1 / 10

Solutions

This comprehensive overview delves into solutions, highlighting their characteristics and formation. A solution is defined as a homogenous mixture formed when a solute is dissolved in a solvent, making individual particles undetectable. Key factors such as temperature, agitation, and surface area significantly affect the rate of dissolving and solubility. The text also covers concepts like colligative properties, including vapor pressure lowering, boiling point elevation, and freezing point depression, which illustrate how solutions behave differently from pure solvents.

jarrod-eaton
Télécharger la présentation

Solutions

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Solutions • Solution – homogenous mixture so evenly mixed that individual particles can not be seen • Solution – made of solute and solvent • Solvent – dissolves a substance • Solute – substance that is dissolved

  2. Solutions – how they form • solution formed when solvent dissolves solute • rate of dissolving affected by surface area of solute, temp. of solvent, stirring (agitation) of solution • agitation will only affect rate of dissolving, not overall amount of solute dissolved

  3. Solubility • based on KTOM(idea that all matter is moving) • dissolving is constantly occurring & reversing simultaneously • when this point is reached, have saturated solution • holds all solute it can at that temp.

  4. Solubility continued • solubility is amt. of solute dissolving in a given amt of solvent at certain temp. to create sat. solution • unsaturated solution holds less solute than CAN at that temp.

  5. Factors affecting Solubility • solubility of solid usually rises as temp. of solvent rises • gases dissolve better in cold liquids, why? (hint: KTOM) • gas solubility increases as the partial pressure of gas above liquid solvent increases (think COKE!)

  6. Factors affecting solubility - 2 • miscible – applies to liquids, will dissolve in each other • Henry's Law (for given temp.) __S1__ = __S2__ P1 P2

  7. Concentrations • measure of amt of solute/given amt of solvent • dilute (low conc. of solute) and concentrated (high conc. of solute) are qualitative descriptions • Molarityis # of moles solute /Liter sol'n (also known as molar concentration) • Dilution reduces moles solute/unit volume but total moles of solute in sol'n doesn't change, so M1V1 = M2V2

  8. Colligative properties vapor-pressure lowering • VP is Pressure exerted by vapor above a liquid • the decrease in VP is proportional to the number of particles in the solution • EX: (NaCl makes many particles, lowers VP more than glucose, which makes less)

  9. Colligative properties • boiling point elevation • BP is temp where Vapor Pressure of liquid = atmospheric Pressure • When the VP decrease, Boiling Point increases • need more KE to raise VP to atmospheric Pressure due to greater attraction btw particles • BP of solution > BP of pure solvent (so salt doesn’t make water boil faster!)

  10. Colligative properties • freezing point depression • FP lowered due to formation of "shells of solvation", groupings of particles that are attracted to one another • freezing these "shells" requires removal of more KE than freezing pure solvent, lowering FP • size of depression is proportional to # of solute particles dissolved in solvent

More Related