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Inorganic Chem > Solution And Colligative Properties > Flashcards

Solution And Colligative Properties Flashcards

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1
Q

What is a solution

A

Homogenous micture composed of 2 or more substances

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2
Q

What are components of the solution

A

Solute-minority component
Solvent-majority component it determones physical state of the solution

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3
Q

In what states can solution be

A

•gas
•liquid
•solid-mainly alloys. Alloys of mercury are called amalgams and can be both liquid and solid

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4
Q

What is saturated solution

A

Solution at equilubrium with a solid in excess

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5
Q

What is solubility of the solute

A

Max mass that can be dissolved in a given mass/volume of the solvent at a particular T

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6
Q

How does temperature impact solubility

A

Of solids increases when T increases. And for the gasses it decreases when the temperature increases

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7
Q

What effect does pressure have on solubility

A

Little on solids and liquids
But it is important effect on solubility of gases

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8
Q

What law explains solubility of gasses

A

Henry’s law-mass of gas that can dissolve in a liquid is proportional to its pressure over the liquid.
c=k(H)×p
c=conc.of the gas
k(H)=Henry constant
p=pressure of the gas over the solution in atm

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9
Q

What is dissolution process

A

It consists of dispersing the particles of the solute in the solvent

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10
Q

Explain which conpounds would mix depending on interacrions between the molecules

A

The interaction between the solute and solvent have to be stronger than the interactions inside the pure substances.
•A-B=stronger than A-A and B-B, A and B will mix
•A-B are much weaker, wont mix
•if A-B are weaker , they may mix depending on T and composition

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11
Q

Explain like dissolves like

A

Substances must have similiar intermolecular forces to form solutions.
•non-polar dissolve in non-polar
•polar dissolves in polar

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12
Q

What does partially miscible mean

A

Wgen compound dissolves in some composituon but not the other

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13
Q

How do molecular substances dissolve

A

The solute has weak intermolecular forces.
They do not ionize and they can form solution through Lindon interactions,Hydrogen bonds etc. They dont conduct electricity

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14
Q

How do ionic compounds dissolve

A

Splute is held through solid electrostatic interactions. They are dissolved in polar solvents and are electrolytes(conduct electricity)

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15
Q

What factors determine dissociation of a ionic solid in polar solvent

A

•lattice energy-higher it is, the lower tendency do dissolve
•ion-dipole interactions(ion of solid and dupoles of the solvent molecule)-higher the interactions, higher tendency to dissolve.

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16
Q

What is solvation process

A

Process of reorganizing solvent and solute molecules. Ion/molecule is surrounded by solvent molecules

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17
Q

What is hydration

A

Solvation by water

18
Q

Can electrolyte be ionic and molecular compound

A

Yes.
For ionic it does dissociation and for molecular its ionozation

19
Q

Explain strength of the electrolyte

A

It can be weak and strong
Strong-completly dissociates its ions in solution
Weak-partially dissociates ions in the solution

20
Q

How are solvents classified

A

By polarity
•polar-present a dipolar moment and contain atomic bonds between the atoms with different electronegativity
•non-polar-contains atoms with similiar or same electronegativity

21
Q

How is polarity of a molecule evaluated

A

With dielectric constant. If its higher than 15->polar

22
Q

How are polar solvents devided

A

•protic-high dielectric constant and high polarity. They have H bonded to O,N,F. Molecules are ready to donate H+ to solutes, by hydrogen bonding
•aprotic-high dielectric constant and high polarity. They do not form hydrogen bonds or donate protons, but they still dissolve many salts

23
Q

What is concentration

A

It tells us how much solute is dissolved in particular volume of the solution.

24
Q

What are types of concentration

A

•molarity-> n/V(L)
•weight precentage-> mass(solute)×100/mass(solute+solvent)
•parts per million mass(solute)×10⁶/mass(solution); if its billion then 10⁹
•molality-> n/mass(kg)
•molar fraction–> X(a)=n(a)/n(a+b)

25
Q

What is dilution

A

It is procedure to prepare less concentrated solution. It is done by adding more solvent

26
Q

Formula for dispersion

A

MiVi=MfVf

27
Q

What are colligative properties

A

Properties that depend on the number of dissolved molecules.
Those are:
•Vapour pressure lowering
•Freezing point depression
•Boilint point elevation
•Odmotic pressure

28
Q

What is Raoult’s law

A

Partial pressure of the solvent in ideal solution(pA)=partial pressure of pure solvent(pA°)×mole fraction(XA)

29
Q

What happens to vappur pressures when substances are volatile

A

Vp of the splution is a sum of vp of single partial pressures
p(A)=pA°×X(A)
p(B)=pB°×X(B)
p(T)=p(A)+p(B)

30
Q

Give formulas for boiling point elevation and freezing point depression

A

•DeltaTb=T(solution)-T(solvent)=Kb(ebulliscopic constant)×m(molality)
•DeltaTf=T(solvent)-T(solution)=Kf(crioscopic constant)×m

31
Q

How do solvent molecules behave in biological processes

A

They go from diluted solution to more concentrated one. But there is semi-permeable membrane that allows solvent molecules to pass but not solute ones

32
Q

What is osmosis

A

Flux of solvent molecules from less concentrated splution to more concentrated one

33
Q

What is osmotic pressure(п)

A

External pressure that must be applied to prevent passing through the membrane

34
Q

What is formula for osmotic pressure

A

П=MRT
R=0.082 L×atm/K×mol=(Pa) 8314.51

35
Q

How are solutions defined based on osmotic pressure

A

•isotonic-2 solutions have same concentration and same п
•when they dont have same conc. and have different п the more conc. is hypertonic and less is hypotonic

36
Q

How do we convert mmHg to atm and atm to Pa

A

Number of mmHg/760mmHg=atm
Number in atm×101325=Pa(1atm=101325 Pa)

37
Q

How to convert from C to K

A

Just add 273.15

38
Q

What is different in formulas for electrolytic compounds

A

Because they generate more particles, we use i-van’t Hoff favtor.
i=number of particles after dissociation/number of formula units before dissociation
П=iMRT
DeltaTb=i×Kb×m
Delta Tf=i×Kf×m

39
Q

Formula for total number of particles

A

i=1+a(z-1)

40
Q

What is difference between expected and real number of particles

A

When substance doesnt dissolve completly, we have expected and experimental(real) values
Expected: i=number of particles after dissociation/ formula units
Experimental: i=1+a(z-1)
z=number of ions. It can be also determined through п=iMRT

Inorganic Chem (9 decks)

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