Module 4: Acid-Base Equilibria In Aqueous Solution

Question 1

Define acid

Answer 1

Proton donor
Or
Electron pair acceptor (Lewis)

Question 2

Define base

Answer 2

Proton acceptor
Or
Electron pair donor (Lewis)

Question 3

Define conjugate acid-base pair

Answer 3

Species that differ by a single proton

Question 4

Define amphirotic

Answer 4

Can accept or donate protons

Acid or base

Question 5

Strong acids (name)

Answer 5

HI
HBr
HCl
H2SO4
HNO3
HClO4 (perchloric acid)

Question 6

Strong bases (name)

Answer 6

Group 1 hydroxides
Group 2 hydroxides
H- (ex NaH)
O(2-) (ex Na2O)
S(2-) (ex Na2S)

Question 7

Binary acids - what increases acid strength

Answer 7

Electronegativity up

Size smaller

Question 8

What increases acid strength of inorganic oxyacids

Answer 8

More terminal oxygens (resonance)

More electronegative central atom

Question 9

What increases acid strength of organic oxyacids

Answer 9

Number of electronegative atoms in R group increases

Distance between electronegative R and COOH decreases

Question 10

What determines pH of weak polyprotic acids

Answer 10

First ionization step

Question 11

Common ion effect

Answer 11

Ionization of a weak acid is significantly suppressed by the addition of a strong acid or A-

Question 12

Define buffer solution

Answer 12

Comparable amounts of weak acid and conjugate base

Able to maintain relatively constant pH even if strong acid or base is added to it

Question 13

Henderson-Hasselbalch equation

Answer 13

pH = pKa + log(A-/HA)

Only for buffer solutions