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Chem 104 > Unit 4 > Flashcards

Unit 4 Flashcards

1
Q

Solutions:

A

homogenous mixtures of two or more substances

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2
Q

Solvent

A

A compound of a solution that is present in the greatest amount

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3
Q

Solute

A

Any component in a solution other than the solvent (i.e, the other ingredients in the mixture)

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4
Q

How is a solution made?

A

By dissolving a solute in a solvent (solute is added to the solvent)

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5
Q

How are solutions described qualitatively?

A

As concentrated or dilute

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6
Q

Concentrated solutions…

A

have a large amount of solute compared to solvent

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7
Q

Dilute solutions…

A

have a small amount of solute compared to solvent

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8
Q

Saturated solution

A

a solution that contains the maximum concentration of a solute possible at a given temperature

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9
Q

Unsaturated solution

A
  • a solution that contains less than the maximum concentration of a solute possible at a given temperature
  • can dissolve more of the solute into the solution
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10
Q

Supersaturated solution:

A

a solution containing more than the maximum quantity of solute predicted to be soluble in a given volume of solution at a given temperature

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11
Q

Concentration units

PPM

A
  • grams of solute per million grams of solution
  • =grams of solute/grams of solution (all times 10^6)
  • OR mg of solute/kg of solution
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12
Q

PPB

A
  • grams of solute per billion grams of solution
  • ppb=grams of solute/grams of solution (all times 10^9)
  • OR micrograms of solute/kg of solution
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13
Q

How to find the amount of solute (moles or grams) in a given voume of solution?

A

Use molarity

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14
Q

Molarity formula

A

Molarity=# of moles of solute/# of L of solution

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15
Q

molarity formula rearranged

number of moles solute=?

A

(molarity)(# liters of solution)

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16
Q

Beer’s law

A

absorbance=molar absorptivity x path length x concentration of absorbing species

intensity of color can be used to measure concentrations

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17
Q

A (in Beer’s law)

A

absorbance (amount of light absorbed by sample)

18
Q

E (in beer’s law)

A

molar absorptivity

19
Q

b (in beer’s law)

A

path length

20
Q

c (in beer’s law)

A

concentration of absorbing species

21
Q

Stock solution

A

a concentrated solution of a substance used to prepare solution of lower concentration

22
Q

Dilution

A

the process of lowering the concentration of a solution by adding more solvent

23
Q

Ionic Theory of Solutions

A
  • proposed by Arrhenius to account for the electrical conductivity of water
  • proposed that certain substances produce freely moving ions when they dissolve in water, and these ions conduct electric current in an aqueous solution
24
Q

Electrolytes

A
  • An electrolye dissolves in water to give an electrically conducting solution
  • most ionic solids dissolve in water
  • ions in previously fixed states are free to move about, forming an electric current
25
Q

Strong electrolyte properties

A
  • Total dissociation
  • Efficient conductivity
  • Includes strong acids, strong bases, and soluble salts
26
Q

Weak Electrolyte

A
  • Partial dissociation
  • Slight conductivity
  • Weak acids and week bases
27
Q

Nonelectrolyte

A
  • no dissociation
  • n/a conductivity
  • includes molecular compounds
28
Q

Ionic compounds in solution

A
  • When an ionic compound is dissolved into solution, the molarity for each ion is based on how many ions there were in the salt
  • For example, in an aqueous solution that is 0.1M NaCl, your solution will have 0.1M Na+ ions and 0.1M Cl- ions based on the 1:1:1 mole ratio.
  • But if you have an aqueous solutio that is 0.1M Na2SO4, your solution will have 0.2M Na+ ions and 0.1M SO4 ions based on the 1:2:1 mole ratio.
29
Q

H+ ions strongly associated with water molecules form…

A

Hydronium ions (H30+)

30
Q

Acids

A

proton (H+ donors)

31
Q

Bases

A

Proton acceptors

32
Q

Neutralization

A

reaction that takes place when an acid reacts with a base a produces a solution of a salt in water

33
Q

Salt

A
  • product of a neutralization reaction
  • made up of the cation of the base plus the anion of the acid
34
Q

amphiprotic

A

acts as acid or base (ex. water)

35
Q

Titration

A

an analytical method to determine the concentration of a solute in a sample by reacting it with a standard solution

36
Q

Standard solution

A

a solution of known concentration (also called the titrant)

37
Q

Equivalence point

A

point when moles of added titrant is stoichiomerically equivalent to moles of substance being analyzed

38
Q

End point

A

point reached when the indicator changes color

39
Q

Precipitation

A

combining an insoluable cation with an insoluable anion forms a precipitate

40
Q

Oxidation

A

loss of electrons

41
Q

reduction

A

gain of electrons

42
Q

Redox reactions

A

transfer of electrons

Chem 104 (20 decks)

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