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DTCC Chemistry > Unit 6 > Flashcards

Unit 6 Flashcards

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1
Q

homogeneous

A

uniform mixture

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2
Q

heterogeneous

A

non-uniform mixture

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3
Q

whats the two types of HOMOgeneous mixtures

A

solutions and collodis

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4
Q

what is a usual characteristic of a solution

A

solutions are usually transparent

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5
Q

whats a observable(visual) characteristic of colloids

A

cloudy/milky or gel-like

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6
Q

what happens when something dissolves

A

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

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

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7
Q

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

A

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

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8
Q

colloid

A

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

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9
Q

whats to solvent dispersed phase of butter

A

gel

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10
Q

what state is shaving cream considered

A

foam

gas as dispersed phase, liquid as solvent phase

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11
Q

what phase is paint

A

sol

solid in dispersed and solvent phase

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12
Q

perfume is an example of what phase

A

liquid aresol

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13
Q

what type of liquid is transparent

A

SOLUTIONS ARE TRANSPARENT

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14
Q

whats a suspension?

A

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.

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15
Q

whats the difference between heterogeneous mixture, colloid and solution

A

size

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16
Q

solubility

A

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.

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17
Q

saturation

A

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.

18
Q

describe supersaturation and precipitation

A

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).

19
Q

whats the equation for vapor pressure

A

Vapor Pressure = Pressure of Gas at Equilibrium

whats happening all the time

20
Q

what is the speed of a reaction proportional to

A

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

21
Q

whats the equation for the speed of a reaction

A

k[h20(l)]

22
Q

what does every variable in the speed of a reaction mean

A

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

23
Q

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

A

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

24
Q

what happens in the evaporation of a liquid

A

the solution decreased vapor pressure

25
Q

boiling point

A

Temperature at which the vapor pressure equals the atmospheric pressure.

If vapor pressure decreases, the boiling point must increase

26
Q

what happens when you add a solute to a solvent

A

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.

27
Q

what happens when ice melts

A

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

28
Q

what is the freezing point depression

A

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.

29
Q

whats colligative properties

A

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

30
Q
  • if doing IONIC(metal to nonmetal) compound, what should you do to find all the particles
A

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

31
Q
  • how can you tell what a particle is by looking at the chemical formula of all nonmetals
A

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

32
Q

what happens when you add salt to a solute

A

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

33
Q

how do you get a boiling point

A

temp. when vapor pressure is = to atm

if vapor pressure decreases, boiling point rises

34
Q

describe every variable in colligative properties

A

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.

35
Q

osmosis

A

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

36
Q

diffusion

A

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

37
Q

semipermeable membrane

A

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

38
Q

osmotic pressure

A

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

39
Q

describe every variable in the osmotic pressure equation

A

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.

40
Q

tonicity

A

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

41
Q

what does the solubilities of solids and gases depend on

A

solids- higher temp=more soluble

gases- higher tem=LESS soluble

42
Q

two most important anions in the body

A

potassium, sodium, chlorine and HCO

DTCC Chemistry (13 decks)

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