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| What determines whether a substance will "dissolve"? | The "compositions of the solvent and the solute" determine whether a substance will "dissolve". |
| What determines how "fast" a substnace will "dissolve"? | "Stirring (agitation), temperature, and the surface area of the dissolving particles" determine how "fast" a substance will "dissolve". |
| Define: Saturated Solution | A "saturated solution" is a solution that "holds the maximum amount of solute" under the given conditions; therefore, no more "solute" can be dissolved into the "solvent" - given that the "temperature and pressure" remain "constant". |
| Define: Solvent | A "solvent" is the substance that "dissolves" the "solute" whe making a solution (For example, |
| Define: Solute | A "solute" is a substance that is being "dissolved" in the "solvent" when making a solution (for example: With sugar and water, then "solute" would be the sugar.) |
| Define: Supersaturated Solution | A "supersaturated solution" is a solution containing more "solute" than the maximum allowed to "dissolve" in the "solvent"; therefore, the "soluton" they is "unstable". |
| Define: Solubility | "Solubility" means how readily (good) a "solute" "dissolves" in a "solute" - also, it is the amount of the "solute" that "dissolves" in a given amount of "solvent" at specified temperature and pressure to produce a saturated solution. |
| Define: Agitation | "Agitation" means to "stir" or "shake". |
| Define: Insoluble | An "insoluble" solute is a solute incapible of "dissolving". |
| Where does the "dissolving" of a "solute" take place? | The "dissolving" of a solute takes place on the "surface" of the solute as the molecules of the "solvent" pass over the surface of the solute. |
| Define: Kenetic Energy | "Kenetic energy" is work in motion - for example, when the heat, or temperature, is raised the molecules of the solvent build up "kenetic energy" and press harder againist the surface molecules of the "solute" - causing a "solute" to "dissolve faster" in the "solvent". |
| Does raising the "temperature" cause more of the "solute" in a solution to "dissolve" in the "solvent"? | No, it does not increase the amount of the "solute" that "dissolves" in the "solvent" it only decreases the amount of time that a given amount of "solute" will "dissolve" in a given amount of "solvent - it makes the process more "faster". |
| What "dissolves" faster, a molecule of a given "solute" that is larger or smaller? | The smaller one will "dissolve" faster because more of it surface are is exposed to the colliding molecules of the "solvent"; while the large molecules, because of its greater size will not expose as much "surface area"; therefore, dissolving more "slowly" in the "solvent". |
| Define: Solvation | "Solvation" is the "dissolving" of the "solute". |
| Define: Crystallization | "Crystallization" means that the "excess solute" will form a solid, 3 dimensional, form and settle down in the "solvent". |
| Why does "crystallization" take place? | "Crystallization" takes place in a solution because no more "solute" can "dissolve" in the "solvent" (the solution has reached its "saturated" level) and the remaining "solute" then turn into solid "crystals" when "disturbed". |
| What is the "dynamic equilibrium" in a solution? | The "dynamic equilibrium" is reached in a solution at the point where no more "solute" can be "dissolved" in the "solvent" (the solution has reached its "saturated level") |
| Does the "mass" of a solution with a "solute" and a "solvent" "lose mass" as it "crystallizes"? | No, the solu0on does "NOT" "lose mass" as it crystallizes because mass is never lost only takes on new forms (such as in the crystals). |
| How is "solubility" often expressed? | "Solubility" is often expressed in "grams of solute per 100 grams of solvent". |
| How is "solubility" ofen express for a "gas"? | Sometime the "solubility" of a "gas" is expressed in "grams per liter of solution". |
| Define: Unsaturated Solution | An "unsaturated solution" is a solution that contains "less solute" than a "saturated solution" at "a given temperature and pressure". |
| What does it mean that "substances are 'infinitely soluble' to each other"? | When "substances" are "infinitely soluble" with each other it means that they will dissolve any amount of each other until they reach the "saturation point" with had trouble for example, water and ethanol are "infinitely soluble". |
| Define: Miscible | "Miscible" describes "liquids" that "dissolve" in "one another" in all proportions. |
| When substances are "miscible" which one becomes the "liquid or solvent"? | When two substances are "miscible" the substance that is considered the "liquid or solvent" is the one in the "greater amount". |
| Define: Partially Miscible | A solution that is "partially miscible" is one that has substances that "are slightly soluble in each other" - for example, water and diethyl ehter. |
| Define: Immiscible | "Immiscible" means that their are liquids present that are "insoluble (can "dissolve into each other") and one another". |
| What do "oil" and "vinegar" have in common when mixed into a solution? | Both "vinegar and oil" are "immiscible" when mixed into a solution. |
| What is the "base of vinegar"? | "Vinegar" is "water-based". |
| What specifically does "temperature" affect as far as the "solubility" of a solution? | "Temperature" affects the "solubility of solid, liquid, and gaseous "solutes" in a "solvent". |
| How does "pressure" affect the solubility of gaseous solutes? | Both "pressure" as well as "temperature" affect the "solubility" of a "gaseous" substance in the "same manner." |
| Define: Precipitate | A "precipitate" is a solid that forms and settles out of a liquid mixture. |
| Why does a "precipitate" form in some chemical reactions? | A "precipate" forms in some chemical reactions because as the solution "cools in air" it "CAN NOT" "contain the same concentration of solution (example: minerals) as it did at a higher temperature - "so some of the solution (example: minerals) precipitate. |
| Define: Concentration | The measurement of the amount of "solute" that is "dissolved" in "a given quantity of solvent". |
| Define: Dilute Solution | A "dilute solution" is a solution that contians a small amount of "solute" and mostly contains a "solvent". |
| Define: Concentrated Solution" | A "concentrated solution" is a solution that contains a large amount of "solute" and less "solvent". |
| Define: Molarity (M) | "Molarity (whose symbol is "M")" is the "concentration of solute in a solution expressed a the 'number of moles' of 'solute' dissolved in '1 liter' of solution". |
| What is the formula to calculte the "molarity" of a solution? | The formular for calculatin the "molarity of a solution" is the following: Molarity (M) = moles of solute/liters of solution |
| What is another name for "molarity"? | Another name for "molarity" is "molar concentration". |
| What happens to the "total number of moles of a solute in a solution" when a solution is "dilluted"? | When a "solution is dilluted" the "total number of moles of a solute in a solution "does NOT change". |
| What happens when a "solution is dilluted"? | When "a solution is dilluted" it "reduces the number of moles of 'solute per unit volume". |
| In what kind of "temperatures" are "solids" more "soluable"? | "Solids" are more "soluble" in "warmer temperatures". |
| In what kind of "temperatures" are "gases" more "soluable"? | "Solids" are more "soluble" in "colder temperatures". |
| Define: Thermal Pollution | "Thermal Poluution" is when "heated water" is dumped into a body of water (such as a lake) causing the temperature entire body of water to increase and in the process killing the aquatic (water) plants and animals in the body of water. |
| Why does "thermal pollution" cause harm to aquatic (water) plants and animals in a body of water? | When the "water temperature increases" it causes the concentration of the dissolved oxygen in the body of water to lower; therefore, depriving the aquatic plant and animal life to be deprived of the needed oxygen and resulting in their death. |
| What is the "MOST soluable" substance "in water" at "various temperatures"? | The "MOST soluble substance" in "water at various temperatures" is "Barium Hydroxide". |
| What is the " LEAST soluable" substance "in water" at "various temperatures"? | The "LEAST soluble substance" in "water at various temperatures" is "Carbon dioxide". |
| When a solution becomes "supersaturated" what can be "used to disturb it" so that "cystallization" occurs? | When a solution becomes "supersaturated" a "seed cystal" can be "used to disturb it" so that "cystallization" occurs? |
| Define: Seed Crystal | A "seed crystal" is used "to disturb" a "supersturated solution" so that "cystalization" takes place. |
| Define: Disturb | To "disturb" means attempting to rearrange the particles in a solution - when this is done in a "supersaturated solution" then the solution will begin to crystalize". |
