Exam 3 prep Flashcards by Faith Kalsow

solute

present in lesser amount

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solvent

present in greater amount

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Electrolytes

can conduct electricity (ions), dissociate 100%

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nonelectrolytes

doesn’t produce ions

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Diatomic particles

I2, F2, Cl2, Br2

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1 Eq

1,000 mEq

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Solubility

g of solute/100 g water

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gas solubility

solubility decreases as temperature increases

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concentration of a solution

Amount of solute/amount of solution

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Mass percent

mass of solute/mass of solution

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Volume percent

volume of solute/volume of solution * 100%

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mass/volume percent

mass of solute/volume of solution * 100%

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Molarity

moles of solute/liter of solution

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Dilution

water is added

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Solute concentrations

C1V1= C2V2 (M1V1-M2V2)

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Solutions

transparent, do not separate

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Colloids

cannot be filtered, separated by semipermeable membrane

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Suspension

particles settle rapidly, can be separated by filters

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solute + water

boiling point increases, freezing point decreases, vapor pressure decreases

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boiling point elevation

change in temperature= molarity * boiling point * number of particles in solution

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Freezing point depression

change in temperature at freezing point=molarity * Kf * number of particles in solution

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Osmosis

Water(solvent) flows from a lower to a higher solute concentration

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Tonicity

Concentration of a solution and how it compares to another solution

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Isotonic Solution

two solutions that have the same concentration as each other

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Hypotonic solution

the less concentrated solution

Hypertonic solution

the more concentrated solution

Dialysis

diffusion of small solute particles across a dialysis membrane

3 things that have to occur for a reaction

collision, orientation, and energy

Activation Energy

the minimum amount of energy needed to convert the colliding molecules into products

Rate of reaction equation

Change in products/change in time

Rate of reaction is affected by

temperature, concentration, catalyst

pressure

only affects rate of reaction for gasses

At equilibrium

rate of forward reaction is equal to rate of reverse reaction, the forward and reverse reactions continue at the same rate

Kc=

products/ reactants

a reaction at a specific temperature...

can only have one value of Kc

small Kc

mostly reactants

Kc=1

at equilibrium (reactants = products)

Large Kc

mostly products

Effect of catalyst on equilibrium

does not change the equilibrium mixture

volume on K

only affects gasses

Arrhenius Acids

Produce hydrogen ions when dissolved in water

acids with hydrogen ion and nonmetal ion naming

hydro prefix and end with ic acid

Acid with hydrogen ion and polyatomic ion naming

ate to ic acid ite to ous acid

Arrhenius bases

produced hydroxide ions in water

naming bases

add hydroxide to the end

Acid characteristics

produces H+, electrolytes, sour, sting, red, colorless

Bases characteristics

produces OH, electrolytes, bitter/chalky, soapy/slippery, blue, pink

Bronsted-lowry definition of acid

donates a proton

Bronsted-lowry definition of base

accept a proton

Amphoteric substances

can act as both acids and bases

strong acid 1

HNO3

Strong acid 2

H2SO4

Strong acid 3

HClO4

String acid 4

HCl

Strong acid 5

HBr

Strong acid 6

Strong Base 1

LiOH

Strong base 2

NaOH

strong base 3

KOH

Strong base 4

Ca(OH)2

Strong base 5

Sr(OH)2

Strong base 6

Ba(OH)2

Strong base 7

Rb and CsOH