Chemistry Chapter 12 Test Questions – Flashcards
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| Heterogeneous Mixture: |
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| compositon not uniform |
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| Homogeneous Mixture |
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| composition uniform throughout |
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| Soluble: |
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| ability of being dissolved |
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| Solution |
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| homogeneous mixture of two or more substances |
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| Solvent |
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| Dissolving medium in a solution(thing its dissolved in) |
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| Solute |
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| substance dissolved in solution(Dissolv-ie) |
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| When a solution is passed through filter paper with the individual components seperate? |
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| no, usual not b/c uniformed throughout |
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| Solutions can happen in gasses, liquids, and solids? T or F |
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| True |
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| Alloys: |
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| solid solutions in which atoms of two or more metals are uniformly mixed |
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Does changing the proportions of each metal in the alloy create wanted properties? Take gold, if mixed with copper and silver will it be stronger? |
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yes yes |
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| Suspension |
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| particles in solvent so large they settle unless mixture is constantly stirred |
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| Colloids |
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| mixture formed by particles that are perfectly sized(not to big or small) |
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| Do colloidal particles seperate when filtered? |
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| no, b/c small enough |
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| Dispersed phase: |
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| colloidal particles |
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| Dispersing medium: |
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| water |
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| Sol |
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Solid Dispered in liquid
paints, mud |
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| Gel |
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solid network extending throughout liquid
gelatin |
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| Liquid Emulsion |
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liquid dispered in a liquid
milk, mayo |
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| Foam |
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gas dispered in liquid
shaving cream, mousse |
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| Solid Aerosol |
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solid dispered in gas
smoke, auto exhaust |
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| Liquid Aerosol |
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liquid dispered in gas
fog, mist, clouds |
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| Solid Emulsion |
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liquid dispered in solid
cheese, butter |
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| Properties of solutions: |
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| Colloid properties: |
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|
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| Suspension properties: |
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; |
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| Tyndall Effect |
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| when light is scattered by colloidal particles dispersed in a transparent medium |
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| Brownian Motion |
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| when particles are seen moving when light is shone upon them at a right angle |
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| What happens to the negative and positive ions when an ionic compound is dissolved? |
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| seperate from eachother and get surrounded by water molecules |
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| Describe the process in which an ionic compund enables a solution to conduct electric current. |
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| When dissolves, compounds positive and negative ions seperate causing them to be surrounded by the H2O molecules. These ions are then free to move, enabling electric current to pass through |
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| Electrolyte |
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| substance that dissolves in water to give a solution that conducts electric current |
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| Can certain high polar molecular compunds be electrolytes? |
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| yes. look at HCl |
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| A substance that dissolves in water to give a solution that doesnt conduct electric current is called a(n): |
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| nonelectrolyte |
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An apparatus glows brightly. The solution is: a)semiconductor b)electrolyte c)non electrolyte |
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| b |
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| Ways that affect the rate of dissolution are: |
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| Is there a limited amount of a solid solute to solvent combination at a given T that can dissolve? |
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| yes |
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| solution equillibrium: |
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| physical stare in which the opposing processes of dissolution and crystalization of a solute occur at = rates |
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| A solution that contains the max. amnt of dissolved solute is: |
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| saturated solution |
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| A solution that contains less solute than a saturated solution under the exsisting conditions is a(n): |
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| unsaturated solution |
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| Supersaturated solution is when: |
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| a solution contains more dissolved solute than a saturated solution contains under same conditions. So if substance is heated so everythng is dissolved, is then coolde, naturally it will seperate, however w/o disturbance it wont seperate |
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| solubility of substance: |
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| amnt of that substance required to form a saturated solution w/ specific amnt of solvent at a specified temp |
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| "Like dissolves like" means: |
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similar substances, such as types of bonding, polarity, etc. are capable of dissolving on another. Rouch general rule. not true for sure! |
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| Why doesthe polarity of the water molecules play such and important role in formation of solutions w. ionic compounds? |
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| b/c the slightly charges particles of water attract ions from ionic compund, therefore causing them to seperate from the crystal(aka dissolving) |
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| Hydration: |
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| is the solution process w/ water as the solvent |
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| What is ment when you say "the ions are hydrated" ? |
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| means that the hyrdated h20 ions are drwing ionic compounds ions away from crystal resultion in dissolution |
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| What are hydrates? |
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| crystalline compunds that incorperate water molecules and maintain same ratios throughout |
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| Whats an immiscible liquid? |
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Liquids that are not soluble in eachother. ; look at some PB and salad dressings. Its the seperation! |
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nonpolar substances with nonpolar liquids are: a) soluble b)insoluble c)mixed but unevenly; not uniform |
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| a. NP have london Disperssion forces =; relativly weak =; molecules from both substances free to intermingle and mix |
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| Liquids that dissolve freely in one another in any proportion are _______. |
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| miscible |
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Pressure effects solubility very little for: a)Solids b)Liquids c)Gasses d) Solids ; Liquids e) Liquids and Gasses |
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| d |
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| Explain process in which P effects solubility. |
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| By ^P it puts stress on the equillibrium, therefore more collisions =; faster rate b/w evaporation and dissolving = equillibrium reached at higher gas solubility |
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| The solubility of a gas in a liquid is directly proportional to the partial P of that gas on the surface of the liquid is____ ____. Which applies to G-L solutions 2 constant T |
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| Henrys Law |
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| That is a perfect example of EFFERVESCENCE in your everyday life? |
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| opening a can of soda. the rapid escape of G from L in which it is dissolved. thats the tssstttt sound when u open a can! this is what causes the 'fizzy-ness' |
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Which is easier to predict? Effects ofSolubility on L and S. or just G? |
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| G |
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| Solvated: |
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| a solute particle that is surrounded by slvent molecules |
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| Enthalpy of solution: |
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| net amnt of E absorbed as heat by the solution when a specific amnt of solute dissolves in solvent |
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If enthalpy of solution is___ then the rxn is ____. a) positive; ____ b) negative; ____ |
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a) exo b) endo |
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| When is E released in enthalpy of solution for gasses? |
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| when a G dissolves in L b/c attraction b/w solute gas and solvent molecules outweighs the E needed to seperate solvent molecules |
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| The ___________ of a solution is a measure of the amnt of solute in a given amnt of solvent or solution |
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| concentration |
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| Molarity is: |
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| the # moles of solute in one L of solution |
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| ________ is the concentration of a solution expressed in moles of solute per kilogram of solvent |
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| Molality |
