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

Q

solubility of BaSO4

A

not soluble

Q

solubility of PbSO4

A

not soluble

Q

solubility of Hg2SO4

A

not soluble

Q

solubility of CaSO4

A

not soluble

Q

solubility of hydroxides

A

only slightly soluble

Q

solubility of NaOH

A

soluble

Q

solubility of KOH

A

soluble

Q

solubility of sulfide

A

only slightly soluble

Q

solubility of carbonate

A

only slightly soluble

Q

solubility of chromate

A

only slightly soluble

Q

solubility of phosphate

A

only slightly soluble

Q

Average kinetic energy equations

A

1/2mv^2 OR 3/2RT

Q

root mean square velocity equation

A

root(3RT/M)

Q

rate of effusion

A

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