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solutions Flashcards

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1
Q

solution

A

homogeneous (1 phase mixture) even distribution of 1+ pure substance mixed together

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2
Q

solvent

A

present in the larger quantity
- substance that does the dissolving

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3
Q

solutes

A

present in the lesser quantity
- substance that gets dissolved in the solvent

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4
Q

aqueous solutions

A

indicates that water is the solvent and that you’re dealing with a solution

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5
Q

miscibility

A

2 liquids mix in any proportion
- “like dissolves like”

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6
Q

qualitative (empirical) proerties

A

electrolytic ability
litmus paper
solution colour
flame colour

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7
Q

ELECTROLYTES

A

ions in solution allow conductivity

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8
Q

NON-ELECTROLYTES

A

non-conductive molecular solute

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9
Q

acid has

A

H+
both red

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10
Q

base has

A

OH-
both blue

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11
Q

SOLUTION COLOUR

A

some ions have characteristic colour when dissolve in water. Allows for qualitative identification of the ion

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12
Q

what ions are aqueous

A

all ions are aqueous as ions only exist in water

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12
Q

FLAME TEST

A

some ions have a characteristic color of flame, when excited by an external heat source

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12
Q

svante arrhenius explaining solutions

A

dissolving
dissociation
ionization
low solubility

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13
Q

DISSOLVING

A

polar molecular solutes mix evenly into water by forming new IMF between the solute and solvent
- “like dissolves like”

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13
Q

DISSOCIATION

A

soluble ionic compounds break apart into individual ions in water.
- crystal lattice breaks
- explains the conductivity of ionic compounds (charged ions)

14
Q

IONIZATION

A

a special type of molecular compound with H+ or COOH-, H2O breaks the bond between the H and the rest of the molecule

15
Q

in ionization, what is the resulting product

A

an acid is now in water, making acid conductive from its charged ions

16
Q

LOW SOLUBILITY

A

non-polar molecular solute

17
Q

in any phase change or chemical reaction, the following sequence of events must occur

A
  • breaking reactive bonds (endo.)
  • forming product bonds (exo.)
18
Q

when forming a solution with bonds broken

A

solutes: ionic- cystal lattice must break
molecular- break IMF’s
solvents: IMF’s between water molecules

19
Q

when forming a solution with bonds forming

A

IMF’s between water and the solute

20
Q

what do we feel the net energy change as

A

we feel it as a change in temperature

21
Q

exothermic solution formation

A

solution gets hotter
reactants require less energy needed to break, products more energy released when forming

22
Q

endothermic solution formation

A

solution gets colder
reactants require more energy, less energy comes back in products

23
Q

why does the endothermic solution feel cold

A

from the lack of heat

24
Q

solution concentration

A

always measures the quantity of solute wihtin a specific quantity of solution

25
Q

solution concentraion formula

A

quantity of solution

26
Q

percent by mass (% m/m)

A

mass (g) of solute/ mass (g) of solution x 100%

27
Q

percent by volume (% v/v)

A

volume (mL) of solute/ mass (g) of solution x 100%

28
Q

percent mass by volume (% m/v)

A

mass (g) of solute/ volume (mL) x 100%

29
Q

parts per million (ppm)

A

mass (g) of solute/ mass (g) of solution x 100%

or

mass of solute (mg)/ volume of solution (L)

30
Q

what is the ppm formula for

A

very low concentrations

31
Q

amount concentration (c)

A

amount (mol)/ volume of solution (L)

32
Q

real life examples of solution concentrations

A

IV bag
toothpaste
sunscreen
vinegar
mouth wash
alcohol

33
Q

amount concentration AKA

A

molar concetration
molarity

34
Q

why is amount concentration the most useful type of concentration in chem

A

chemists need to know exact chemical amounts when solutions are used for chemical reactions and analytical techniques

Chem (10 decks)

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