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Chem 2B > Chapter 17 Solutions > Flashcards

Chapter 17 Solutions Flashcards

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1
Q

Dalton’s Law of partial pressures

A

The P total is the sum of all partial pressures
Ptot= Pgas1 + Pgas 2 + Pgas3…

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2
Q

A solution has two components.

A

A solute (lesser) A solvent (greater)

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3
Q

Solutions Examples (Solute and Solvent)

A

Humidity - Gas - Gas
Rain - Liquid - Gas
snow - Solid - Gas
Carbonated Drinks, Sodas - gas -Liquid
Gin and Tonic - Liquid - Liquid
Salt Water, Solutions in lab- Solid -Liquid

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4
Q

Solution concentration

A

Molar (M)= amount of solute (moles)/ volume of solution (liters)

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5
Q

Percents (Formulas)

A

Mass percent:
(mass of solute/mass of solution) x 100
Volume percent:
(volume of solute/volume of solution) x 100) Volume is based on the initial volumes.
Mass Volume percent
(mass of solute(grams)/ volume of solution(mL)) x 100

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6
Q

Parts per Unit

A

a. Part per million:

1ppm= 1mg/L = 1g solute/ 1 x10^6g solution

b. Part per billion

1ppb = 1 ug/L = 1g /10^9 solution

c. Part per trillion

1ppt = 1ng/L = 1g/ 10^12 g solution

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7
Q

Mole Fraction (xi) and Percent
Mole percent xi (100)

A

xi = moles of i/ (total solution moles)

where xi +xj + xk+… =1.00

mole percent = 100xi

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8
Q

Molality(m)

A

amount of solute (moles)/ mass of solvent (kg)
Molality and Molarity are equal for dilute solutions where water is the solvent
Solution density is that of water (1g/mL)
(1L solution) (1000mL/L) (1g/mL) (kg/1000g) = 1kg solution

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9
Q

Normality (N)

A

the molarity multiplied by the number of equivalents. Used with acids( H+), bases (OH-), redox and precipitation
Normality (N) = ( # of equivalents) (Molarity)

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10
Q

Solubility

A

amount of solute that can be dissolved in a solvent.

Solubility = grams of solute dissolved/ given mass or volume of solvent

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11
Q

Molar Solubility

A

units are moles of solute per liter of solution
M soln = M solute + M solvent

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12
Q

Volume formula

A

Sometimes they are additive unless there is stated volume change or density change
V soln = V solute + V solvent

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13
Q

Polar molecules

A

Asymmetric molecules
Water, ionic compounds, salts, Alcohol, Water-Soluble Compounds, Hydrophillic

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14
Q

Non-polar molecules

A

Symmetric molecules
- Hydrocarbons
Molecular compounds
Oils, etc.

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15
Q

Like dissolves like idea

A

When polar molecules interact with other polar molecules, and non-polar molecules interact with other non-polar molecules they dissolve each other.

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16
Q

Enthalpy of solution

A

Enthalpy solution > 0 is endothermic
Enthalpy of solution < 0 is exothermic

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17
Q

Factors that contribute to enthalpy of solution

A

Breaking the solute into individual components, called expanding the solute endothermic
- Overcoming intermolecular forces in solvent to make room for the solute called expanding the solvent. (H2) endothermic

  • Allowing the solute and the solvent to interact to form a solution (H3) exothermic

H soln = H1 + H2 + H3

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18
Q

Ideal solution

A

Change in enthalpy = 0

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19
Q

Possible combinations:

A

Solutes and Solvents:
Polar = Enthalpy large > 0
Non-polar with Enthalpy is small. < 0

When all values are small or Large they cancel each other out or dissolve and become small.

A mixture of both small and large: Total enthalpy = Large

Total Enthalpy small = solution forms
Total Enthalpy Large = no solution forms

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20
Q

Solution formation and equilibrium

A

Dissolving process will occur until equilibrium is reached
Solute + Solvent = Solution

Solubility (increases with temp except sulfates and phosphates).

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21
Q

Saturated

A

Saturated line represents the point where the dissolution and crystallization are both occuring and in equilibirum wiht each other

22
Q

Undersaturated

A

Region on the graph below the saturated line when the solven cen dissolve more solute than available.

23
Q

Supersaturated

A

Region on the graph occurs when the solution has more solute in solution than equlibrium allows.
Scenario = unstable and cause excess solute to crystalize

24
Q

Fractional Crystallization

A

Solubulity to seperate solute.
Ex: Impure solid with mostly A and some B. Dissolve solide in high
temp then cool solution and each A and B will crystalize at different times.

25
Q

Structure effects

A

Structure is affected extremely by solubility:

Fat soluble compound are non-polar

Water-soluble compounds are polar

26
Q

What are Fat soluble compounds composed of?

A

Mostly C and H atoms and possibly on e OH group

27
Q

What are water-soluble compund composed of

A

Mostly OH groups (polar) along with C and H atoms

28
Q

Temp effects

A
  • Soldis dissolved in liquids = solubility increases as temp increaese
  • gases dissolved in liquids = the solubility of a gas in a liquid decrease as temperature increases.
    Reason is because the increase temp increases the kinetic energy of the gas causing the gas to escape the solution
29
Q

Pressure effects (For gases dissolved in liquid

A

As pressure increases the solubility of a gas in a liquid increase

30
Q

Henry’s Law

A

C is solubility or concentration. K is Henry’s law constant.
Pgas = pressure of gas

Formula examples
C= k Pgas
k = C1/P1 = C2/P2

C= mol/L

31
Q

Raoult’s Law

A

Partial pressure (Pa) = to the mole fraction (xa) multiplied by the pure pressure of solvent (PA o)

Pa = xa PoA
Pb = xbPbO
Xa +Xb =1.00
Ptot = Pa+ PB
Ptot = xA PA^o + xbPB^o
PA = xAPtot

32
Q

novolatile

A

Does not have an appreciable vapor pressure. Partial pressure of the solvent is the only contributor to total pressure.

33
Q

Negative deviation

A

When there is a mixture of polar molecules

34
Q

Positive deviation

A

When there is a mixture of polar and nonpolar molecules

35
Q

Behavior of various types of solutions

A

Unlike forces = like forces
(Enthalpy soln) = 0

Raoul’s law Deviation:
None(ideal solution)

Polarity:
Nonpolar -Nonpolar interaction

Unlike forces > like forces
Enthalpy soln (Negative )

Raoult’s Law deviation:
Negative

Polarity
Polar- Polar interaction

Unlike forces < like forces
Enthalpy solution (Positive)

Raoult’s Law Deviation

Positive

Polarity
Nonpolar - polar
interaction

36
Q

Osmotic Pressure (Π)

A

When a solute is separated by a semipermeable membrane, pure solvent will pass into the solution by osmosis= large pressure

Π = MRT
M= Molarity T in Kelvin. R is 0.08206 L atm/mol K.

37
Q

Chang in temperature is calculated as follows where k is given constant for the solvent and m is molarity.

A

Change in T = km

Concentration should be considered when there is a change in temperature.

Also, when you calculate the boiling point of a value and you are solving for change in enthalpy add an additional 100 celcius

38
Q

Bp and Fp relasonship

A

If it takes more energy for the solvent molecules to leave the solution the bp will be higher

Concentration should be considered

39
Q

Colligative properties affect fp, bp, and Π

A

Also, they use an electrolyte as a solute is adjusted by the van’t Hoff factor. Eelctrolyes need adjustment because they sperate in solution adding more particles than expected.

i = moles of particles in solution/ Moles of solute dissolved

i has different values depending on the compound. If compound is weak on non-electrolyte then i =1.

40
Q

Strong electrolytes

A

Strong acids
Strong Bases
Ionic compounds
Salts

41
Q

Weak or Non-Electrolytes

A

Weak acids (any state)
Weak bases (any state)
Molecular Compounds
Organic compounds
Liquids, Solids, and gases.

42
Q

Colligative property formula include i as follows

A

Change in T = ikm
Π = iMRT

43
Q

Colloid

A

A suspension of particles which is stabalized by electrostatic repulsion.

44
Q

Mass percent formula

A

Mass of solute in grams/ total mass (in grams) x 100 percent

45
Q

Volume percent

A

Volume of solute (in mL) / total volume (in mL) x 100 percent

46
Q

Mass Volute Percent Formula

A

Mass of solute in grams / total volume (in mL) x 100 percent

47
Q

Low solute concentrations of aqueous solutions are express using ppm

A

Mass of solute (in grams)/ total mass (in grams) x 10^6

48
Q

Mole fraction

A

Xi = moles of component i/ total moles of all components

X1 + X2 + X3 + … Xn = 1

49
Q

Mole % i

A

Xi x 100percent

50
Q

Molarity (M)

A

Moles of solute/ volume of solution (in liters)

51
Q
A

Chem 2B (12 decks)

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