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| 2 ways of expressing the ratio of solute particles to solvent particles |
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Definition
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Term
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Definition
moles of solute mol
--------------- = ----- = m
kg of solvent kg
the number of moles of solute per kg of solvent |
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Term
| What is the main difference between molarity and molality? |
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Definition
| One is the ratio of moles to volume of the solution and the other is the ratio of moles to the mass |
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Definition
moles of solute
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moles of solution
the ratio of number of moles of the solute per moles of the ENTIRE solution |
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Definition
= Increased concentration
(direct relationship) |
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Definition
moles of solute mol
---------------- = ------ = M
L of solution L
quantitative measure (number) relating moles of solute to solvent |
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Definition
when you make ________, the number of moles of solute does not change
M1(V1) = M2(V2) |
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Term
In the formula:
M1(V1) = M2(V2)
what do M and V represent? |
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Definition
M1= Molarity of stock (More concentrated solution)
V1= amount of stock solution to take
M2= more dilute concentration
V2= final volume of dilute solution |
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Definition
| High surface tension, low vapor pressure, and high boiling point |
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Term
| How much heat energy does it take to raise the temp of 1 g of H20? & Why is it so high? |
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Definition
4.18 J
because H20= hydrogen bonds (remember IMFs: they're the 2nd strongest) |
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Term
| Density of ice versus liquid H20 |
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Definition
Density increases because its mass stays constant (conservation of mass) Ice = MORE DENSE than liquid water
(*Note: this is ABNORMAL) |
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Term
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Definition
| the dissolving medium in a solution |
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Term
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Definition
| the dissolved particles (in a solution) |
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Term
| What determines if a solute will dissolve in water? |
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Definition
| Solubility & polar solvents dissolve ionic & polar compounds ("like dissolves like") |
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Term
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Definition
| compounds that conduct an electric current in aqueous solution or the molten state |
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Term
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Definition
| compounds that do not ocnduct an electric current in either aqueous solution or the molten state |
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Term
| Polar covalent or ionic = |
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Definition
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| Alike molecules that stick together (ex: water molecule + water molecule = water droplet) |
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The joining of 2 different substances due to attractive forces that hold them
(ex: keeps the water drops on the surfaces of leaves & flowers in place) |
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Definition
the tendency to move up a narrow tube AGAINST gravity
(ex: water climbs up through trees) |
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Term
| Solvation is also known as |
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Definition
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Term
Considering "like dissolves like"
Solvent:
polar
ionic
nonpolar |
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Definition
Solute:
polar, ionic
polar, ionic
nonpolar |
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Term
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Definition
| when a solute splits to dissolve (ionics only!!) |
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Term
| Polar molecules (covalents) dissolve but... |
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Definition
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Term
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Definition
| When a given amount of solvents at a given temperature is holding the max amount of solute |
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Term
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Definition
| When a given amount of solvents at a given temperature is holding less than the max amount of solute |
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Term
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Definition
When a given amount of solvents at a given temperature is holding more than the max amount of solute
(Note: UNSTABLE) |
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Term
When referring to a heating curve:
on a line = |
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Definition
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Term
When referring to a heating curve:
below a line = |
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Definition
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Term
When referring to a heating curve:
above a line = |
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Definition
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Term
| You require 5mL of 1.0M KOH, but you have 1L of 0.5M KOH. Can you make it work with dilution? |
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Definition
| No because it needs to be more concentrated than what you currently have, so diluting it would be pointless because it wouldn't be the final product that you want. (Basically, you can't make a solution MORE concentrated w/ a dilution) |
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Term
| Why do you not need to round for sig. fig.s for dilution equations? |
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Definition
| in dilution equations, ACCURACY is extremely important |
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Term
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Definition
| Any property of a solvent that changes by the addition of a solute |
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Term
| Add solute to a solvent with vapor pressure |
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Definition
| the vapor pressure will decrease (less of the solvent will evaporate) |
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Term
| When is a solution boiling? |
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Definition
| When vapor pressure = atmospheric pressure |
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Term
| When you add a solute to a solvent, the boiling point... |
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Definition
| increases (boiling point elevation) |
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Term
| When you add a solute to a solvent the vapor pressure... |
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Definition
| decreases because you must add more energy to equal atm (atmospheric pressure) |
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Term
| when you add a solute to a solvent the freezing point... |
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Definition
| decreases (freezing point depression) |
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Term
| The formula for calculating Boiling Point Elevation: |
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Definition
(delta)Tb=Kb(m)(i)
In english:
(delta)Tb= change in boiling temp
Kb= boiling point constant
m= molality
i= number of particles solute breaks into
(for ionics, i= number of ions
for molecules, i= 1) |
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Term
| The formula for calculating Freezing Point Depression |
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Definition
(delta)Tf=Kf(m)(i)
In english:
(delta)Tb= change in freezing temp
Kb= freezing point constant
m= molality
i= number of particles solute breaks into
(for ionics, i= number of ions
for molecules, i= 1) |
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