Acid/Base, Kinetic Theory & Organic Test

Question 1

Define Concentrated + formula

Answer 1

Expressed as a ratio of solute to solution.

• Concentration = Quantity of solute/Quantity of solution

Question 2

Define Saturated

Answer 2

Solution in which no more pure solute can be dissolved into a given mass of solvent at a specified temp. & pressure

Question 3

Define Unsaturated

Answer 3

Solution in which more pure solute can be dissolved into a given mass of solvent at a specified temp & pressure

Question 4

Define super-saturated

Answer 4

More solute has been added than can be added in a given mass of solvent at a specified temp. & pressure

Question 5

Define ionisation

Answer 5

Process where a molecular substance dissolves in water producing separated ions

Question 6

Define dissociation

Answer 6

Process where an ionic substance dissolves in water producing ions

Question 7

Define strong electrolyte + example

Answer 7

• When substance dissolved in water
• completely ionises
• dissociates & thus present entirely as ions.
• Good conductors of: Strong acids, bases & soluble compounds
  (e. g. salt)

Question 8

Define weak electrolyte + example

Answer 8

• when substance dissolved in water
• only partly dissociates or ionises
• only partly present ions
• small amount of conductivity.
• Weak acids + bases are weak electrolytes
  (e. g. vinegar)

Question 9

Define non electrolyte + example

Answer 9

Substances dissolved in water don’t produce any ions.

- Doesn’t conduct electricity & any substances that doesn’t fit in any categories.
e. g. sugar

Question 10

Define strong acid + example

Answer 10

• Completely ionises in water
• Conduct electricity
• Strong electrolytes

(e.g. only nitric acid (HNO3), sulfuric acid (H2SO4) & hydrochloric acid (HCL))

Question 11

Define strong base + example

Answer 11

• Completely dissociates in water
• Conduct electricity
• Strong electrolyte

(e. g. G1 & 2 hydroxides & oxides)
* Only thing that dissociates ^

Question 12

Define monoprotic acid + example

Answer 12

Acid that contains one hydrogen atom

e.g. acetic acid (CH3COOH), nitric acid (HNO3), hydrochloric acid (HCL)

Question 13

Define polyprotic acid + example

Answer 13

Compound that contains multiple hydrogen atoms

e.g. phosphoric acid (H3PO4), sulfurous acid (H2SO3), sulfuric acid (H2SO4)

Question 14

Define weak bases + example

Answer 14

Partially ionise in water, only conduct a little energy and are weak electrolytes

(e.g. ammonia)

Question 15

Define weak acids + example

Answer 15

Only partly ionise in water, conduct little to no electricity and are weak electrolytes.

(e.g. acetic acid, hydrofluoric acid, phosphoric acid and carbonic acid)

Question 16

Define Arrhenius - acid

Answer 16

A substance that produces H^+ ion in solution

e.g. HCL –> H^+ + Cl-

Question 17

Arrhenius - base

Answer 17

A substance that produces OH^- ion in solution

e.g. NaOH –> Na^+ + OH-

Question 18

Assumptions of kinetic theory

Answer 18

• Gases consist of tiny particles moving in rapid, random, straight line motion until they collied with one another or the walls of the container.
• Size of the particles is negligible compare to size of the container in which they are moving. The particles have mass but no volume.
• Any attractive or repulsive forces between particles in the gas phase is negligible.
• The average kinetic energy of particles increase as temp. increase
• As temp. increase = kinetic energy increase
• Gas exert pressure = due to particles far apart + moving and colliding