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52 Cards in this Set
- Front
- Back
viscosity
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friction or resistance liquids have when moving past each other
the stronger the attraction between the molecules the more resistance there is so the more viscous it is ex. syrup=higher water=lower |
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surface tension
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molecules (liquids) have spread out attractions in every direction so liquids act as a film
like how a pin floats on water |
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capillary action
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liquids attracted to solids will move around on the solid
like liquid going up a straw liquids tend to be pulled upwards like chromatography paper |
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phase equilibrium
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when 2 phases balance each other out
ex. eventually the water evaporating and the water condensing will reach an equilibrium and balance each other out |
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dynamic equilibrium
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when opposing changes (water evaporating and water condensing) occur at equal rates
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le chatlier principle
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when a system at equilibrium is stressed it will react to minimize the stress and reach a new equilibrium
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boiling points
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when the vapor pressure increases as the temp increases it will reach a boiling point where liquid will convert to gas
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critical temp.
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the temperature above where a phase can no longer exist regardless of pressure
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critical pressure
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the minimum pressure needed to change phases at the critical temperature
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solids
include 3 types of crystalline structures |
most ordered system
crystalline solids- like brick wall amorphous solids- random structure polycristalline solids- many crystallines put together |
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sublimation
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solid--> gas
happens with a very high vapor pressure |
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melting point
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solid-->liquid
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heat of fusion
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heat needed to change phases
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triple point
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point on a phase diagram where all three lines meet- where all three phases can exist
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distillation
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process of purifying water
removes any substance with a boiling point higher than water by evaporating all the water, letting it condense, then collecting the condensation separates matter by boiling points |
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aeration
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purifies water as well
water is sprayed into the air and anything that's not water falls out |
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hard water
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water with stuff in it like Ca and Cl2
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composition of water
talk about helpful ratios and stuff |
H2 and O2 combine to form water in a 1mass:8mass ratio by MASS
so 1 g of H2 and 8 g of O2 makes 9 g of H2O gaseous H2O exists in VOLUME in 2volume:1volume ratios (H2:O2) |
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heavy water
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water with an isotope of Hydrogen
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Molar heat of fusion
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amount of heat energy required to melt one mole of solid at its melting point
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molar heat of vaporization
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heat energy needed to vaporize a mole of liquid at its boiling point
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Calorimetry problems
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Quantity of heat needed= m x C
m=mass c=heat of fusion |
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Anhydrides
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oxides that react with water to form two classes of compounds (acids and bases)
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Basic anhydrides
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ex. Na
Na2O + H2O= 2NaOH an element that when it's made an oxide and reacted with water it forms excess OH - ions ALWAYS metal + oxygen like Na2O |
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Acidic anhydrides
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ex. CO2
CO2 + H2O= H2CO3 any element that when its made an oxide and reacted with water it forms excess H+ ions ALWAYS nonmental + oxygen like CO2 |
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saturated
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when substances are dissolved in water to the extent that no more will dissolve at that temperature
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unsaturated
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solution with less solute than a saturated solution under existing conditions
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polar things dissolve in
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polar things
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nonpolar things dissolve in
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nonpolar things
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hydrated ion
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things dissolve when the entire ion/molecule is surrounded by water molecules- the ion and the water molecules are held together by dipole forces- the entire molecule is a hydrated ion
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miscible
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when two liquids mix and dissolve in each other
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immiscible
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when 2 liquids don't mix
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colloid
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substances microscopically dispersed evenly throughout another colloid
mixtures whose particles are larger than the size of a molecule but smaller than particles that can be seen with the eye ex. milk, butter, plaster particles are microscopically visible |
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suspensions
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heterogenous fluid with solid particles big enough for sedimentation
particles are visible |
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solutions
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homogenous mixtures where a solute is dissolved in a solvent
particles are NOT visible HAS MORE SOLVENT and less SOLUTE |
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dilute
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small amount of solute is dispersed in the solvent
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concentrated
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large amount of solute is dissolved in the solvent
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supersaturated
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when a solution is cooled enough the solute can't come out of the solvent- then the solution can be packed with more solute than usual because it's cooled
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Water's heat of vaporization
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40.79 kj/mol
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water's heat of fusion
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6.01 kj/mol
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%concentration
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grams of solute/grams of solution x 100
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Molarity (M)
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# moles of solute / 1L of solution
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Molality (m)
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# moles of solute / 1000 g of solvent
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mole fraction
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# moles of solute / moles solute + moles of everything else
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DILUTION PROBLEMS EQUATION
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M1V1=M2V2
M= Molarity V= Volume in L IMPORTANT: when the question asks how much water needs to be ADDED make sure you solve for final volume and subtract that from the initial volume!!!! |
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colligative properties of solutions
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properties that depend on the concentration of particles not the type of particle
ex. freezing and boiling points |
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calculating freezing and boiling points
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how to calculate the degree increase or decrease of a substance's boiling or freezing point
- find MOLALITY of solution - use MOLALITY to find the number of moles of solute in the solution BELOW ARE CHANGES BASED ON 1 MOL PER 1000 GRAMS 1) count number of particles (ions its made of up) ex. NaCl=2 Cu(NO3)2=3 2) for boiling point- multiply by 0.51 3) for freezing point- multiply by -1.86 this gives you the change in boiling or freezing points |
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Hydrate
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substance that holds a definite proportion of water in its crystal structure
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efflorescent
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hydrated crystals that lose water of hydration when exposed to air at ordinary temperatures
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deliquescent/hydroscopic
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hydrates that absorb water from the air and become wet
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water specific heat
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C= 4.18 J/g
C= 1 cal |
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what happens to the boiling point/freezing point when you add a solute?
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raises boiling points and lowers freezing points
saltwater boils at higher temperature than pure water |