Unit 6

Question 1

homogeneous

Answer 1

uniform mixture

Question 2

heterogeneous

Answer 2

non-uniform mixture

Question 3

whats the two types of HOMOgeneous mixtures

Answer 3

solutions and collodis

Question 4

what is a usual characteristic of a solution

Answer 4

solutions are usually transparent

Question 5

whats a observable(visual) characteristic of colloids

Answer 5

cloudy/milky or gel-like

Question 6

what happens when something dissolves

Answer 6

In a solution, the solute breaks up into individual molecules or ions

The solute particles are all less than 2 nm in diameter.

Question 7

what happens to a solution when the particles, what does the solution look like

Answer 7

Because the solute particles are so small, they do not scatter light. Solutions are transparent.

Question 8

colloid

Answer 8

A colloid is a homogeneous mixture with particles that are between 2 nm – 1000 nm in diameter. Because the particle size is comparable to the wavelength of light, colloids scatter light

Question 9

whats to solvent dispersed phase of butter

Answer 9

gel

Question 10

what state is shaving cream considered

Answer 10

foam

gas as dispersed phase, liquid as solvent phase

Question 11

what phase is paint

Answer 11

sol

solid in dispersed and solvent phase

Question 12

perfume is an example of what phase

Answer 12

liquid aresol

Question 13

what type of liquid is transparent

Answer 13

SOLUTIONS ARE TRANSPARENT

Question 14

whats a suspension?

Answer 14

A suspension is a heterogeneous mixture with particles that are larger than 1000 nm in diameter. Suspensions have been thoroughly mixed are temporarily uniform, but because the particle size is so large, it will eventually settle into two phases.

Question 15

whats the difference between heterogeneous mixture, colloid and solution

Answer 15

size

Question 16

solubility

Answer 16

The solubility of a substance is the maximum amount of it that can dissolve in a given amount of solvent.

For example, the solubility of sodium chloride at 25 °C is 359 g/L. That means you could dissolve up to 359 g of NaCl in 1.0 L water at room temperature.

Question 17

saturation

Answer 17

If the maximum amount of a solute is dissolved in a solvent, the resulting solution is called a saturated solution. Anything less than the maximum amount dissolved is called an unsaturated solution. Anything more than the maximum amount dissolved is called a supersaturated solution.

Question 18

describe supersaturation and precipitation

Answer 18

We could dissolve 400 g of sugar in 100 mL of boiling water. When it cools down, it will be supersaturated. Some of the sugar will eventually precipitate out (revert to the solid state).

Question 19

whats the equation for vapor pressure

Answer 19

Vapor Pressure = Pressure of Gas at Equilibrium

whats happening all the time

Question 20

what is the speed of a reaction proportional to

Answer 20

The speed of a simple reaction is directly proportional to the concentration (molarity) of the reactant.

Question 21

whats the equation for the speed of a reaction

Answer 21

k[h20(l)]

Question 22

what does every variable in the speed of a reaction mean

Answer 22

k = a constant (related to temperature)
[H2O(l)] = molarity of liquid water
[something] = molarity of something

Question 23

what happens if you add a solute what happens to the liquid from of water

Answer 23

if we add soluter, you descrease the liquid form of what and would in turn

that would slow evaporation but not condensation
vapor pressure would decrease
boiling point would increase

Question 24

what happens in the evaporation of a liquid

Answer 24

the solution decreased vapor pressure

Question 25

boiling point

Answer 25

Temperature at which the vapor pressure equals the atmospheric pressure. If vapor pressure decreases, the boiling point must increase

Question 26

what happens when you add a solute to a solvent

Answer 26

Salt or ANY solute will lower the freezing point of any solvent. This can melt ice because the air is no longer cold enough to freeze it.

Question 27

what happens when ice melts

Answer 27

When the ice melts, the solution gets colder because melting is endothermic

Question 28

what is the freezing point depression

Answer 28

h20(l) H20(s) at the melting point 0 degrees equilibrium is established and occurs fast. By adding a solute, [H2O(l)] is decreased. That decreases the speed of freezing but not melting. At a lower temperature equilibrium is reestablished.

Question 29

whats colligative properties

Answer 29

These colligative properties depend only on the amount of solute, not on the type of solute.

Question 30

* if doing IONIC(metal to nonmetal) compound, what should you do to find all the particles

Answer 30

if doing an ionic compound, write out all elements to find the number of particles

Question 31

* how can you tell what a particle is by looking at the chemical formula of all nonmetals

Answer 31

if molecule is all non-metals the entire formula is a particle

Question 32

what happens when you add salt to a solute

Answer 32

lowers freezing point of ANY solvent. Melts ice b/c air not cold enough to freeze it

Question 33

how do you get a boiling point

Answer 33

temp. when vapor pressure is = to atm | if vapor pressure decreases, boiling point rises

Question 34

describe every variable in colligative properties

Answer 34

Where ΔT is the change in freezing or boiling point, m is the concentration of the solution in molality, K is a constant for the solvent, and i is the number of particles the solute splits up into when dissolved.

Question 35

osmosis

Answer 35

Osmosis is the flow of water from a region of low solute concentration to high solute concentration.

Question 36

diffusion

Answer 36

Diffusion is the flow of solute particles from a region of high solute concentration to low solute concentration.

Question 37

semipermeable membrane

Answer 37

A semipermeable membrane is one that allows the solvent, but not the solute, to diffuse from one side of the membrane to the other

Question 38

osmotic pressure

Answer 38

Osmotic pressure also only depends on the amount of solute, not on the type of solute.

Question 39

describe every variable in the osmotic pressure equation

Answer 39

Where π is the osmotic pressure, V is the volume in liters, i is ionization factor, n is the moles of solute, R is the ideal gas constant, and T is temperature in Kelvin.

Question 40

tonicity

Answer 40

when all water leaves, hypertonic when solute and solvent is equal, isotonic when all water goes to solute, hyPOtonic

Question 41

what does the solubilities of solids and gases depend on

Answer 41

solids- higher temp=more soluble | gases- higher tem=LESS soluble

Question 42

two most important anions in the body

Answer 42

potassium, sodium, chlorine and HCO