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Chemistry > Solutions > Flashcards

Solutions Flashcards

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1
Q

Solutions

A

homogeneous mixtures of two or more substances that combine to form a single phase (usually liquid but can be any phase!)

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2
Q

Mixtures

A

gases dissolved in other gases as the moleculles do not interact chemically

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3
Q

Solute and Solvent

A

solute is dissolved into the solvent

the solvent stays in the same phase after mixing and is in greater quantity

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4
Q

Solvation

A

electrostatic interaction between solute and solvent molecules. breaking of intermolecular bonds of solute/solvents and combining solute to solvent

Also known as Dissolution and hyrdation if water is the solvent

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5
Q

When new interactions are stronger than original ones, the solvation is an ____ process and favored at _____ temperatures

A

exothermic

low

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6
Q

hen new interactions are weaker than original ones, the solvation is an ____ exothermic process and favored at _____ temperatures.

A

endothermic

high

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7
Q

Ideal Solution

A

bonds before and after solvation are equal ins strength and enthalpy is 0

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8
Q

Whether or not dissolution will occur spontaneously is dependent on the ______, _____ and _____ change.

A

gibbs free energy, enthalpy and entropy

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9
Q

Solubility

A

maximum amount of substance that can be dissolved in a particular solvent at a given temperature

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10
Q

Saturation

A

when maximum solute has been added and is in equilibrium, any more solute added will not dissolve and will precipitate

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11
Q

Dilute

Concentrated

A

when solvent:solute ratio is much larger for the solvent side

when solvent:solute ratio is much larger for the solute side

either way maximum equilibirum concentration has not been met

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12
Q

When change in gibbs free energy is ____, solute is soluble. When it is _____, solute is ______

A

soluble, insoluble

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13
Q

Sparingly Soluble Salts

A

solutes that dissolve minimally in solvent (molar solubility under 0.1 M)

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14
Q

Aqueous Solution

A

most common solution where solvent is water and interact with solute with hydration

can form hydronium ions when acids are involved

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15
Q

General Solubility Rules

A
  1. all salts containing ammonium and alkali metal (group 1) cations are water soluble
  2. all salts with nitrate (NO3-) and acetate (CH3COO-) are water soluble
  3. Halides except flourides are water soluble UNLESS formed with Ag+, Pb2+ and Hg2 2+
  4. Salts of sulfate ions are water soluble except those with Ca2+, Sr2+, Ba2_ and Pb2+
  5. All metal oxides are insoluble except those with alkali metals, ammonium, CaO, SrO, and BaO which form metal hydroxides
  6. all hydroxieds are insoluble EXCEPT those with alkali metals, ammonium, Ca2+, Sr2+ and Ba2+
  7. all carbonates, phosphates, sulfides and sulfites are insoluble except those with alkali metal and ammonium
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16
Q

General Solubility Rule you NEED to know

A

all salts of group 1 metals and all nitrate salts are soluble

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17
Q

Complex Ion Complex/Coordination Compound

A

molecule where cation is bonded to atleast one electron pair donor (which may include water)

help together with coordinate covalent bonds where a lewis base (electron donor) and lewis acid (electron acceptor) form bonds

found in proteins, ex: hemoglobin in blood where oxygen, CO2 and CO are ligands

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18
Q

Ligand

A

electron pair donor molecule

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19
Q

Chelation

A

central cation bonds to same ligand in multiple places

large, organic ligands

20
Q

Volume Percent

A

volume of solute / volume solution * 100%

21
Q

Units of Concentration

A

mass. mole fraction, molarity, molality, normality

22
Q

Percent Composition by Mass

A

mass of solute / mass of solution *100%

23
Q

Mole Fraction (X)

A

Xa = moles of a / tota; moles of all species

summation of mole fractions in a system = 1

24
Q

Molarity (M)

A

moles of solute/liters of solution

25
Q

Molality (m)

A

moles of solute/ kilograms of solvent

boiling point elevation and freezing point depression

26
Q

Normality (N)

A

number of equivalents of interest per liter od solution

equivalent = mole of species of interest (hyroxide, proton, ion, electron)

ex: in acidic condition, 1 mole of permanganate ion accepts 5 moles electron so its normality is 5 N

27
Q

Dilution

A

C1V1 = C2V2

C = concentration in molairty

28
Q

Saturation Point

A

equilibrium reached during solution preparation where solute concentration is at its max at a given temp/pressure

29
Q

When a solution is unsaturated/dilute, the thermodynamically favored process is _____ and the rate of dissociation will be ____ than the rate of precipitation.

As the solution becomes more concentrated and approaches saturation, the rate of dissolution _____ and the rate of precipitation _____.

At equillibrium the change in free energy is _____

A

dissolution
increase
decrease

decreases
increases

0

30
Q

An ionic solid in a polar solvent dissociation equation

A

Am + Bn m A ^n+ + n B ^ m+

31
Q

Solubility Product Constant (Ksp)

A

these are equilibrium concentrations

for formula AmBn

Ksp = [A^n+]^m * [B^m-] ^n

**dissociation reactions never have a denominator for Ksp because they always start as solids!!!

32
Q

The solubility product constant_______with increases temperature for NON-GAS SOLUTES and _____ for GAS SOLUTES

Dissociation of gas solutes, Ksp will be ____ for gases at higher pressures than lower ones.

A

increases

decreases

higher

33
Q

Ion Product (IP)

A

IP = [A^n+]^m * [B^m-]^n

for reaction AmBn

analogous to Q, determines where a system is with respect to equilibrium, uses ‘current’ ion concentrations

IP < Ksp -> unsaturated

IP = Ksp -> saturated

IP > Ksp -> supersaturated

34
Q

Molar Solubility

A

molarity of a solute in a saturated solution

35
Q

Why do complex ions increase the solubility of a salt in solution?

A

formation of multiple polar bonds leads to increased dipole interactions and stabilizes the dissociation of the ion leading to high Ksp values.

36
Q

Formation/Stability Constant of Complex Ion in Solution (Kf)

A

formation of a complex ion after the dissolution of the original solution

the initial dissolution is the rate limiting step as it has the lower value in Ksp compared to the Kf

37
Q

Solubility is impacted by:

A

temperature, pressure and the addition of other substances to the solution

38
Q

The solubility of a salt is _______ when it is dissolved in a solution that contains one of its constituent ions compared to a pure solvent. This is known as the ________. Hence the molar solubility also ______.

However, Ksp is ______

A

considerably

common ion effect

decreases

constant

39
Q

Colligative Properties

A

physical properties of solutions that are dependent on the concentration of dissolved particles but not the IDENTITY of the particles

vapor pressure depression, bp elevation, fp depression, osmotic solutions

40
Q

Raoults Law

A

PA = XA PA(degree)

PA = vapor pressure of solvent A

XA = mole fraction of solvent

PA degree = vapor pressure of solvent A in pure state

accounts for vapor pressure depression caused by added solutes in solution

condensation rate is unaffected by the solute particles, but the evaporation rate is reduced by solute particles

applies only to ideal solutions where attraction between molecules of different components of mixture is equal to the attraction between molecules of any one component in its pure state

41
Q

When a nonvolatile solute is dissolved into a solvent, the boiling point of the solution will be _____ than that of pure solvent

If vapor pressure of a solution is lower than that of a pure solvent, then ____energy (______temp) will be required before its vaporpressure = ambient pressure

A

greater

more , higher

42
Q

deltaTb

A

deltaTb = iKbm

delta Tb = change in boiling point

i is vant Hoff factor number of particles produced from solute)

Kb is proportionality constant

m = molality

43
Q

The presence of solute particles in a solution interferes with the formation of the ______ of solvent molecules in the solid state. Thus, a _____ amount of energy must be removed resulting in _____ temps to solidify.

A

lattice

greater

lesser

44
Q

deltaTf

A

deltaTf = iKfm

Kf is proportionality for solvent

m is molality

45
Q

Osmotic Pressure

A

pressure generated ti draw water into a solution

II - iMRT

M - molarity

R - ideal gas constant

water moves towards higher solute concentration

Chemistry (9 decks)

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