Shared Flashcard Set

Details

Ch 16 & 17
H20, Solution, Dilution, Solvation, Molarity, Molality, Mole fraction, Solution Stoich., and Colligative Properties
43
Chemistry
10th Grade
04/02/2012

Additional Chemistry Flashcards

 


 

Cards

Term
2 ways of expressing the ratio of solute particles to solvent particles
Definition
molality & mole fraction
Term
Molality
Definition
moles of solute mol
--------------- = ----- = m
kg of solvent kg

the number of moles of solute per kg of solvent
Term
What is the main difference between molarity and molality?
Definition
One is the ratio of moles to volume of the solution and the other is the ratio of moles to the mass
Term
mole fraction
Definition
moles of solute
----------------
moles of solution

the ratio of number of moles of the solute per moles of the ENTIRE solution
Term
Increased molarity
Definition
= Increased concentration
(direct relationship)
Term
Molarity
Definition
moles of solute mol
---------------- = ------ = M
L of solution L

quantitative measure (number) relating moles of solute to solvent
Term
Dilutions
Definition
when you make ________, the number of moles of solute does not change

M1(V1) = M2(V2)
Term
In the formula:
M1(V1) = M2(V2)
what do M and V represent?
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
Term
IMF of H20?
Definition
Hydrogen bonds
Term
Properties of H20?
Definition
High surface tension, low vapor pressure, and high boiling point
Term
How much heat energy does it take to raise the temp of 1 g of H20? & Why is it so high?
Definition
4.18 J
because H20= hydrogen bonds (remember IMFs: they're the 2nd strongest)
Term
Density of ice versus liquid H20
Definition
Density increases because its mass stays constant (conservation of mass) Ice = MORE DENSE than liquid water
(*Note: this is ABNORMAL)
Term
Solvent
Definition
the dissolving medium in a solution
Term
solute
Definition
the dissolved particles (in a solution)
Term
What determines if a solute will dissolve in water?
Definition
Solubility & polar solvents dissolve ionic & polar compounds ("like dissolves like")
Term
electrolyte
Definition
compounds that conduct an electric current in aqueous solution or the molten state
Term
nonelectrolytes
Definition
compounds that do not ocnduct an electric current in either aqueous solution or the molten state
Term
Polar covalent or ionic =
Definition
soluble
Term
Nonpolar covalent
Definition
insoluble
Term
Cohesion
Definition
Alike molecules that stick together (ex: water molecule + water molecule = water droplet)
Term
Adhesion
Definition
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)
Term
Capillary action
Definition
the tendency to move up a narrow tube AGAINST gravity
(ex: water climbs up through trees)
Term
Solvation is also known as
Definition
dissolving
Term
Considering "like dissolves like"

Solvent:
polar
ionic
nonpolar
Definition
Solute:
polar, ionic
polar, ionic
nonpolar
Term
Dissociate
Definition
when a solute splits to dissolve (ionics only!!)
Term
Aqueous species
Definition
the dissociated elements
Term
Polar molecules (covalents) dissolve but...
Definition
they don't dissociate
Term
Saturated
Definition
When a given amount of solvents at a given temperature is holding the max amount of solute
Term
Unsaturated
Definition
When a given amount of solvents at a given temperature is holding less than the max amount of solute
Term
Supersaturated
Definition
When a given amount of solvents at a given temperature is holding more than the max amount of solute
(Note: UNSTABLE)
Term
When referring to a heating curve:

on a line =
Definition
saturated
Term
When referring to a heating curve:

below a line =
Definition
unsaturated
Term
When referring to a heating curve:

above a line =
Definition
supersaturated
Term
You require 5mL of 1.0M KOH, but you have 1L of 0.5M KOH. Can you make it work with dilution?
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)
Term
Why do you not need to round for sig. fig.s for dilution equations?
Definition
in dilution equations, ACCURACY is extremely important
Term
Colligative Properties
Definition
Any property of a solvent that changes by the addition of a solute
Term
Add solute to a solvent with vapor pressure
Definition
the vapor pressure will decrease (less of the solvent will evaporate)
Term
When is a solution boiling?
Definition
When vapor pressure = atmospheric pressure
Term
When you add a solute to a solvent, the boiling point...
Definition
increases (boiling point elevation)
Term
When you add a solute to a solvent the vapor pressure...
Definition
decreases because you must add more energy to equal atm (atmospheric pressure)
Term
when you add a solute to a solvent the freezing point...
Definition
decreases (freezing point depression)
Term
The formula for calculating Boiling Point Elevation:
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)
Term
The formula for calculating Freezing Point Depression
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)
Supporting users have an ad free experience!