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grade 11 > chem - solutions > Flashcards

chem - solutions Flashcards

1
Q

what is a solute

A

the substance that dissolves in a solution

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2
Q

what is a solvent

A

the substance that dissolves a solute to form a solution

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3
Q

what is a solution

A

a uniform mixture that may contain solids, liquids, or gases. Made up of at least one solute and one solvent.

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4
Q

define homogenous

A

a mixture that has a uniform composition throughout and always has a single phase. (all solutions are homogenous mixtures)

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5
Q

define heterogenous

A

a mixture that does not have uniform composition

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6
Q

name the 9 types of solutions, give examples of each

A

G + G (N2 + O2 = air)
G + L (air + H2O = moist air)
G + S (air+ charcoal = charcoal filter)
L + G (H2O + CO2 = carbonated water)
L + L (H2O + ethylene glycol = antifreeze)
L + S (H2O + Na = saltwater)
S + G (C + poisonous gas = charcoal filter)
S + L (Ag + Hg = tooth filling)
S + S (Cu + Zn = brass)

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7
Q

define electronegativity

A

the relative ability of an elements atoms to attract electrons in a chemical bond.

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8
Q

define polarity

A

the positive or negative charge of an atom

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9
Q

describe what a polar water molecule would look like

A

h are +ve, o is -ve

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10
Q

in a water molecule, which element is more electronegative?

A

oxygen

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11
Q

what is the difference between soluble and insoluble

A

soluble- can be dissolved

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12
Q

what is the difference between miscible and immiscible

A

miscible- liquid that can be dissolved

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13
Q

describe the dissolving process of an ionically bonded substance, at an atomic level.

A

salt -> h of h2o surrounds cl-, o of h2o surrounds na+

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14
Q

what is solvation?

A

the process in which solvent particles are pulled into a sphere around solute particles, causing the solute to be hidden from view

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15
Q

what is hydration?

A

solvation but with water as the solvent

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16
Q

describe the dissolving process of a covalently bonded substance, at an atomic level

A

solvent surrounds each solute molecule, covalent bonds are too strong to be broken

17
Q

define exothermic

A

when a solute dissolves in a solvent and the overall solution increases in temperature. This is because the forming of bonds gave off more energy than the breaking of the initial bonds

18
Q

define endothermic

A

when a solute dissolves in a solvent and the overall solution decreases in temperature. This is because the breaking of the initial bonds required more energy than the forming of the bonds gave off

19
Q

what type of bond forms electrolyte solutions?

A

ionic

20
Q

what type of bond releases positive and negative ions when dissolved?

A

ionic

21
Q

what is a dipole?

A

the separation of a charge in a polar molecule

22
Q

what is a non-polar substance? Give an example.

A

a molecule with atoms of similar electronegativities, does not have specifically charged poles. (ex. oil)

23
Q

list what happens with each possible solution of polar and non-polar substances.

A
  1. both polar: Polar attraction, solution possible.
  2. polar solvent and nonpolar solute: Polar particles attracted to each other only, solution unlikely.
  3. nonpolar solvent and polar solute: same as above
  4. both nonpolar: some may dissolve, solution possible
24
Q

like dissolves like.

A

like dissolves like.

25
Q

what is dynamic solution equilibrium

A

the point where ions are entering the solution at the same rate as they are leaving it.

26
Q

name the 3 factors affecting the rate of solution for solids

A

surface area, temperature, agitation

27
Q

why is temperature a factor in dissolving solids?

A

process is endothermic (requires heat)

28
Q

what happens when you increase temperature while dissolving a gas?

A

rate of dissolving goes down because solvation of gasses is usually exothermic (gives off heat)

29
Q

what is Henry’s Law

A

The mass of a gas solute dissolved in a liquid is proportional to the pressure of the system.

30
Q

What is the effect of pressure on solvation?

A

increases if its a gas, not much if its a solid or liquid

31
Q

what is concentration

A

the amount of solute in a given amount of solution, measured usually in g/L or mol/L

32
Q

what is molarity? What are the 3 ways of expressing it?

A

concentration of moles, expressed as “M”, “C” or “[…]”

33
Q

list the 6 steps for preparing a stock solution

A
  1. determine number of moles of solute
  2. convert to grams
  3. measure out that many grams
  4. dissolve required mass in slightly less than the required volume of solvent to allow for more precision
  5. transfer to a volumetric flask of the exact volume needed
  6. use a dropper pipette to finish dilution by adding the perfect amount of solvent

grade 11 (3 decks)

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