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Chemistry > Solutions and solubility > Flashcards

Solutions and solubility Flashcards

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1
Q

What is a solution

A

A homogenous mixture of 2 or more substances
Remains fuly mixed in same perportions
Liquid and gaseous solutions are transparent
solutions can be coloured or not

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2
Q

What is a solvent

A

any substance that has another substance dissolved in it.
It is the substance that is present in the largest amt

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3
Q

What is concentration

A

describes the ration of the quantity of solute to the quantity of solvent or solution

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4
Q

solid solid solution ex

A

alloys like
copper nickel

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5
Q

Solid liquid solution ex

A

sea water, salt and water

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6
Q

solid and gas solution ex

A

mothballs

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7
Q

liquid and solid solution ex

A

mercury and silver

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8
Q

Factors that affect the dissolving process (3)

A

Temp - for solid solutes they dissolve faster at higher temp
agitation - brings fresh solvent into contact with solute
lump or powder - size of particles changes rate of dissolve

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9
Q

How to write a dissociation equation

A

use only for ionic comp
solid on left ions it releases on right
do not include water
Example:
K3PO4(s) -> 3K+(aq ) + PO43- (aq)

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10
Q

Why do some molecular compounds dissolve in water and others dont. what are they called

A

dissolves in water - some can form hydrogen bonds ex. Glucose - miscible
Do not dissolve in water ex oil, hydrocarbons, They are non polar

Acetic acid can dissolve in both

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11
Q

What is a surfactant

A

it encourages oil and water to mix
has long hydrocarbon tail and charged head
One side attracts water, the other oil
surfactant surrounds oil and allows the water to wash it away

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12
Q

What affects solubility (4)

A

temp
Molecule size
ion carge
pressure
measured in
g/100g H2O

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13
Q

How is solubility measured

A

g/100g H2O

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14
Q

How does molecule size affect solubility
which extreme is more soluebl

A

small molecules are often more soluble than larger ones
ex methanol and ethanol are more soluble than pentanol

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15
Q

How does the ion charge affect solubility
ex, group 1 metals are soluble, sulfides are not

A

compounds with ions of smaller charges are more soluble
because the charge increases the force that holds the ions togethor

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16
Q

How does the ion size affect solubility
which extreme is more soluble

A

Small ions bond more closely than large ions
bonds between smaller ions are stronger
compounds with smaller ions tend to be less soluble
Metals have smaller ions than non metals
size gets bigger down a period

17
Q

How does temperature affect solubility of solids gases and liquids

A

Solids - higher temp means more energy to break bonds
Gases - solubility of gases decreases with higher temp
liquid - temp does not affect solubility

18
Q

How does pressure affect solubility

A

Pressure does not have an affect on solid and liquid
Solubility of gas increases as pressure increases

19
Q

What are the degrees of saturation

A

Unsaturated - solution contains less than max quantity of solute
Saturated - solution contains max quantity of solute at a given temp
Supersaturated - Force a solution to siddlve more solute than it would normally.
(done by heating solution, dissolving solute then cooling)

20
Q

How do you calculate concentration using molar concentration

A

c = q of solute / q of solution
measured in mol/L
c = n/v
Always convert to Liters

21
Q

What is the dilution equation based off of c = n/v

A

C1V1 = C2V2
This is because when you dilute the solution the amt of moles stays the same.

22
Q

What is the dilution factor

A

The concentration of the diluted solution divided by the concentration of the concentration solution
C2/C1
Multiply V2 by the dilution factor and you get V1

23
Q

Qualitative analysis vs quant analysis

A

qual - the identification of the specific substances present
quant - the measurement of the quantity of a substance present

24
Q

How does sequential chemical analysis work

A

To determine whether an element is present or not, a compound could be added to form a precipitate.
If nothing happens then the element was not present. If a reaction occurs then it was
done in a flow chart manner.
the precipitation formula must be stated

25
Q

what colour do acids and bases turn with litmus paper test

A

acid - red
Base - blue

26
Q

What is arrhenius theory

A

Theory abt acids and bases when they were dissolved in water
suggested that both acids and bases ionize/dissociate in water
Acids have H and ionize in water and increase H+ concentration (PH)
Bases have OH and dissociate to increase OH - concentration

27
Q

What are the limitation of arrhenius theory (5)

A
  1. Water is often left out of the equation, it interacts with the molecules someway
  2. Free hydrogen ions do not exist in water
  3. Things like ammonia do not contain OH but are basic
  4. only works with aqueous things
  5. doesnt explain why salts with carbonate act basic
28
Q

What is the Bronsted lowry theory

A

Acid is substance where an H+ ion can be removed
A base is something that can remove an H+ ion from acid

29
Q

what are conjugate pairs

A

two molecules that differ because of the transfer of a proton
ex HCl and Cl

30
Q

How do you determine the strength of an acid

A

the concentration of H+ ions
If more than 99% ionizes when dissolving in water it is strong

31
Q

What are the strong acids (6)

A

HCl, HBr, HClO4, H2SO4, HNO3, HI

32
Q

Example of strong bases

A

Examples include oxides and hydroxides of Group 1 metals and Group 2 metals below beryllium

33
Q

Do bases ionize

A

Bases dissociate acids ionize

34
Q

How do you calculate PH

A

-log(H+ concentration)
or
-log(H3O+ concentration)

35
Q

What are the sigfig rules for PH calculation

A

The digit to the left of the decimal is not significant. Write the same amt of decimal places as there are sigfigs in the concentration

36
Q

what is the titrant in the titration

A

The solution in the burette, has a known concentration
is added to the unknown solution

37
Q

What is the analyte in a titration

A

the solution in the erlenmeyer flask, has unknown concentration

38
Q

Equivalence point vs endpoint

A

Equivalence - the point in a titration when the quantity of acid has exactly neutralized the quantity of base
Endpoint - the point during a titration in which an observable change (usually a colour change) caused by a significant change in pH has occurred, signifying that the equivalence point has been reached

39
Q
A

Chemistry (14 decks)

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