Acids and Bases

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Total cards: 24•Content version: v4•Public deck•Updated: 8/1/2026

Card preview (24)

Front (Question)

Arrhenius base

Back (Answer)

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

Front (Question)

Arrhenius acid

Back (Answer)

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

Front (Question)

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

Back (Answer)

neutralization

Front (Question)

What is a neutralization reaction?

Back (Answer)

acid + base –> water + salt

Front (Question)

Bronsted-Lowry acid

Back (Answer)

species that produces H+

Front (Question)

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

Back (Answer)

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

Front (Question)

Bronsted-Lowry Base

Back (Answer)

species that accepts H+

Front (Question)

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

Back (Answer)

acid LOSES proton base GAINS proton

Front (Question)

Lewis acid

Back (Answer)

electron-pair acceptor hint: lewis Acid = electron pair Acceptor

#10

Front (Question)

Lewis base

Back (Answer)

electron-pair donor

#11

Front (Question)

A Lewis acid is a/an: a) electrophile b) nucleophile

Back (Answer)

a) electrophile hint: lewis Acid = electron pair Acceptor

#12

Front (Question)

A Lewis base is a/an: a) electrophile b) nucleophile

Back (Answer)

b) nucleophile

#13

Front (Question)

Which species is fundamental to understanding MCAT OCHEM? a) Arrhenius b) Bronsted-Lowry c) Lewis

Back (Answer)

c) Lewis

#14

Front (Question)

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

Back (Answer)

FALSE

#15

Front (Question)

List the strong acids (7).

Back (Answer)

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

#16

Front (Question)

List the strong bases (7).

Back (Answer)

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

#17

Front (Question)

What does the term “pH” refer to?

Back (Answer)

“potential of the hydrogen ion”

#18

Front (Question)

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

Back (Answer)

pH = -log[H3O+] hint: p = -log[whatever]

#19

Front (Question)

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

Back (Answer)

pOH = -log[OH-] hint: p = -log[whatever]

#20

Front (Question)

pH + pOH = ?

Back (Answer)

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

#21

Front (Question)

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] = ?

Back (Answer)

• 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

#22

Front (Question)

Calculate the following: \+log(1) = ? \+log(3.2) = ? \+log(10) = ?

Back (Answer)

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

#23

Front (Question)

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

Back (Answer)

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

#24

Front (Question)

given the reaction below, what is the formula for the equilibrium constant (Kc)? aA + bB –>/<– cC + dD

Back (Answer)

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