Exam:2

Question 1

Spectator Ion

Answer 1

An ion that doesn’t participate in a reaction

Question 2

Saturated solution

Answer 2

A solution with the maximum possible
amount of a substance dissolved in it (Q=Ksp)

Question 3

Unsaturated solution

Answer 3

A solution with lower concentrations
than a saturated solution (Q<Ksp) (No precipitation)

Question 4

Supersaturated solution

Answer 4

A solution with higher concentrations
than a saturated solution (Q>Ksp) (precipitation will form)

Question 5

In a rice table, are the products positive while reactants negative?

Answer 5

Yes,
Products = Positive (Right)
Reactants = Negative (Left)

Ksp=Products/Reactants

Question 6

Common ion effect

Answer 6

If a solution has an ion in common with a solid, the solid will be less
soluble

Question 7

Determining which is more soluable in water.

Answer 7

If the Ksp is bigger = more soluble
If the Ksp is smaller = less soluble

Question 8

Sulfate (SO4) Charge
Sulfite (SO3) Charge

Answer 8

-2

Question 9

Phosphate (PO4) ,
Phosphide (PO3) Carges

Answer 9

-3

Question 10

Nitrate (NO3) Charge
Nitrite (NO2) Charge

Answer 10

-1

Question 11

Bicarbonate (HCO3) Charge
Hydroxide (OH) Charge

Answer 11

-1

Question 12

Acetate (C2H3O2) Charge
Ammonium (NH4) Charge

Answer 12

Ace. : -1
Amm. : +1

Question 13

If a Molecule is both a hydrogen donor/acceptor, it is a…?

Answer 13

Ambiprotic

Question 14

Acidic Solution vs. Basic Solution

Answer 14

A solution that contains extra [H+] is called acidic
A solution that can absorb extra [H+] is called basic

Question 15

Protonating vs. De-protenating

Answer 15

Adding an [H+] = protonating
Removing an [H+] = de-protonating

Question 16

When reacting acid with water

Answer 16

Acid + Water = H30 + Conjugate Base

Question 17

When reacting base with water

Answer 17

Wase + Water=HO- + Conjugate base

Question 18

Strong Acids (6)

Answer 18

[HCI] : Hydrochloric Acid

[HBr] : Hydrobromic Acid

[HI] : Hydroiodic Acid

[HNO3] : Nitric Acid

[HCIO4] : Perchloric Acid

[H2SO4] : Sulfuric Acid

Question 19

For Strong Acids, is the Ka greater than or less than (1) ?

Answer 19

Ka&raquo_space; 1

Question 20

Weak Acids (4)

Answer 20

[HF] : Hydrofluoric Acid

[HC2H302] : Acetic Acid

[H2SO3] : Sulforus Acid

[H3PO4] : Phosphoric Acid

Question 21

For Weak Acids, what is the Ka constant and is it greater than or less than (1)

Answer 21

Ka = 3.5 x 10 ^-4

Ka<1

Question 22

Strong Bases (8)

Answer 22

[LiOH] : Lithium Hydroxide

[NaOH] : Sodium Hydroxide

[KOH] : Potassium Hydroxide

[RbOH] : Rubidium Hydroxide

[CsOH] : Cesium Hydroxide

[Ca(OH)2] : Calcium Hydroxide

[Sr(OH)2] : Strontium Hydroxide

[Ba(OH)2] : Barium Hydroxide

Question 23

Weak Bases (Explanation)

Answer 23

Similar reactions as Bases (H20–> OH-), However the arrows go both ways indicating that there is partial dissasociation in the presense of water.

Question 24

Moles of Acid = …

Answer 24

Moles of Base

Question 25

For Weak Acids and Bases (only) what represents them at equilibrium?

Answer 25

Weak acid: equilibrium constant Ka Weak base: equilibrium constant Kb

Question 26

How to determine which Weak acid or base is stronger...

Answer 26

EX] If A has a LARGER Ka than B, we say A is a stronger acid than B

Question 27

Kw Constant

Answer 27

1.00 x 10^-14

Question 28

Ka X Kb = ...

Answer 28

Kw [C][D]/[A][B]

Question 29

If you have both Kw and Kb; solving for for Ka (vice versa). How would you solve?

Answer 29

[Kb]=[Kw]/[Ka]

Question 30

Turning Scientific Notation into (P) Variables

Answer 30

EX] [H] = 1.0x10^-6 = 0.000006 P[H] = -Log10 (1.0x10^-6) = 6.000

Question 31

All (P) Values (4)

Answer 31

[H+] = pH [OH-] = pOH [Ka] = pKa [Kb] = pKb

Question 32

as pH = -Log10 (H+), how does it look in reverse

Answer 32

10^pH

Question 33

pH vs. H+ (Acid Added) (Base Added)

Answer 33

Acid Added: H+ : Increase pH: Decrease Base Added: H+: Decrease pH: Increase

Question 34

pOH vs. OH- (Acid Added) (Base Added)

Answer 34

Acid Added: H+ : Decrease pH: Increase Base Added: H+: Increase pH: Decrease

Question 35

pH <-> pOH

Answer 35

pH + pOH = 14

Question 36

H+ <-> OH

Answer 36

Kw= [H+][OH]

Question 37

ph --> H H--> pH

Answer 37

1) 10^-ph 2) -Log10[H+]

Question 38

pOH --> OH OH--> pOH

Answer 38

1) 10^-pOH 2) -Log10[OH-]

Question 39

pKa<-->pKb

Answer 39

pKa + pKb = 14

Question 40

pKa --> Ka Ka --> pKa

Answer 40

1) 10^-pKa 2) -Log10(Ka)

Question 41

pKb --> Kb Kb --> pKb

Answer 41

1) 10^-pKb 2) -log10(Kb)