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Chemistry > Solution Chemistry > Flashcards

Solution Chemistry Flashcards

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1
Q

what terms describes the solubility of a solid or gas in a liquid

A

soluble and insoluble

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2
Q

what terms describes the solubility of a liquid in a liquid

A

miscible and immiscible

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3
Q

in what conditions are gases most soluble?

A

low temp high pressure

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4
Q

when are solid solutions most soluble?

A

in warm temperatures

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5
Q

alloys

A

a mixture of two or more metals. ex: sterling silver, brass

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6
Q

amalgam

A

a solid solution of metals that contains mercury

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7
Q

list things that solubility is dependent upon

A

temperature, pressure if a gas, chem. nature of the solute/solvent (polarity)

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8
Q

formula for molarity?

A

moles of solute/liters of solution

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9
Q

percent by mass formula?

A

mass of solute/mass of solution * 100

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10
Q

percent by volume formula?

A

volume of solute/volume of solution * 100

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11
Q

parts per million formula

A

grams of solute/grams of solution * (1x10^8)

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12
Q

colligative properties

A
  • only applied to solutions
  • depends only on the ratio between solute and solvent, not the kind of solute
  • the more particles in the solution the greater the temperature change
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13
Q

why does the difference between FP and BP increase with the amount of solute added?

A

because the solute particles decrease vapor pressure and get in the way of the solute’s particles during freezing

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14
Q

formula for change in boiling/freezing point temperature

A

change in T = ikm, where k is altered for boiling or freezing

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15
Q

what does k (b) mean in the change in BP/FP formulas?

A

constant for the solute

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16
Q

what is water’s k value for BP?

A

0.52

17
Q

what is water’s k value for FP?

A

1.86

18
Q

what is i in the change in temperature formulas?

A

the van’t hoff factor, the number of ions per formula unit if the solute is an ionic substance. Polyatomic ions are counted as one ion.

19
Q

the actual value for change in temperature is usually ______ than the expected value because _______________

A

lower, because at any point in time, some of the ions in the solution will be paired

20
Q

molality formula

A

moles of solute/kg of SOLVENT

21
Q

electrolytes

A

a substance, which when dissolved in water is able to conduct electricity

22
Q

what do strong electrolytes do?

A

they dissociate completely

23
Q

what are the parameters for conducting electricity

A

you must have something that moves and carries a charge

24
Q

what do weak electrolytes do?

A

they only dissociate slightly, therefore mostly staying together

25
Q

complete ionic equation

A

separation of aqueous solutions into positive and negative ions, putting coefficients in front

26
Q

net ionic equation

A

only keep the ions that make the solid, liquid, or gaseous product on the reactant side and only keep that product on the other side (none of the aqueous components)

27
Q

formula for dilutions

A

M of initial * Volume of initial = M of final * V of final

28
Q

in dilutions, should the final molarity be smaller or greater than the original

A

smaller, because you are DILUTING IT

29
Q

explain how to do a dilution in the lab

A
  • do the math
  • add like 20 ml of water into a volumetric flash
  • add in the calculated amount of stock solution
  • stir then cool (most of these are exothermic)
  • add deionized water to graduated marking
30
Q

calculations for making a solution from a solid reactant?

A

still us MV = MV but convert to grams where needed

31
Q

procedure for making a solution from solid reactant

A
  • calculations
  • add deionized water in flask, a small amount
  • measure out solute and add to flask
  • heat/stir to dissolve
  • cool to room temperature and add deionized water to the mark

Chemistry (17 decks)

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