods of Analysis. Springer, Cham. https://doi.org/10.1007/978-3-031-36777-9_3
- ^ Akhter, Mymoona; Alam, M. Mumtaz (2023), Akhter, Mymoona; Alam, M. Mumtaz (eds.), "Colligative Properties", Physical Pharmacy and Instrumental Methods of Analysis, Cham: Springer Nature Switzerland, pp. 21–44, doi:10.1007/978-3-031-36777-9_3, ISBN 978-3-031-36777-9, retrieved 2024-11-03