Needs a New Boy - super negative and has a lot of baggage (electrons) - looking for positive charge to balance her out - she is a lewis base because will provide electrons to the positive electrophile

Acids/Bases Flashcards by Lindsey Young

bicarbonate

base HCO3-

when added to something that is acidic, will increase pH to become more basic because HCO3- consumes H+

H+ + HCO3- H2CO3 H2O + CO2

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ksp

solubility product constant

the products are multiplied together. If that concentration exceeds the ksp, they will also form a precipitate because ksp represents the limit of solubility. Everything under ksp value will be dissolved, everything over becomes solid

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How does the stability of the conjugate base affect acidity?

conjugate bases made from smaller halogens will be less stables because a smaller radius has less surface area to spread out the charge (thus stabilize)

therefore while fluorine is the most electronegative, it will form a short, strong bond with H that is not acidic (wants to keep H)

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What determines acidity of functional group?

more electronegative atoms are more acidic

ability to stabilize negative charge through charge distribution (atom size) or delocalization (resonance)

more acidic protons will be the first to deprotonate as pH increases

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What is more acidic alkene, alkane, or ketone?

ketones are less acidic than alcohols, but more acidic than hydrocarbons. The negative charge in the conjugate base of a ketone is delocalized by resonance across the alpha carbon and carbonyl oxygen atoms, which helps stabilize the charge

alkene proteins (sp2 C-H) are more acidic than alkane proteins (sp3 C-H)

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What is more acidic, primary or secondary alcohol?

a primary alcohol is more acidic which contributes to their enhanced ability to react because deprotonation by a base makes the alcohol a better nucleophile

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nucleophile

Needs a New Boy

super negative and has a lot of baggage (electrons)
looking for positive charge to balance her out
she is a lewis base because will provide electrons to the positive electrophile

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electrophile

Electron loving
positive - wants to accept electrons
Lewis acid

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How do acids affect nucleophiles?

nucleophiles are out looking for protons to make her happy because she is so negative.
acids come along and donate their H+ to nucleophile which is a bronsted base (accepts protons)

because already has a proton, will not actively search for more, reducing the nucleophilicity of the molecule

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indicators

determine endpoint by changing color during titration to signal close to equivalence point (when the acid and base are equal amounts)

one color represents low pH and another color represents high pH

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buffers

region that will not have a large change in pH
weak acid + conjugate base or weak base + conjugate acid (or salt)

need weak acid or base so it doesn’t completely dissociate. acids donate protons and bases accept them so work together to resist changes in pH

buffering zones are horizontal on a titration curve - point of inflection

buffering zone = 1/2 [weak acid/base]

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NH3

ammonium

weak base

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strong acids

HClO4
HI
HBr
H2SO4
HCl
HNO3
H3O+ or H+

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perchloric acid

HClO4

strong acid

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hydrochloric acid

HCl

strong acid

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sulfuric acid

H2SO4

strong acid

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nitric acid

HNO3

strong acid

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acidic in nature

the more oxidated something is, the more acidic

ex: CO2 is surrounded by oxygen and is like breaking pure acid

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strong bases

LiOH
NaOH
KOH
Ca(OH)2
Ba(OH)2
Sr(OH)2
CsOH
RbOH

strong bases completely dissociate in solutions because the conjugate acid cation is very stable

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weak acids

HCOOH (formic acid)
CH3COOH (acetic acid)
HF (hydrofluoric acid)
HCN (cyanide)
H2S (hydrogen sulfide)
H2O (water)

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weak bases

NH3 (ammonium)
NR3 (amine)
C5H5N (pyridine)
NH4OH (ammonium hydroxide)
H2O (water)

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neutralization

acid + base –> salt + water

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equivalence point

vertical line where [base]=[acid] - neutralized

amount of equivalence points is dependent on number of acidic protons (H+) - polyprotic acids have multiple pKas

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strong base + strong acid

Study These Flashcards

equivalence point is pH 7

strong base + weak acid

equivalence point at higher pH than 7

strong acid + weak base

equivalence point lower than pH 7

titration

technique to determine the concentration of an unknown solution use a known concentration and slowly add to unknown solution with known volume and use indicator to see change

polyprotic acids

have more than one acidic proton the number of acidic protons will be the number of equivalence points adding strong base will neutralize and remove protons in stepwise fashion

How to tell acidic protons

acidic protons are attached to functional groups with low pKa values ``` acidic --> basic H-X R-H-O-H+ R-NH3+ carboxylic acid phenol alcohol SP amine SP2 SP3 ``` look for protons on electronegative atoms first --> O, N, S

the most stable conjugate base will be

the strongest acid

oxyacid

acid that contains a hydrogen, oxygen, and another element HClO dissolves in water and creates acidic solution ex: HClO + H2O --> H30+ + ClO-

oxides

oxygen and another element ex: SO2

arrhenius acid

H+ donor HA --> H+ + A-

arrhenius base

OH- donor BOH --> B+ + OH-

Bronsted-Lowry acid

H+ donor

Bronsted-Lowry base

H+ acceptor

Lewis acid

electron acceptor aka electrophile

Lewis base

electron donor aka nucleophile

water as an acid or base

water is amphoteric - can act as either acid or base will act a certain way depending on conditions in basic conditions acts a s a base

ionization

complete loss of electrons left with just an ion M --> M+ + e-

NO2-

nitrite

NO3-

nitrate

NO4-

peroxynitrate

nitroxide

SO3^(2-)

sulfite

SO4^(2-)

sulfate

PO4(3-)

phosphate

PO3(3-)

phosphite

ClO3-

chlorate

ClO2-

chlorite

HCO3-

bicarbonate bi = single Hydrogen atom

HSO4-

bisulfate

H2PO4-

dihydrogen phosphate di = two hydrogen atoms

ferrous

Fe2+ ous = lower charge for metal

ferric

Fe3+ ic = higher charge for metal

neutralization

acid + base --> salt + H20 can figure out how much is needed by using NacidVacid=NbaseVbase N= normalities = number of grams/volume V=volume so this can be thought of as moles acid = moles base

What makes a strong Lewis acid?

smaller ionic radius and strong positive charge

Why is the conjugate base a better nucleophile than the acid?

because the conjugate base has more electron density due to the negative charge

Acids/Bases Flashcards

(58 cards)