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Chemistry > Chapter 7 - Solutions > Flashcards

Chapter 7 - Solutions Flashcards

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1
Q

solvent

A

the substance present in greater amount

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2
Q

solutes

A
  • spread evenly throughout the solution
  • cannot be separated by filtration
  • can be separated by evaporation
  • are not visible, but can give a color to the solution
  • the solute can be molecular or ionic and is dissolved in the solvent
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3
Q

the solute and solvent in a solution can be a combination between?

A

solid, liquid, and or gas

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4
Q

gas solutions

A

gas in a gas = air

O2(gas) + N(gas)

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5
Q

liquid solutions

A

gas in a liquid soda water CO2 + H20 and NH3 + H20
liquid in a liquid (vinegar) acetic acid and water
sollid in a liquid (seawater) NaCl + H20
iodine + alocohol

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6
Q

solid solutions

A

liquid in a solid = dental amalgam = mercury L + silver S

solid in a solid = Brass = Zn S + Cu S and Steel C S + Fe S

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7
Q

Factors that affect dissolving rate

A
  • conditions that increase the mixing between solvent and solute increase that speed of solution formation
    a. particle size
    b. temperature
    c. stirring/agitatioin
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8
Q

particle size

A

smaller crystals will have a larger surface to volume ratio

- smaller crystals will dissolve faster due to the increased solute-solvent contact

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9
Q

temperature (for solid)

A

at higher temperatures solvent molecules posses more kinetic energy (more movement)
- at higher temp solvent molecules will hit the crystal surfaces with more force and frequency

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10
Q

stirring/agitation

A

increases the solute - solvent contact

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11
Q

solubility

A

the maximum amount of solute that dissolves in a specific amount of solvent
- expressed as grams of solute in 100 grams of solvent usually water
g of solute
__________
100 g of water

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12
Q

solubility term for solid

A

soluble, slightly soluble, insoluble

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13
Q

solubility term for liquid

A

miscible, immiscible, partially miscible

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14
Q

Factors that affect solubility

A

Temperature
pressure
nature

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15
Q

temperature

- affects solubility

A

in general, the solubility of solids increases with increasing temperature
- sulobulity of gases decreases with increasing pressure

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16
Q

pressure ( gases)

- affect solubility

A

the solubility of gases increases with increasing pressure

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17
Q

nature of solute/solvent

- affect solubility

A

like dissolve like

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18
Q

Aqueous solution

A

solution in which water is the solvent

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19
Q

Water

A
  • the most common solvent
  • the most important solvent for life
  • polar molecule
  • forms hydrogen bonds between hydrogen atom in one water molecule and the oxygen atom in a different water molecule
  • only ionic compounds and polar molecules are solute in water
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20
Q

What are soluble in water?

A

only ionic compounds and polar molecules

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21
Q

some ionic compounds, like NaCl dissolve very well in water at room temperature because of?

A

ion-dipole attraction

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22
Q

compounds that dissolve in a solvent are said to be? while those that do not are said to be?

A

soluble,

insoluble

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23
Q

the degree of solubility depends on?

A

the temperature

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24
Q

concentrated solutions

A

contains large amounts of solute

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25
Q

dilute solutions

A

contain small amounts of solute

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26
Q

unsaturated solutions

A

contain less than the maximum amount of solute

- can dissolve more solute

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27
Q

saturated solutions

A

contain the maximum amount of solute that can dissolve

- have un-dissolved solute at the bottom of the container

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28
Q

Concentration (equations)

A

C = Solute = amount of solute/ amount of solution

  1. percentage concentration: % m/m; m/v; v/v
  2. Molar concentration (molarity) M = mole of solute/L of solution
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29
Q

Isotonic solutions of iv fluids

A

NaCl = .9% m/v (saline)

5% glucose m/v

30
Q

common solutions: percentage concentration

A

vinegar: .5% v/v
hydrogen peroxide H2O2 30% v/v
rubbing alcohol: isopropanol = 70% v/v

31
Q

Dilution problems equation

A

C1V1 = C2V2

32
Q

What happens when a solute dissolves in water?

A

individual solute particles are attracted to the surrounding water molecules

  • they are pulled off and away from the solute
  • when particles enter the solution, each solute particles are surrounded by water molecules (hydrated) and become insulated from one another
33
Q

ionic compounds dissociate into?

A

cations and anions

- Ionization

34
Q

molecular compounds dissolves into?

A

individual molecules

35
Q

electrolytes

A

materials that dissolve in water to form a solution that will conduct electricity

36
Q

nonelectrolytes

A

materials that dissolve in water to form a solution that will not conduct electricity

37
Q

strong electrolytes

A 
materials that dissolve completely as ions-only ions are present in solution
- water soluble ionic compounds
- strong acids
- strong bases
their solutions conduct electricity well
38
Q

what are the strong acids?

A 
HNO3
HClO4
H2SO4
HCl
HBr
HI
39
Q

What are the strong bases?

A 
LiOH
KOH
RbOH
NaOH
CsOH
Sr(OH)2
Ba(OH)2
Ca(OH)2
40
Q

weak electrolytes

A

materials that dissolve mostly as molecules, but partially as ions

  • weak acids
  • weak bases
  • their solutions conduct electricity, but not well
41
Q

acids

A

H-containing molecular compounds that ionize when they dissolve in water

42
Q

when acids ionize, they form?

A

H+ and anions

  • percentage of molecules that ionize varies from one acid to another
  • acids that ionize virtually 100% are called strong acids
43
Q

acids that only ionize a small percentage are called?

A

weak acids

44
Q

acids that ionize virtually 100% are called?

A

strong acids

45
Q

Dissociation Equation for strong electrolyties (soluble ionic compounds)

A

Kl(aq) ->

46
Q

what happens when compounds containing a polyatomic ion dissolve

A

the polyatomic ion stays together

47
Q

dissociated cations and anions are the?

A

species actually existing in the aqueous solution

48
Q

dissolution equation for non-electrolytes

A

non-electrolytes are compounds that dissolve into molecules
- there is no ions in the aqueous solutions of nonelectrolytes
C12H22O11 -> C12H22O11

49
Q

our body fluids, such as intra- and extra cellular fluids and blood are?

A

solutions containing many different cations and anions
Cat: Na, K, Ca, Mg
Ani: Cl, HCO3-, CO3^2-, PO4_3-

50
Q

Equivalent Eq and milli-equavalent mEq

A

of Eq = charge of ions x mole of ion

1 Eq of Na+1 = 1mole x charge of Na = 1000mEq

51
Q

the concentration of ions in body fluids are most conveniently expressed in terms of?

A

mEq/L

52
Q

Electrolytes in body fluids

cations vs anions

A

must balance each other

if there is 155mEq/L of cations, there must be 155mEq/L of anions

53
Q

what are the colligative properties of solutions?

A
  • osmosis
  • hypertonic, isotonic, and hypotonic solutions and the red blood cells
  • dialysis
54
Q

colligative properties of solutions

- the properties of a solvent change by?

A

the presence of solute molecules

55
Q

the change in properties of colligative properties of solution depends on?

A

the number of particles (mole of solute) in a given amount kg of solvent and not on the nature or the mass of the particles

56
Q

colligative properties of solutions

- adding 1 mole of Urea in water or any substance

A
  • depresses freezing temperature - -1.86 C
  • elevation of boiling temperature = 100.512 C
    increases in osmolarity
57
Q

osmosis

A

the passage of a solvent from a dilute solution (or pure solvent) across a semi-permeable membrane into a more concentrated solution

58
Q

osmotic pressure

A

the pressure required to stop the net flow of solvent through the membrane

59
Q

at equilibrium of osmotic pressure

A

there is no net movement of H2O and the liquid levels stabilize

60
Q

the higher the solute concentration

A

the higher the osmolarity

61
Q

the osmotic pressure is determined by?

A

relative number of impermeable solute particles on two sides of the semi-permeable membrane, not the nature of the solute particles

62
Q

the outer most cell membrane

A
  • plasma
  • semipermeable membrane
  • permeable to H20, urea, O2, and CO2
  • not permeable to electrolytes and proteins
63
Q

solution with the same osmotic pressure as the intracellular fluid of RBC is?

A

isotonic

64
Q

hypertonic

A

solution with higher osmotic pressure

65
Q

hypotonic

A

solutions with lower osmotic pressure

66
Q

effect of solute concentration on tonicity of red blood cell

A

shrinking - crenation - hypertonic
swelling - hemolysis - hypotonic
no change - isotonic

67
Q

osmosis in normal body function

A
  • absorption of water by small intestine

- drinking sea water (3.5 NaCl) cause body to lose water rather than absorb it

68
Q

conditions associated with osmolarity imbalance

A
  • dehydration, over sweating
  • over hydration
  • drinking methanol (wood alcohol) or anti-freeze
69
Q

reverse osmosis in water

A

purification/desalination

70
Q

dialysis

A
  • common lab technique for separating molecules in solution by the difference in theri rates of diffusion through a semipermeable membrane
  • solvent and small solute particles pass through an artificial membrane; large particles are retained inside
  • waste particles such as urea from blood are removed using hemodialysis
71
Q

hemodialysis (artificial kidney)

A

artificial membrane with small pores that allow small waste molecules in the blood (urea, or other small waste metabolites) to diffuse out while retain large particles (platelet, red/white blood) cells and large molecules (plasma proteins)

72
Q

homogenous mixture

A

two or more substances

- consists of a solvent an done or more solutes

Chemistry (17 decks)

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