Term
| What is the Brownian motion? |
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Definition
| the erratic, random movement of colloid particles that results from collisions of particles of the dispersion medium with the dispersed particles |
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Term
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Definition
| a mixture containing particles that don't settle out |
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Term
| What does it mean if something is immiscible? |
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Definition
| two liquids can be mixed together but will separate shortly after |
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Term
| What does it mean if something is insouble? |
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Definition
| the substance doesn't dissolve in a solvent |
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Term
| What does it mean if something is miscible? |
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Definition
| two liquids that are soluble in each other in any proportion |
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Term
| What does it mean is something is soluble? |
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Definition
| substance can dissolve in a solvent |
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Term
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Definition
| a mixture containing particles that settle out if left undisturbed |
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Term
| What is the Tyndall effect? |
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Definition
| Dispersed colloid particles scatter light while partilces in a true solution let light shine through |
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Term
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Definition
| a measure of how much soute is dissolved in a specific amount of solvent or solution |
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Term
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Definition
| the ratio of the number of moles of solute dissoved in 1 kg of solvent |
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Term
| What is the formula for molality? |
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Definition
| m=moles of solute/kg of solvent |
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Term
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Definition
| the number of moles of solute dissolved per liter of solution |
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Term
| What is the formula for molarity? |
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Definition
| M=moles of solute/liters of solution |
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Term
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Definition
| the ratio of the number of moles of solute or solvent in a solution to the total number of moles of solute and solvent |
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Term
| What is the formula for a mole fraction? |
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Definition
For a Solute: Xa= na/(na+nb)
For a solvent: Xb= nb/ (na+nb) |
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Term
| What is the heat of solution? |
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Definition
| the overall energy change that occurs during the solution formation process |
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Term
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Definition
| At a given temperature, the solubility of a gas in a liquid is directly proportional to the pressure of the gas above the liquid |
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Term
| What is a saturated solution? |
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Definition
| contains the maximum amount of dissolved solute for a given amount of solvent at a specific temperature and pressure |
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Term
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Definition
| the process of surrounding solute particles with particles to form a solution |
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Term
| What is a supersatureated solution? |
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Definition
| contains more dissolved solute than a saturated solution at the same temperature |
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Term
| What is an unsaturated solution? |
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Definition
| contains less dissolved solute for a given temperature and pressure than a saturated solution |
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Term
| What is boiling point elevation? |
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Definition
| adding a solute to a solvent will raise its boiling point. the temperature diffence is called boiling point eleveation |
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Term
| What is the colligative property? |
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Definition
| property that depends on the number of solute particles in a solution |
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Term
| What is freezing point depression? |
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Definition
| adding a solute to a solvent lowers the freezing point of the solution |
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Term
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Definition
| diffusion of a solvent through a semipermeable membrane |
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Term
| What is osmotic pressure? |
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Definition
the amount of additional pressure caused by the water molecules that moved into the concentrated solution
Depends on the number of solute particles in the solution |
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Term
| Waht s vapor pressure lowering? |
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Definition
| When a solute is added to a solvent and the vapor pressure is lowered |
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Term
| What is the formula for percent by mass? |
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Definition
| Percent by mass= (mass of solute/mass of solution) x 100 |
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Term
| What is the formula for percent by volume? |
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Definition
| Percent by volume = (volume of solute/ volume of solution) x 100 |
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Term
| What is the formula for Henry's Law? |
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Definition
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Term
| What are the factors that affect solvation? |
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Definition
| Agitation, Surface area, and temperature |
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Term
| How does agitation help with solvation? |
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Definition
| stirring or shaking moves solute particles away from each other allowing collisions between solute and solvent particles |
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Term
| How does surface area help with solvation? |
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Definition
| breaking apart solute particles allows for more surface area in shich more collisions can occur |
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Term
| HOw does temperature help with solvation? |
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Definition
| as temperature increases, solvation increases |
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Term
| What do you do if you are finding the freezing point depression or boiling point elevation of a convalent bond? |
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Definition
| Don't multiple the moles of the solute, because the moles don't break apart when you find molality |
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Term
| What do you do if you are finding the freezing point depression or boiling point elevation of an ionic bond? |
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Definition
| Multiply the number of moles by the number of ions in the bond when you find molality |
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Term
| What is a thixotropic mixture? |
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Definition
| suspension that separates into a solid like mixture on the bottom and water on teh top and flows like a liquid |
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Term
| What is a heterogeneous mixture? |
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Definition
| mixture that doesn't blend smoothly throughout and the individual substances remain distinct |
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Term
| What is a homogeneous mixture? |
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Definition
| one that has a uniform composition and in which the individual substances don't remain the same |
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Term
| What is the most common sovent? |
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Definition
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Term
| What Law only works if the solution is a gas dissolved in a liquid? |
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Definition
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