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General Chemistry MCAT > Chapter 4: Solutions > Flashcards

Chapter 4: Solutions Flashcards

(50 cards)

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1
Q

Compound of which there is MORE is called a ______ and the compound of which is LESS is called _______.

When neither compound predominates, BOTH compounds are referred to as ________.

A

Solvent; Solute

Solvents

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2
Q

3 Types of solutions

A

1) Ideal solutions - made from compounds that have similar properties (meaning compounds can be interchanged within the solution w/o changing spatial arrangement of the molecules or intermolecular attractions); Example: Benzene in toluene
2) Ideally dilute solutions - solute molecules are completely separated by solvent molecules so they have NO interaction with each other.
3) Nonideal solutions - violate both conditions

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3
Q

Example of Colloid

A

Hemoglobin

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4
Q

Colloidal system can be any combination of phases except for…

A

Gas in gas

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5
Q

Example of colloidal systems

A

Aerosol - LIQUID or SOLID particles in a gas like fog/smoke

Foam - GAS particles in a LIQUID (like whipped cream)

Emulsion - LIQUID particles in a LIQUID or solid like milk or butter

Sol - SOLID particles in LIQUID like paint

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6
Q

Colloid particles may be ATTRACTED (_________) or REPELLED (________) by their dispersion medium.

A

Lyophilic; lypophobic

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7
Q

Lypophobic colloids form when amphipathic (hydrophilic and hydrophobic parts) or charged particles ________ to the surface of the colloidal particles which stabilizes them in the dispersion medium.

A

Absorb

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8
Q

General rule for dissolution (dissolving) is…

A

‘Likes dissolve likes’

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9
Q

These molecules are held together by STRONG intermolecular bonds formed by the attraction b/n their __________ charged ends.

These molecules are held together by WEAK intermolecular bonds resulting from instantaneous _________ moments.

These forces are called….

A

Highly polar molecules; partially charged

Nonpolar molecules; dipole

London dispersion forces

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10
Q

A ________ solute interacts with a _________ solvent by tearing __________ bonds apart and forming ___________ bonds.

A

Polar; polar

Solvent-solvent; solvent-solute

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11
Q

No polar solvent can tear apart a WEAK bond of a _________

A

Nonpolar solvent

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12
Q

Ionic compounds are dissolved by ….

A

Polar substances

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13
Q

Process of Solvation

A

When ionic compounds dissolve, they break apart into their respective cations and anions and are surrounded by OPPOSITELY charged ends of the POLAR SOLVENT.

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14
Q

When water molecules surround individual ions pointing their positive hydrogens at the anions (-) & their negative oxygens towards cations (+)

When several molecules attach to one end of an ionic compound, they’re able to overcome the strong ionic bond, and break the compound. The water molecules then surround ion. In water this process is called ….

A

Hydration

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15
Q

Something that’s hydrated is …

Define hydration number

A

An aqueous phase

Number of water molecules needed to surround an ion that varies according to the size & charge of the ion. *This # is commonly 4 or 6

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16
Q

Compound that forms ions in an aqueous solution is called an …

STRONG electrolytes

WEAK electrolytes

A

Electrolyte

Create solutions which CONDUCT ELECTRICITY well and CONTAIN MANY IONS.

Compounds which form FEW IONS in solution

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17
Q
  • Nitrite
  • Nitrate
  • Sulfite
  • Sulfate
  • Hydrochlorite
  • Chlorite
  • Chlorate
  • Perchlorate
  • Bicarbonate
  • Phosphate
A
  • NO2-
  • NO3-
  • SO3^2-
  • ClO-
  • ClO2-
  • ClO3-
  • ClO4-
  • CO3^2-
  • HCO3^-
  • PO4^3-
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18
Q

Fun fact: what is “HYPONATREMIA”

What are NORMAL sodium levels?

What low sodium levels due to drinking too much water can be critical or even lead to death?

A

When sodium levels become too low (reduced sodium levels) as a result of drinking too much water

135mM-145mM

125-120mM or lower

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19
Q

5 Ways to measure concentration

A

1) Molarity (M): mols of compound/ vol of solution (unit: mol/vol)
2) Molality (m): mols of solute/ kg of solvent (unit: mol/kg)
3) Mole Fraction (X): mols of compound/ total moles of all species in sol’n (units: NONE)
4) Mass percentage: 100 x’s the ratio of the mass of the solute/ total mass of solution
5) Parts per million (ppm): 10^6 x’s the ratio of the mass of solute/ total mass of solution

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20
Q

Define a solution

A

Homogenous mixture of 2 or more compounds in a solid, liquid, or gas

Example: Brass
A solid solution of zinc and copper

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21
Q

Grams / mw =

22
Q

1 atm =

23
Q

Formation of a solution is what type of reaction?

24
Q

Physical reactions involve 3 steps:

Study These Flashcards
A

1) Breaking the intermolecular bonds between the solute molecules
2) Breaking the intermolecular bonds between the solvent molecules
3) Forming of intermolecular bonds between the solvent and the solute molecules

25
Entropy INCREASES for _____ & _____ dissolving in _______. Entropy usually DECREASES for ________ dissolving in _______.
Solid and liquids; liquids Gases; liquids
26
If the overall reaction RELEASES energy (exothermic) , the new intermolecular bonds are ________ and intermolecular attractions within the solution are STRONGER than the intermolecular attractions with the PURE substance. Less energy in the system means what? If the OVERALL reaction ABSORBS energy (endothermic) then ....
MORE stable A MORE STABLE system The REVERSE is TRUE
27
Overall Change in energy of the reaction is = to the change in ENTHALPY and is called .... A NEGATIVE heat of solution results in A POSITIVE heat of solution results in
The heat solution (delta)Hsol STRONGER intermolecular bonds WEAKER intermolecular bonds
28
Since COMBINED mixture is MORE DISORDERED than the separated pure substances, the formation of the solution involves a what kind of entropy? Exception to increased entropy rule is what?
Increased When a gas dissolves in a liquid or solid - this allows for the entropy change to be NEGATIVE
29
When a liquid or solid dissolves into one another the entropy does what?
Increase entropy
30
-(delta)G indicates what type of reaction? When a LIQUID or SOLID dissolves in a LIQUID, (delta)S (entropy) is usually what? Therefore entropy usually does what?
Spontaneous Positive; FAVORS spontaneous solution FORMATION
31
Vapor pressure of liquid Vapor pressure of the compound
Pressure created by the molecules in the open space Equilibrium b/n liquid & gas phases of compound occurs when molecules move from liquid to gas (L➡️G) as quick as G⬅️L . Partial pressure of the compound necessary to create EQUILIBRIUM is VP OF COMPOUND
32
When a fluid moves what happens to the partial pressure?
The partial pressure of WATER VAPOR DECREASES!!
33
Partial pressure of water vapor is LOWER than the vapor pressure of water at that temp, and # of water molecules leaving is ______ than the # of water molecules entering the water. Which means the water is doing what?
Greater | Evaporating
34
What causes a compound to boil??
Vapor Pressure = local atmospheric pressure
35
What is atmospheric pressure?
The sum of ALL partial pressures in the air above the liquid
36
Define MELTING POINT
Temperature of at which the VP of the SOLID is = VP of LIQUID
37
What is a NONVOLATILE SOLUTE What is a VOLATILE SOLUTE
A solute with NO VP A solute with VP
38
What's an ideal solution
Where a solute and solvent have similar properties
39
Some molecules of a volatile solute escape from solution & contribute to ...
VP
40
What is solubility?
A solutes's tendency to dissolve in a solvent | On MCAT: A solute will mostly be a SALT and the SOLVENT will be WATER
41
Dissolved molecules of SALT reattach to what?
The SURFACE of the SALT CRYSTAL
42
What is PRECIPITATION? INITIALLY precipitation takes place at a _______ rate than dissolution
The reverse reaction of a dissolving salt SLOWER
43
As salt DISSOLVES, the CONCENTRATION of salt _____, the rate of DISSOLUTION and PRECIPITATION _______.
BUILDS EQUILIBRATE
44
Dissolution = precipitation, the solution is what? When Saturated, the concentration of dissolved salt reaches a ______ in a saturated solution.
SATURATED
45
Is the crystallization of salts endothermic/exothermic?
Exothermic
46
Solubility is.... Solubility depends upon what?
The maximum # of moles of the solute that can dissolve in solution Temperature & ions in a solution
47
Solubility Product changes only with what?
Temperature
48
Spector Ion Common Ion Effect
Ions that have NO effect on EQUILIBRIUM (ex. Sodium ions: Na+) Ions that DO affect the EQUILIBRIUM (F-) b/c it involves AN ION COMMON TO AN ION IN EQUILIBRIUM
49
Le Chatalier's Principle
The ADDITION of a COMMON ION will push the equilibrium In a direction which tends to REDUCE the concentration of that ion
50
As temp _________, salt _______.
Increases; increases

General Chemistry MCAT (4 decks)

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