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77 Cards in this Set
- Front
- Back
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PPM can be measured in ____ or ____.
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mg/kg
or mg/L |
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concentration:
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the amount of a solute dissolved in a given quantity of solvent
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A concentrated solution contains a _____ amount of solute.
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large
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A dilute solution contains a _____ amount of solute
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small
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solution:
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a homogeneous mixture of 2 or more substances, in which one is called the solvent and the other is the solute.
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solvent:
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main medium, what is there in the largest quantity
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solute:
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dissolved in the solvent
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molarity:
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the number of moles of solute dissolved in 1 L of solution.
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aqueous solutions:
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-water will always be present in excess
-there will be solute species that are either molecules or ions -REMEMBER: polyatomic ions remain intact when a salt dissolves in water |
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dissociation
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separating the ions from ionic compounds
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polarity:
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allows water to attract ions and pull them from their crystal structure in a process known as hydration.
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dilution equation:
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Molarity initial x Vol initial =
Morality final x Vol final |
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soluble:
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generally refers to the inability of a solute to dissolve in a given amount of solvent
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insoluble:
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generally refers to the ability of a solute to dissolve in a given amount of solvent
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electrolyte solutions:
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all contain ions dissolved in water
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non-electrolyte solutions:
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contain whole molecules dissolved in water.
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acids are molecule compounds that ____ when they dissolve in water.
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iodize
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strong acids:
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acids that iodize virtually 100% (strong electrodes)
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weak acids:
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acids that only ionize a small percentage (weak electrodes)
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unsaturated solutions:
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do not contain as much solute as possible at a given temperature
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saturated solution:
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contains the max concentration of solute that can dissolve in it
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supersaturated solution:
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contains more than the quantity of a solute that is predicted to be soluble in a given volume at a given temp
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when a salt dissolved in water, it produces ___ and ____
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cations and anions
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precipitate:
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forms if any new combinations of the ions form a salt that is insoluble in water
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Metathesis Reaction
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also known as precipitation reactions.
AX+BY=AY+BX |
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acid/base reactions
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-also known as "neutralization" reactions
-usually react to form water |
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Arrhenius acid:
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substance that produces H+ ions in aqueous solutions.
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Arrhenius base:
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substances that produce OH- ions in aqueous solutions
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Bronsted Lowry base:
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proton acceptor
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Bronsted Lowry acid:
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proton donor
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monoprotic acid:
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when ionized, it releases one proton per molecule
EX: HCl |
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diprotic acid:
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when ionized, it realeases two protons per molecule
EX: H2SO4 |
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titration:
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adding a base to an acid until it is neutralized, to determine how much acid is present (or vice versa)
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amphiprotic:
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acts as base or acid
EX: water |
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oxidation:
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loss of electrons
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reduction:
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gain of electrons
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pure elemts have an oxidation number of ____
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zero
EX: Na, Cl2 |
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precipitation/double replacement reactions are NOT ____
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oxidized
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Boyle's Law: Volume & Pressure
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inverse relationship: increasing pressure decreases volume
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Charle's Law: Volume and Temperature
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direct relationship: increasing temperature increases volume
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Avogadro's Law: Volume and Amount (moles)
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direct relationship: increasing amount of gas increases volume
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when gases are mixed together, their molecules are ____ of one another.
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independent. all gases in the mixture have the same volume and temperature
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partial pressure:
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the pressure of a single gas in a mixture of gases
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Dalton's Law of Partial Pressures
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the sum of partial pressures of all the gases in the mixture equals the total pressure
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vapor pressure:
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the pressure exerted by a vapor at equilibrium with its liquid
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thermochemical equation:
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inclues heat energy as a reactant or product
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Postulate 1 of Kinetic Molecule Theory: Particle Volume
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gas particles are considered to have mass, but no volume
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Postulate 2 of Kinetic Molecule Theory: Particle Motion
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gas particles are in constant, random, straight-line motion except when they collide w/ each other
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Postulate 3 of Kinetic Molecule Theory: Particle Collisions
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collisions are elastic therefore the total kinetic energy of the particles is constant
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average kinetic energy of the gas molecules depends on the average ___ and ____
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mass and velocity
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gases in the same container have the same temp, thus the same ___________
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average kinetic energy
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if gases have different masses, the only way for them to have the same kinetic energy is to have different ______
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average velocities
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A __ is a device used to measure atmospheric pressure
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barometer
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Pressure (P) = __/__
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Force/Area
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___ is used to measure gas pressure in the laboratory.
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Manometer
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Boyle's Law
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inverserve relationship between VOLUME and PRESSURE.
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Charle's Law
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direct relationship between TEMPERATURE and VOLUME
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Ideal Gas
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hypothetical gas whose pressure, volume, and temp is completely described by the gas law (PV=nRT)
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specific heat capacity is an ____ property.
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intensive (depends on kind not on amount)
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enthalpy is an ____ property.
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extensive (directly related to the amount of the reactant)
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state function
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only the initial and final states are important
EX: energy, temp, pressure, loacation |
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path function
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numerical value cannot be determined unless the entire process is observed
EX: heat and work |
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bond breakage requires energy ___
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input
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bond formation ___ energy
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releases
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firsth law of thermodynamics
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the internal energy of a system is the sum of all the kinetic & poetential energy of that system
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heat (q)
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energy transferred between a system and its surroundings as a result of a difference in their temperatures
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work (w)
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energy transferred when an object is MOVED by a force
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exothermic
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"feels hot"
q is less than 0 heat leaving the system |
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endothermic
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"feels cold"
q is greater than 0 heat entering the system |
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heating curve: horizontal line means ___.
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no change in temperature, just a change in physical state
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heat capactity depends on two things:
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1) amount of substance
2) type of material object is made of |
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bomb calorimeter
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used to measure change in E because it is a constant volume system.
change in E = q system |
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coffee cup calorimetry
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used to mesure change in H because it is a constant pressure system.
change in E= q + w |
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enthalpy (H)
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the internal energy plus the product of the pressure and volume.
mesure of heat flow in/out of system under constant pressure. H = E + PV |
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When change in H is positive, the system has ___ heat from surroundings.
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gained (endothermic)
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When change in H is negative, the system has ___ heat to surroundings.
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lost (exothermic)
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The enthalpy change for a reaction is ___ in magnitude but ___ in sign
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equal in magnitude
opposite in sign |
