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MCAT Prep > Solutions and Solubility > Flashcards

Solutions and Solubility Flashcards

1
Q

solution

A

a homogenous mixture

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2
Q

homogenous mixture

A

has uniform composition

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3
Q

What are MCAT solutions generally?

A

solids dissolved in liquids

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4
Q

Saturation and units

A

how much solute is dissolved

g/L

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5
Q

When will a precipitate form?

A

adding more solute to an already saturated solution

or decreasing the solubility of a solution

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6
Q

When is a solution saturated?

A

a solution is saturated when concentrations of reactants are equal to Ksp

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7
Q

Ways to decrease the solubility of a solution?

A

through the common ion effect or by changing temperature/pressure

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8
Q

Do most dissolutions change temperature or pressure?

A

yes. most solutions are endothermic and require heat, which lowers the environment’s temp.

Most dissolutions also increase pressure.

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9
Q

supersaturated

A

more than max solute is dissolved in solution

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10
Q

electrolyte

A

ions in solution that can conduct electricity

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11
Q

What does a higher temperature do to solubility of an ionic compound?

A

increases solubility

most dissolutions are endothermic and require heat

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12
Q

What does a lower temperature do to solubility of an ionic compound?

A

decreases solubility

most dissolutions are endothermic and require heat

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13
Q

Relationship between solubility of a gas and temperature

A

Lower temperature makes the gas less soluble

Gas has less energy to escape the solution

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14
Q

Alkali metals solubility

A

always soluble in H2O

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15
Q

What molecules are always soluble?

A

nitrates, chlorates, and acetates

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16
Q

Halides solubility

A

always soluble unless with Ag, Pb or Hg

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17
Q

Halide atoms

A

F, Cl, Br, I

18
Q

SO4 2- solubility

A

always soluble expect with Ca, Sr or Ba

19
Q

What molecules are generally insoluble?

A

carbonates, phosphates, S2- and sulfates

except with alkali metals that are always soluble

20
Q

Are oxides generally soluble or insoluble?

A

generally insoluble

except for with Ca, Sr, Ba or alkali metals

21
Q

Molarity

A

M

moles of solute / liter of solution

22
Q

Molality

A

m

moles of solute / kg of solvent

23
Q

For water, one liter equals

A

one kilogram

24
Q

For water, one mL equals

A

one gram

25
Q

When do we use molality?

A

when discussing colligative properties

26
Q

colligative properties

A

properties changing solely with concentration of a solution

ex: adding salt to H2O lowers freezing point

27
Q

Normality

A

number of equivalents / liter of solution

28
Q

When do we use normality?

A

in acid-base chemistry

the equivalents are H+ or OH- ions

29
Q

How can we get molarity from normality of an acid?

A

N = M(acid) * H+ in acid molecule

30
Q

How can we get molarity from normality of a base?

A

N = M(base) * OH- in base molecule

31
Q

What does Ksp tell us?

A

how soluble something is

32
Q

Relationship between Ksp and solubility

A

higher Ksp = more soluble

33
Q

What is Ksp formula generally?

A

= [anions] [cations]

*solid reactant and pure water are not included in formula

34
Q

When Q>Ksp what happens?

A

a precipitant forms

maybe not right away, solution could be supersaturated for a little

35
Q

When saturated what rates are equal?

A

rates of dissolution and precipitation, ie. forward and reverse reactions

36
Q

common ion effect

A

solubility of an ionic species decreases when one of its component ions is already present in solution

37
Q

How does common ion effect theoretically work?

A

since some reactant is already present, less solute can dissolve before Ksp is reached

means that we have less solubility

shifts reaction towards the solid reactant

38
Q

Where do we see the common ion effect?

A

in acid base chemistry

ex: having a basic solution (more OH-), might make Pb(OH)2 less soluble

39
Q

Can you shift a dissolution towards the reactants?

A

sure

can use a coordination complex around a metal to remove ions from the solution

40
Q

Weak electrolyte

A

does not produce many ions when dissolved in solution

MCAT Prep (22 decks)

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