Solutions and Solubility (5/10) Flashcards

1
Q

Solution definition

A

A homogeneous mixture

  • mixture: two substances
  • Homogeneous: evenly distributed
  • Heterogeneous: not evenly distributed (like a salad)
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2
Q

Dissoultion

A

Minority component (solute) reacts with solvent (majority component)

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3
Q

Dissolving

A

Like dissolves like

-polar amino acids dissolve most readily in polar solvents (like water)

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4
Q

Saturation

A

extent which solute is dissolved in solvent

-adding more solute than what solvent can handle to dissolve will precipitate

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5
Q

Supersaturation

A

Solute concentration>solute solubility

must heat and cool slowly to keep all dissolved. If not, crystallized

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6
Q

Electrolyte

A

Ions conduct electricity in a solution

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7
Q

higher temperature for solids

A

higher solubility in endothermic reactions

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8
Q

Higher temperature for gases

A

lowers solubility for gases

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9
Q

Solubility rules: alkali metals

A

All soluble in water

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10
Q

Solubility rules: Nitrates

A

All soluble in water

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11
Q

Solubility rules: Halides

A

soluble in water except when combined with silver, lead, or mercury

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12
Q

Solubility rules: Sulfates

A

Souble in water except when combined with calcium, silver, lead, etc

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13
Q

Solubility rules: Carbonate, phosphate, sulfide

A

Insoluble except when combined with sodium carbonate or ammonium phosphate

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14
Q

Solubility rules: Hydroxides and metal oxides

A

Insoluble except if combined with alkali metals

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15
Q

Molarity

A

moles of solute/Liters of solution

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16
Q

Molality

A

Moles of solute/Kg of solvent

17
Q

High concentration of solute

A

Impacts volume

Molarity does not equal molality

18
Q

Colligative properties

A

Properties changing solely with the concentration of solute in solution

19
Q

Normality

A

Equivalents of solute/ Liters of solution

20
Q

Calculating normality

A

(molarity of acid) x (acidic protons per molecule)

molarity of base) x (hydroxide ions per molecule

21
Q

Solubility equilibria

A

balance between reactant and balanced species

22
Q

Ksp expression

A

Product ions only

high value = large concentration of dissolved ions (high solubility)

23
Q

Insolubility

A

No compound is truly insoluble

24
Q

Molar solubility

A

Ksp/[cation] = [anion]

number of moles that need to dissolved for the solution to be saturated

25
A saturated aqueous solution when at equilibrium is...
The rates of dissolution and precipitation are equal
26
Common ion effect
solubility of an ionic species decreases when one of its component ions is already present in solution
27
Example of the common ion effect
AgCl --> Ag+ + Cl- external Cl- is the common ion which moves closer to saturation before Ag+ can dissolve because it takes up solvent so we decrease the solubility of Ag
28
Coordination complex
complex ion | takes external ions and adds them to something else to allow reactants to dissolve better