- do not fully disassociate (separate) into their component ions - are weak electrolytes

- are acids that contain two acidic protons (ex H2SO4 has 2 H+, AKA acidic protons) - every 1 mole of diprotic acid can react with 2 moles of OH- instead of just one - similarly, acids with three acidic protons (ex H3PO4) can react as 1 mole of acid to 3 moles of OH-

- on the reactants side - is the acid after donating a proton, thus becoming a base itself

- on the reactants side - is the base after accepting a proton, thus becoming an acid

- what goes into the buret for titration - concentration is always known

- an acid-base indicator - turns pink in basic solution - goes into the analyte solution

quiz 8 Flashcards by Maya T

molarity equation

moles (of solute)/liters (of solution)

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dilution equation

M1V1=M2V2

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arrhenius definition of acids

chemicals that increase the concentration of H+ (protons)

ex: HCl

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arrhenius definition of bases

chemicals that increase the concentration of OH-

ex: NaOH

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a solution is acidic if

it has more moles of acid than base, which means its pH is less than 7

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a solution is basic if

it has more moles of base than acid, which means its pH is greater than 7

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a solution is neutral if

it has an equal number of moles of acid and moles of base, meaning that its pH is exactly 7

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bronsted-lowry definition of acids

chemicals that donate protons, AKA proton donors

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bronsted-lowry definition of bases

chemicals that accept protons, AKA proton acceptors

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H+ vs H3O+

they mean the same thing

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strong acids

fully disassociate (separate) into their component ions, aka complete ionization
are strong electrolytes

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weak acids

do not fully disassociate (separate) into their component ions
are weak electrolytes

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strong bases

full disassociate (separate) into their component ions, AKA complete ionization

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weak bases

-do not fully disassociate (separate) into their component ions

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true or false, water reacts with itself in an acid-base reaction

true, this is self-ionization

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value of [H3O+] and [OH-] in pure water

both 10^-7 M

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diprotic acids

are acids that contain two acidic protons (ex H2SO4 has 2 H+, AKA acidic protons)
every 1 mole of diprotic acid can react with 2 moles of OH- instead of just one
similarly, acids with three acidic protons (ex H3PO4) can react as 1 mole of acid to 3 moles of OH-

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buffer solution

resists change in pH and keeps pH level constant

- is created by making a solution where moles of weak acid and moles of conjugate base are present in 1 to 1 ratio

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conjugate base

on the reactants side

- is the acid after donating a proton, thus becoming a base itself

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conjugate acid

on the reactants side

- is the base after accepting a proton, thus becoming an acid

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how to use a burette

amount dispensed = final volume - initial volume

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titrant

what goes into the buret for titration

- concentration is always known

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analyte

what is in the beaker during titration

-concentration is always unknown, to be determined from the titration experiment

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phenolphthalein

an acid-base indicator
turns pink in basic solution
goes into the analyte solution

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once a reversible reaction reaches equilibrium, what happens to the rate of the forward reaction and rate of reverse reaction?

they become equal

once a reversible reaction reaches equilibrium, what happens to the concentration of reactants and products?

- both concentrations become stable | - but [reactants] does not always equal [products]

in a reversible reaction, when is the rate for the forward reaction the fastest and slowest?

- fastest at the very beginning | - slowest at equilibrium

when is the rate for the reverse reaction the fastest?

-at equilibrium

equilibrium can only be achieved when

1. the reaction is reversible 2. the reaction takes place in a closed system 3. none of the chemical compounds precipitate as a solid

equilibrium constant

- Keq=[products]/[reactants]=([C]^c*[D]^d)/([A]^a*[B]^b) when aA + bB cC + dD (lowercase are coefficients, uppercase are reactants/products) - only take the concentrations of aq solutions and gases, and exclude solids and liquids

at what Keq does the reaction become irreversible?

- at Keq>10^10 | - this means that it's 0% reactant, 100% product

at what Keq does the reaction become NO reaction?

at Keq<10^-10 | -this means that it's 100% reactant, 0% product

le chatelier's principle

when a chemical system at equilibrium is disturbed, the system shifts in a direction that minimizes the disturbance

ways to disturb an equilibrium

1. change the concentration of one of the chemicals involved 2. change the temperature 3. change the volume of the system

what change in concentration would make a system shift to the left?

- adding product | - removing reactant

what change in concentration would make a system shift to the right?

- adding reactant | - removing product

what change in temperature would shift a system to the left?

- adding energy to an exothermic reaction | - removing energy from an endothermic reaction

what change in temperature would shift a system to the right?

- adding energy to an endothermic reaction | - removing energy from an exothermic reaction

when volume is decreased in an equilibrium system,

reaction wants to shrink, and therefor shifts to the side with less volume

when volume is increased in an equilibrium system,

reaction wants to expand, and therefor shifts to the side with more volume

why do combustion reactions not immediately occur (without the assistance of energy)?

because all reactions have a required activation energy/barrier

how to overcome the activation energy/barrier

either - raise the temperature - use a catalyst

a catalyst

lowers the height of the activation barrier/energy

enzymes

are biological catalysts

- a way to express the concentration of H30+ - pH less than 7 is acidic - pH of 7 is pure water - pH greater than 7 is basic

when calculating pH

- the SF in [H3O+] is the # of decimal places for your pH level - in reverse, the # of DP in your pH level gives you the # of SF in your concentration

list of strong acids

- HCl - HBr - HI - HClO4 - HNO3 - H2SO4

list of weak acids

-HF -HC2H3O2 -H2CO2 -H2CO3 -H2SO3 H3PO4

list of strong bases

anything that contains OH and is soluble

list of weak bases

- NH3 - C5H5N - CH3NH2 - CH3CH2NH2 - HCO3-

oxidation state of elemental compound

always zero

oxidation state of ion

equal to its charge

relationship between sum of oxidation states and net charge of a molecule

they are equal | ex: h20 net charge is 0, and sum of its oxidation states is 0

oxidation state of alkali metals

oxidation state of group alkaline earth metals

oxidation state of fluorine

-1

oxidation state of hydrogen

+1, with exceptions like LiH, NaH, CaH2 (oxidation state of group 1 & 2 metals take precedent)

oxidation state of oxygen

-2

oxidation state of halides

-1

oxidation state of sulfur and its group members

-2

oxidation state of nitrogen and its group members

-3

order of precedence for H, O, F oxidation states

FHO

mnemonic for oxidation and reduction

LEO the lion goes GER LEO: Loss of Electrons is Oxidation GER: Gain of Electrons is Reduction

half reaction method

write out net ionic equation, then separate into reduction half reaction and oxidation half reaction and add electrons to each accordingly. then (if necessary) multiply each by an integer to make the # of electrons on each side of the "complete" reaction equal

quiz 8 Flashcards

(64 cards)