pH, ACIDS, BASES...

Question 1

Acid

Answer 1

Compound that donates protons.

Question 2

Base

Answer 2

Compound that accepts protons

Question 3

Conjugate acid

Answer 3

Chemical compound formed when a base accepts a proton.

Question 4

Conjugate base

Answer 4

Chemical compound formed when an acid donates a proton.

Question 5

LEWIS defn

Answer 5

Acid : e- acceptor

Base: e- donor

Question 6

Dissociation

Answer 6

Takes place in Ionic compounds

Involves separation of ions of the ions already present.

Question 7

Ionization

Answer 7

Takes place in polar covalent compounds and metals.

Involves formation of charged ions from the molecules which were not in ionic state.

Question 8

Hydration

Answer 8

Process in which ions are surrounded by water molecules.

Question 9

Heat of solution

Answer 9

Solution formation can be accompanied by a change in temperature.

Question 10

Strength of acids/bases

Answer 10

Depends on degree of ionization.

Strong acids and bases fully ionize.
-single arrow
- strong acids: HCl, H2SO4, HNO3
-strong bases: any hydroxide.

(weak acids only partially ionize in solution. (double arrow). CH3COOH, HF, NH3 and ammonia derivatives. Reactants and products enter into an equilibrium.

Question 11

pH formulas

Answer 11

pH = -log[H+] & [H+]=10*-pH

Question 12

pOH formulas

Answer 12

pOH = -log[OH-] & [OH-] = 10*-pOH

Question 13

Titrant

Answer 13

Solution of known concentration, often placed in burette

Question 14

Indicator

Answer 14

A weak acid or base that changes colour
depending on pH values

Question 15

Equivalence point

Answer 15

When moles of acid are neutralized by
moles of base

Question 16

Endpoint

Answer 16

A colour change by the indicator to signal end of titration

Question 17

Titration

Answer 17

Technique to determine the concentration of an unknown solution using acid-base neutralization reaction.