Calculate the following pH/pOH: - log[1M] = ? - log[1 x 10^-1 M] = ? - log[1 x 10^-2 M] = ? - log[1 x 10^-13 M] = ? - log[1 x 10^-14 M] = ?

- log[1M] = 0 - log[1 x 10^-1 M] = 1 - log[1 x 10^-2 M] = 2 - log[1 x 10^-13 M] = 13 - log[1 x 10^-14 M] = 14

Acids and Bases Flashcards by Monique Yuan

Arrhenius base

species that produces OH- in aqueous solution (hydroxide ions)

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Arrhenius acid

species that produces H+ (hydrogen ions) in aqueous solution

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An Arrhenius base can react with an Arrhenius acid in a/an ___________________ reaction.

neutralization

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What is a neutralization reaction?

acid + base –> water + salt

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Bronsted-Lowry acid

species that produces H+

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True or False: Bronsted-Lowry bases and acids are the same as Arrhenius bases and acids.

FALSE: Bronsted-Lowry ACIDS are the SAME as Arrhenius ACIDS (species that produces H+)…but Bronsted-Lowry BASES are different from Arrhenius BASES.

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Bronsted-Lowry Base

species that accepts H+

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When a Bronsted-Lowry acid _______ a proton, it forms a conjugate base.

When a Bronsted-Lowry base _______ a proton, it forms a conjugate acid.

acid LOSES proton

base GAINS proton

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Lewis acid

electron-pair acceptor

hint: lewis Acid = electron pair Acceptor

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Lewis base

electron-pair donor

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A Lewis acid is a/an:

a) electrophile
b) nucleophile

a) electrophile

hint: lewis Acid = electron pair Acceptor

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A Lewis base is a/an:

a) electrophile
b) nucleophile

b) nucleophile

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Which species is fundamental to understanding MCAT OCHEM?

a) Arrhenius
b) Bronsted-Lowry
c) Lewis

c) Lewis

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True or False: a given species cannot have multiple classifications (Arrhenius, Bronsted Lowry, Lewis).

FALSE

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List the strong acids (7).

HI (hydroiodic acid)
HBr (hydrobromic acid)
HCl (hydrochloric acid)
HNO3 (nitric acid)
HClO4 (perchloric acid)
HClO3 (chloric acid)
H2SO4 (sulfuric acid)

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List the strong bases (7).

NaOH (sodium hydroxide)
KOH (potassium hydroxide)
NH2- (amide ion)
H- (hydride ion)
Ca(OH)2 (calcium hydroxide)
Na2O (sodium oxide)
CaO (calcium oxide)

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What does the term “pH” refer to?

“potential of the hydrogen ion”

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how is pH defined in terms of the proton concentration? (provide equation)

pH = -log[H3O+]

hint: p = -log[whatever]

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How is pOH defined in terms of the hydroxide ion concentration? (provide equation)

pOH = -log[OH-]

hint: p = -log[whatever]

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pH + pOH = ?

pH + pOH = pKw = 14 (at room temperature)

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Calculate the following pH/pOH:

log[1M] = ?
log[1 x 10^-1 M] = ?
log[1 x 10^-2 M] = ?
log[1 x 10^-13 M] = ?
log[1 x 10^-14 M] = ?

log[1M] = 0
log[1 x 10^-1 M] = 1
log[1 x 10^-2 M] = 2
log[1 x 10^-13 M] = 13
log[1 x 10^-14 M] = 14

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Calculate the following:

\+log(1) = ?
\+log(3.2) = ?
\+log(10) = ?

\+log(1) = 0
\+log(3.2) = 0.5
\+log(10) = 1

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What is the pH of an aqueous solution of HCl with an initial concentration of 3.2 x 10^-5 M?

pH = -log(3.2 10^-5 M)

-log(10^-5M) = 5
\+log(3.2) = 0.5

pH = 5 - 0.5 =4.5

NOTE: SUBTRACT log of the mantissa

given the reaction below, what is the formula for the equilibrium constant (Kc)?

aA + bB –>/<– cC + dD

Kc = ( [C]^c [D]^d ) / ( [A]^a [B]^b )

Changes in which of the following influence(s) the equilibrium constant? Select all that apply: a) volume b) pressure c) temperature d) catalyst

c) temperature

TRUE OR FALSE: do NOT include pure liquids and gasses in the equilibrium constant calculation

TRUE

What does amphoteric mean?

can act as both and acid and a base

TRUE or FALSE: water is amphoteric

TRUE

What is the equilibrium equation for the self-ionization/autoionization of water?

H2O (acid) + H2O (base) -->/<-- HO- (conjugate base) + H3O+ (conjugate acid)

What is the equilibrium constant for the self-ionization of water?

Kw = [H3O+][OH-] = 1.00 x 10^-14 ....at 25C and 1 atm note: [H3O+] = [OH-] = 1.00 x 10^-7

Ka x Kb = ?

Ka x Kb = Kw = 10^-14

If Ka of a weak acid is greater than 10^-7 (e.g. 10^-6), its conjugate base will be __________. a) stronger b) weaker hint: consider the value of Ka x Kb (or Kw)

b) weaker

If Ka of a weak acid is less than 10^-7 (e.g. 10^-8), its conjugate base will be __________. a) stronger b) weaker hint: consider the value of Ka x Kb (or Kw)

a) stronger

What is the relationship between pKa and pKb? provide a formula/equation.

pKa + pKb = pKw = 14

acid strength ___________ with an increase in Ka. a) increases b) decreases

a) increases

acid strength ___________ with an increase in pKa. a) increases b) decreases

b) decreases

base strength ___________ with an increase in Ka. a) increases b) decreases

b) decreases

base strength ___________ with an increase in pKa. a) increases b) decreases

a) increases

provide the products: strong acid + strong base -->

water + neutral ions

provide the products: strong acid + weak base -->

water + acidic cation + neutral anion

provide the products: weak acid + strong base

water + neutral cation + basic anion

provide the products: weak acid + weak base

water + acidic cation + basic anion

As atomic radius increases, acid strength and stability of conjugate base ____________. a) increase b) decrease

a) increase

TRUE or FALSE: Acid strength increases to the right and down the periodic table (opposite of Zeff).

FALSE: SAME as Zeff

Resonance ______________ conjugate bases. a) stabilizes b) destabilizes

a) stabilizes

TRUE or FALSE: electronegativity increases with acid strength.

TRUE

TRUE or FALSE: an increase in induction (EWG) causes a decrease in acidity.

FALSE: acidity increases with induction

TRUE or FALSE: pKa increases as distance between the acidic proton and the electronegative atom increases.

TRUE

What is a zwitterion?

ion that can be protonated or deprotonated

For polyprotic acids, acid dissociation _____________ with sequential deprotonation. a) increases b) decreases

b) decreases

At the equivalence/stoichiometric point (pH 7), number of moles of acid are _______________ number of moles of base. a) greater than b) less than c) equal to

c) equal to

What is the name of the chemical used to visualize the equivalence point?

indicator

TRUE or FALSE: An indicator is usually a strong acid or strong base; whose conjugate form is a different colour.

FALSE: an indicator is usually a WEAK acid or base

When does the indicator change colour?

at the end point

TRUE or FALSE: A correct indicator will change colour at a pH that is far from the equivalence point, so that you can distinguish the end point from the equivalence point.

FALSE: A correct indicator will change colour at a pH that is very CLOSE tot he equivalence point.

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