Acid/base Equalibrium

Question 1

Acid

Answer 1

The proton (H+) donor

Question 2

Base

Answer 2

The proton (H+) acceptor

Question 3

pH

Answer 3

A measure of acidity; pH = -log[H+]

Question 4

Hydronium ion

Answer 4

Formed when water bonds to a proton donated from an acid. H3O+

Question 5

Amphoteric

Answer 5

Able to act as both an acid and a base

Question 6

Polyprotic

Answer 6

An acid that can donate multiple protons.

Question 7

Ionization constant

Answer 7

The equilibrium constant for the ionization of a weak electrolyte

Question 8

Buffer solution

Answer 8

A solution that resists changes in pH; contains a weak acid and it’s conjugate base.

Question 9

Henderson-Hasselbalch equation

Answer 9

Used to calculate the pH of a buffer solution.
pH=pKa + log [conj base]/[acid] ; pOH= pKb + log [conj. Acid]/[base]

Question 10

Dissociation

Answer 10

The separation of ions that occurs when an ionic compound dissolves .
ex. CaCl2 (s) -> Ca^2+(aq) + 2Cl^- (aq)

Question 11

Neutralization reaction

Answer 11

A reaction between an acid and a base

Question 12

Buffering capacity

Answer 12

The amount of acid or base the buffer can neutralize before the pH behind to change appreciably

Question 13

Hydrolysis

Answer 13

The reaction of a substance with water

Question 14

Common ion effect

Answer 14

Suppression of ionization of a weak electrolyte by the presence of a common ion from a strong electrolyte

Question 15

End point

Answer 15

The point in a titration where the indicator changes color

Question 16

Equivalence point

Answer 16

The point in a titration where the moles of titrant is equal to the moles of unknown solution