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Handout 1: States of Matter, Gases, Liquids and Phase transition > 2.1 > Flashcards

2.1 Flashcards

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1
Q

Solutions: what are mixtures?

A
  • most natural substances
  • have variable composition
  • retain component properties
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2
Q

what is a solution?

A
  • homogenous mixture (uniform distribution) of 2 or more substances in A SINGLE PHASE
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3
Q

Gas and solid solutions what happens?

A
  • gases completely miscible (be able to mix)

- gas dissolved in solid: occupies spaces in solid lattice eg. H2 in Pd

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4
Q

What is an alloy?

A

solid solution of metals ( a metal made by combining 2 or more metallic element)

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5
Q

true or false: substances with similar types of intermolecular forces will dissolve in each other

A

true

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6
Q

The solution process: what are the factors which determine whether a substance dissolves

A

enthalpy- exothermic favors dissolving

entropy- always favors solution formation ( solutions form naturally; not pure substances)

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7
Q

true or false: energy required to separate particles

A

true

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8
Q

true or false: energy released when particles mixed and new attractions form

A

true

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9
Q

What does delta H soln stand for?

A

Heat of solution: it = the total enthalpy change when solution forms from pure solvent and pure solute

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10
Q

What does forming a solution involve?

A
  1. ) solute particles separate - endothermic
  2. ) solvent particles separate - endothermic
  3. ) solute + solvent particles mix - exothermic
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11
Q

express delta H solution = ….

overall enthalpy change - reflection of strength of intermolecular attractions

A

delta H solution = delta H solvent + delta H solute + delta H mixture

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12
Q

What are the heats of solution measured by?

A

calorimeter

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13
Q

true or false: When the delta H solution is highly positive, it is likely that the solute is highly insoluble

A

true

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14
Q

What does hydration mean?

A

solvation in water

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15
Q

true or false: solvation of ions in water is always exothermic

A

true

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16
Q

delta H hydration =….

A

delta H h20solvent + delta H mix

17
Q

what is delta H hydration related to?

A
  • charge density of ion

- distance between ion and dipole

18
Q

why does the higher the charge the more negative the delta H of hydration?

A

water molecules can experience a greater magnitude and attraction to ion

19
Q

why does the smaller the ion the more negative the delta H of hydration

A

the closer the ions can come to the water

20
Q

What does lattice energy mean?

A

it is the amount of energy required to separate a solid ionic compound into GASEOUS IONS

21
Q

express delta H solution when ionic compound is dissolved in water

A

delta H soln = delta H solute + delta H hydration

22
Q

define solubility

A

maximum amount of solute THAT WILL dissolve in a solvent at a certain temperature

23
Q

What are solutions classified as?

A

saturated and supersaturated

24
Q

Define saturated

A

contains maximum quantity of dissolved solute in presence of solid( at that temperature) ; if we add anymore will not dissolve anything

25
Q

define super saturated

A

contains more solute than equilibrium amount of solute dissolved is unstable

26
Q

what happens to solutions at equilibrium?

A

for solid in solution with time:

rate of dissolving = rate of crystallization

27
Q

What are the factors which affect rate of dissolution

solvent molecules must make contact with solute

A

rate of dissolution increased by:

  • increasing surface area of solute (also stirring)
  • increase temperature
28
Q

definition of dissolution

A

is the process in which a solute forms a solution in a solvent

29
Q

true of false: most ionic solids are more soluble at higher solvent temperatures

A

true

30
Q

Does increasing the temperature usually increase the amount of solute that dissolves to give a saturated solution

A

yes

31
Q

what does henry’s law state

A

that the solubility of gas in liquid is proportional to gas pressure

32
Q

Express henry’s law

A

Sg= KhPg

33
Q

what does Sg mean?

A

solubility of gas in liquid (mol L-1)

34
Q

what does Kh mean?

A

henry’s constant (mol L-1 atm-1)

35
Q

what does Pg mean?

A

partial pressure of gas above solution (atm)

36
Q

the relationship of temperature and solubility

A

as solvent temperature increases, gas solubility decreases

think of cold water

Handout 1: States of Matter, Gases, Liquids and Phase transition (9 decks)

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