Chem Lesson 5: 14.4, 14.6 - 14.7

Question 1

Ionic Bond

Answer 1

Chemical bond between metals and non-metals involving the transfer of electrons.

Question 2

Salt (Def)

Answer 2

Ionic compounds composed of cations and anion which may be capable of ionizing into it’s constituent parts in water.

Question 3

Periodic table (staircase) metals and non-metal locations

Answer 3

Metals to the left of stair case and non-metals to the right.

Question 4

Periodic table charges

Answer 4

+1, +2, +3, skip -3, -2, -1

Question 5

Salt (how they are produced)

Answer 5

Produced by the reaction of an acid with a base. (One is usually a base)

NaOH + HCl -> NaCl + H20

Question 6

Strong Bases (Molecular Mnemomic)

Answer 6

Liking - Li(OH)
Killer - K(OH)
Badgers - Ba(OH)2
Can - Ca(OH)2
Cause - Cs(OH)
Strong - Sr(OH)
Nausea - Na(OH)

Question 7

Strong Acids (Mnemonic and Acid)

Answer 7

So - H2So4 - Sulfuric Acid
I - HI - Hydroiodic Acid
Brought - HBr - Hydrobromic Acid
No -HNO3 - Nitric Acid
Clean - HCl - Hyrdochloric Acid
Clothes - HCLO4 - Perchloric Acid

Question 8

Strong Acids and Bases produce (strength) solutions?

Answer 8

Neutral

Question 9

Weak Acids produce (x) solutions?

Answer 9

Weak basic solutions

Question 10

Weak bases produce (x) solutions?

Answer 10

Weak acidic solutions

Question 11

What should I use to find the equilibrium concentrations of the products in a dissociation reactions involving acids and bases?

Answer 11

Ka and Kb

Question 12

What is used to help us to distinguish strong acids/bases from weak acids/bases?

Answer 12

Ka and Kb

Question 13

Pka

Answer 13

-log(ka)

Question 14

Buffers

Answer 14

Solutions that resist changes in water.

(Prevents H2O from being converted into H3O+ or OH-)

Question 15

Buffer capacity

Answer 15

Amount of acid or base that can be added to a buffer solution before the PH changes by more than one.

Question 16

Suitable Buffers (2 Rules)

Answer 16

1. Good buffers should have equal concentrations of both acid and it’s conjugate. (no more than 10% difference).

Question 17

Henderson Hasselbach Equation

Answer 17

PH = pka + log([A]/[HA])

Question 18

Henderson Hasselbach Equation (What it’s used for)

Answer 18

Used to calculate PH of buffer solutions.

Question 19

Limiting Reactant

Answer 19

Reactant consumed first in a chemical reaction and limits how much product can be formed.

Question 20

How to get rid of log in an equation?

Answer 20

Raise both sides to the power of 10

Question 21

Arrhenius Acid

Answer 21

Increase H+ concentration in water

Question 22

Arrhenius Base

Answer 22

Increases OH- concentration in water

Question 23

How can you tell if a compound is a salt?

Answer 23

If it’s made up of cations and anions

Question 24

Pure Salt (what are they made of?)

Answer 24

Strong acids and bases

Question 25

Solubility Rules & Exeptions

Answer 25

N nitrates
A acetates
G group 1

S sulfates
A ammonium (nh4+)
G group 17

Execemptions
1. Never soluble with sulfates or group 17
P Lead (Pb)
M Mercury (Hg2+2)
S Silver (Ag+)

Castro Bear
2. Never soluble with sulfates
Ca2+ Sr 2+ Ba 2+

Question 26

Analyte

Answer 26

Solution with unknown concentration

Question 27

Titrant

Answer 27

Known quantity that is added to the analyte

Question 28

End Point

Answer 28

Change in color

Question 29

Equivalence Point

Answer 29

Moles of titrant equals moles of analyte.