RMS Solutions

Question 1

Qsp > Ksp

Answer 1

The concentration of ions too high (above solubility limit), so precipitation should form

Question 2

Qsp = Ksp

Answer 2

Saturated solution and at equilibrium for this temperature

Question 3

Qsp < Ksp

Answer 3

More solute can dissolve until a saturated solution is reached at equilibrium

Question 4

a (pure solid) = ?

Answer 4

ZERO

Question 5

a (pure liquid) = ?

Answer 5

ZERO

Question 6

Kw

Answer 6

1.0 x 10^-14

Question 7

Brønsted–Lowry acid

Answer 7

Proton (H+) donor

Question 8

Brønsted–Lowry base

Answer 8

Proton (H+) acceptor

Question 9

Lewis acid

Answer 9

Electron pair acceptor

Question 10

Lewis base

Answer 10

Electron pair donor

Question 11

Amphoteric

Answer 11

Can be either acids OR bases depending on conditions

Question 12

Arrhenius acid

Answer 12

Species that increases the number of H3O+ ions when dissolved in water (pH decreases).
Arrhenius acids are limited to aqueous solutions. All Arrhenius acids are Brønsted–Lowry acids.

Question 13

Arrhenius base

Answer 13

Species that increases the number of OH- ions when dissolved in water (pH increases)

Question 14

What is a good approximation to use for [HIn]:[In-]?

Answer 14

HIn = colour 1
In- = colour 2

Colour 1 occurs if 10:1, i.e. excess of HIn, so log0.1 = 1.
Colour 2 occurs if 1:10, i.e. excess of In-, so log10 = +1

Question 15

If a species is oxidised, it is the _ _

Answer 15

Reducing agent

Question 16

If a species is reduced, it is the _ _

Answer 16

Oxidising agent

Question 17

Electrode

Answer 17

Conductive interface where electron transfer can occur

Question 18

Salt bridge

Answer 18

Allows ions to flow to maintain electron neutrality of solutions

Question 19

Convention of anode and cathode order

Answer 19

Anode is on the left and cathode is on the right

Question 20

Electrodes in galvanic (voltaic) cell

Answer 20

Cathode = positive electrode
Anode = negative electrode

Question 21

Standard Hydrogen Electrode (SHE)

Answer 21

Platinum terminal -> conductive inert metal provides a phase boundary where electron transfer may occur
Standard conditions -> pressures at 1 bar (p⦵), concentrations all at 1 mol dm^-3 (c⦵), and a specified temperature (usually 298K)

BY DEFINITION: E⦵ = 0.000 V
Half cell reaction: 2H+ (aq) + 2e- -> H2 (g)

Question 22

The greater the E⦵, the …

Answer 22

Higher reducing potential, the more likely it is to be reduced.

The one with the greater E⦵ will be reduced.

Question 23

E⦵ cell = _ - _

Answer 23

E⦵ cell = E⦵ (cathode) - E⦵ (anode)

E⦵ cell = E⦵ (RED) - E⦵ (OX)

Question 24

RED CATS

Answer 24

reduction occurs at cathode

Question 25

OXID AN

Answer 25

oxidation occurs at anode

Question 26

E⦵ cell > 0

Answer 26

Rxn spontaneous

Question 27

E⦵ cell < 0

Answer 27

Rxn non-spontaneous

Question 28

For standard cell notation, if no electrode material is listed, you use _

Answer 28

Platinum solid, Pt (s)

Question 29

“I” denotes what in standard cell notation?

Answer 29

Phase boundary

Pt (s) |Fe3+ (aq) , Fe2+ (aq) ||Br2 (l) |Br– (aq) |Pt (s)

Question 30

”||” denotes what in standard cell notation?

Answer 30

Salt bridge

Pt (s) |Fe3+ (aq), Fe2+ (aq) ||Br2 (l) |Br– (aq) |Pt (s)

Question 31

”::” denotes what in standard cell notation?

Answer 31

Semi-permeable membrane

Question 32

”,” in standard cell notation

Answer 32

Mixed (aq) species are separated by a comma

Pt (s) |Fe3+ (aq), Fe2+ (aq) ||Br2 (l) |Br– (aq) |Pt (s)