L.7 Acids & Bases

Question 1

Arrhenius Acid & Arrhenius Base

Answer 1

Produce excess H+ in aqueous solution

Produce excess OH- in aqueous solution

Question 2

Bronsted-Lowry Acid & Bronsted-Lowry Base

Answer 2

BLAD Species that can Donate hydrogen (H+) ions

BLBA Species that can Accept hydrogen (H+) ions

Question 3

Lewis Acid & Lewis Base

Answer 3

Lewis Acid Electron Pair Acceptor

Lewis Base Electron Pain Donor

Question 4

Amphoteric Species

Answer 4

Species that act like acids in basic solution & act as bases in acidic solution

Amphiprotic = Bronsted Lowry Acid or Base

• Water is amphoteric
• conjugate species of polyvalent acids and bases can also behave as amphoteric and amphiprotic species.

Question 5

Four Strong Bases

Answer 5

Completely dissociate in solution & have very weak (inert) conjugates.

NaOH

KOH

Ca(OH)2

Mg(OH)2

Question 6

Six Strong Acids

Answer 6

Completely dissociate in solution & have very weak (inert) conjugates.

HClO4

HCl

HBr

HI

H2SO4 sulfuric acid

NHO3 nitric acid

Question 7

What is the Autoionization of water?

Answer 7

Even the purest form of water conducts electricity, has the presence of ions

Water can react with itself, in a process called autoionization…

H₂O + H₂0 —> H3O + OH

@ Equilibrium reactants are favored

Question 8

What is Kw?

Answer 8

Kw is the water dissociation constant

Kw= [H3O+] [OH-] = 10^-14 @ 25^oC (298K)

Kw = (1.0 * 10^-7) (1.0 * 10^-7​)

Kw= (1.0 * 10^-14​)

• Also known as the autoionization or ion product constant
• Only affected by temperature

Question 9

What is pH & pOH?

Answer 9

The concentration of hydrogen/hydroxide ions is measured in terms of pH & pOH

Is the negative log of the hydronium/hydroxide ion concentration

pH = -log [H3O⁺] & pOH = -log [OH^-]

pH + pOH = 14 @ 298 Kelvin

• SAME AS*
• pH = log [x]* = pH = log 1 / [x]

Question 10

What is Ka & Kb?

Answer 10

Weak acids and bases do not completely dissociate in solution and have corresponding Dissociation Constants (Ka & Kb)

Small Ka = weaker acid, thus dissolves less

vice-versa

Ka x Kb = Kw

Question 11

The relationship between Ka, Kb & pKa, pKb?

Answer 11

Low Kb then High pKb

Kb = 1.0 * 10^{-12 ———->} pKb = 12

Question 12

Go through steps on how to calculate the pH of a 1.00 M solution of CH₃COOH

Answer 12

CH₃COOH + H2O ——-> H3O+ + CH₃COO-

initial 1.00 0 0

Change -x. + x + x

1 - x x x

Ka = Products/ reactants

x<<<<1

Question 13

Relate Kw pKw pOH pH

Answer 13

Kw = 1 x 10^-14 then pKw = 14

kw = 1 x 10^-7 x 1 x 10^{-7 (each the concentration of H+ & OH- ions)}