chapter 4-6 Flashcards by Sam Rocke

Q

solvent

A

able to dissolve other substances

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Q

solute

A

dissolved in the solvent

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Q

molarity

A

moles/liter

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Q

equivalence point

A

perfect neutralization attained

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Q

end point

A

where indicator changes color

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Q

analyte

A

something is unknown

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Q

titrant

A

molarity and volume precisely known

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Q

oxidation

A

loss of electrons; more positive

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Q

reduction

A

gain of electron; more negative

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Q

oxidizing agent

A

electron acceptor

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Q

reducing agent

A

electron donor

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Q

density equation

A

D=PM/RT=m/V

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Q

bronsted-lowry definition of acid/base

A

acid is a proton donor; base is a proton acceptor

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Q

arrhenius definition of acid/base

A

acid produces H+; base produces OH-

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Q

solubility of nitrate salts

A

most are soluble

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Q

solubility of alkali metals

A

soluble

Q

solubility of ammonium ions

A

soluble

Q

solubility of chloride

A

soluble

Q

solubility of bromide

A

soluble

Q

solubility of iodide

A

soluble

Q

solubility of Ag+

A

insoluble

Q

solubility of Pb2+

A

insoluble

Q

solubility of Hg2^2+

A

soluble

Q

solubility of sulfate salts

A

soluble

solubility of BaSO4

not soluble

solubility of PbSO4

not soluble

solubility of Hg2SO4

not soluble

solubility of CaSO4

not soluble

solubility of hydroxides

only slightly soluble

solubility of NaOH

soluble

solubility of KOH

soluble

solubility of sulfide

only slightly soluble

solubility of carbonate

only slightly soluble

solubility of chromate

only slightly soluble

solubility of phosphate

only slightly soluble

Average kinetic energy equations

1/2mv^2 OR 3/2RT

root mean square velocity equation

root(3RT/M)

rate of effusion

higher for lower molar mass root of M1/Root of M2