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Chemistry > Unit 8 Test > Flashcards

Unit 8 Test Flashcards

1
Q

What are the properties of water and how do they relate to hydrogen bonding?

A

It has high surface tension, and low vapor pressure, freezes into a honeycomb shape, is a universal solvent, has a high boiling point, and has a high specific heat capacity.

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2
Q

What is the Tyndall effect?

A

the scattering of light by particles

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3
Q

What is Brownian motion?

A

the random motion of particles

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4
Q

What’s a solution?

A

Solute+Solvent, homogenous, particles less than 1nm

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5
Q

What are suspensions?

A

can see them and are bigger than 1000 nm

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6
Q

What are colloids?

A

between 1 nm and 1000 nm

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7
Q

A colloidal dispersion of a liquid in a liquid (mayo)

A

emulsion

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8
Q

What is a solvent?

A

dissolves solute

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9
Q

What is a solute?

A

the stuff being dissolved

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10
Q

saturated

A

can’t dissolve anymore/contains max of solute for solvent

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11
Q

unsaturated

A

contains less solute than a saturated solution

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12
Q

supersaturated

A

contains more solute then theoretically could be held at given temperature

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13
Q

property that depends on the number of solute particles, not identity

A

colligative property

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14
Q

What are the three colligative properties of solutions?

A

Vapor Pressure lowering, freezing point depression, boiling point elevation

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15
Q

What effect does the solute have on Vapor pressure?

A

solute particles reduce the number of free solvent particles able to escape the liquid.

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16
Q

What effect does the solute have on Freezing point depression?

A

the magnitude of freezing point depression is proportional to the number of solute particles dissolved.

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17
Q

What effect does the solute have on Boiling point elevation?

A

the magnitude of boiling point elevation is proportional to the number of solute particles dissolved in solvent.

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18
Q

What are the factors that determine how fast a substance dissolves?

A

stir it up, heat it up, beat it up

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19
Q

How many particles are in the following
C6H12O6
Na2SO4
KNO3

A

1
3
2

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20
Q

What does it mean to beat it up?

A

break into smaller particles so that there is more surface area

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21
Q

dilute

A

not concentrated

22
Q

What is the formula for dilutes?

A

M1xV1=M2xV2 M=molarity. V=volume

23
Q

Suppose you need 250 mL of 0.20M NaCl solution, but the only supply of sodium chloride you have is a solution of 1.0M NaCl. Describe how you would prepare the required solution.

A

200mL

24
Q

What is concentration?

A

how much stuff is in your stuff

25
Q

What’s the formula for concentration?

A

M=mole S solute/L solution=
mol/L

26
Q

Calculate the molarity of a solution made by dissolving 95.0 g of MgCl2 in enough water to make 750 mL of the solution.

A

1.33 M MgCl2

27
Q

How much you can put for it to dissolve or the amount that can dissolve at a given temperature and pressure

A

solubility

28
Q

The solubility of methane, the major component of natural gas, in water at 20 degrees C and 1.00 atm pressure is 0.026g/L. If the temperature remains constant, what is the solubility of this gas at 1.80 atm?

A

0.05

29
Q

What is the formula for solubility?

A

g/L. g/L
—— =. ——-
atm. atm.

30
Q

The number of moles of solute in 1 liter of solution

A

molarity

31
Q

What is the formula for molarity?

A

M= moles of solute/liters of solute

32
Q

What does henry’s law mean

A

gases are only affected by pressure

33
Q

What’s the formula for henrys law

A

S1/P1=S2/P2
S=g/L
P=atm, kPa, Torr

34
Q

How does polarity affect solubility?

A

like dissolves like
polar dissolves polar
nonpolar dissolves nonpolar

35
Q

If it dissolves in H20 it will conduct electricity

A

electrolyte

36
Q

weak electrolyte and what elements are

A

kinda dissociates (weak acids and bases) look for acetic acid HC2H3O2 and ammonia NH3

37
Q

strong electrolyte and what elements are

A

completely dissociates (salts or ionic compounds)

38
Q

non-electrolyte and what elements are

A

doesn’t dissociate (molecular compounds)

39
Q

Things with elements____ are most likely non-polar.

A

C

40
Q

ionic compounds dissolve in _____

A

polar

41
Q

What mass of Mg(OH)2 is produced when 75.0 mL of 0.425 M Mg(NO3)2 is added to excess NaOH solution according to the reaction given below
Mg(NO3)2 (aq) + 2NaOH (aq) ———> 2NaNO3 (aq) + Mg(OH)2 (s)

A

1.86 g Mg (OH)2

42
Q

solute ions or molecules become surrounded by solvent molecules

A

solvation

43
Q

aqueous solution

A

can dissolve in H20

44
Q

anything that is gonna interfere with hydrogen bonding and reduces the surface tension (soap or detergents)

A

surfactant

45
Q

The inward force or pull that tends to minimize the surface area of a liquid

A

surface tension

46
Q

When water is used as the solvent

A

water of hydration

47
Q

Water is a polar solvent and gasoline is a nonpolar solvent. Decide which compounds are more likely to dissolve in water and which are more likely to dissolve in gasoline.
Sucrose (C12H22O11)
Na2SO4
Methane (CH4)
KCl

A

gasoline
water
gasoline
water
ionic=polar
C=nonpopar
polar bonds with polar
non-polar bonds with non-polar

48
Q

What is the percentage of water in the hydrate FeSO4x7H20

A

45%
mass of H20/mass of hydrate

49
Q

What mass of NaNO3 (solubility=88.0g NaNO3/100g H20 at 20 degrees C) can dissolve in 250.0 g water?

A

220 g NaNO3

50
Q

What mass of CaCl2 is needed to make 250 mL of a 0.10M CaCl2 solution?

A

2.77 g CaCl2

51
Q

Aqueous solutions of aluminum chloride and sodium phosphate are mixed and a double replacement reaction occurs forming an aluminum phosphate precipitate.
Write the balanced chemical equation of the reaction
Write a balanced net ionic equation for the reaction that occurs
What are the spectator ions in the resulting solution
If 50.0 mL of a 1.50 M aluminum chloride solution is reacted with 75.0 mL of a 1.00 M sodium phosphate solution, which reactant would be the limiting reagent, and what mass of precipitate could theoretically be produced by the reaction?

A

AlCl3
10g

Chemistry (17 decks)

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