final lab

Question 1

flame test

Answer 1

used to detect the presence of a metal (cation)

Question 2

what causes flames to change colors in the flame test

Answer 2

Electrons absorb energy → jump to higher orbitals → fall back down → emit light

Question 3

why does Li produce a red flame

Answer 3

The electrons jump a shorter distance, releasing less energy

Question 4

why does Na produce a yellow flame

Answer 4

the electrons jump a medium distance

Question 5

why does K produce a purple flame

Answer 5

the electrons jump a longer distance, releasing more energy

Question 6

what happens when a carbonate (CO3) salt is mixed with an acid

Answer 6

they release CO2 which causes bubbling

Question 7

why does Mg produce a colorless flame

Answer 7

the energy required for the electron transition is too great

Question 8

insoluble

Answer 8

produces a precipitate

Question 9

what flame color is the hottest, which one is less hot

Answer 9

blue is hotter than yellow

Question 10

what metals are always soluble

Answer 10

group I A (alkali earth) metals

Question 11

does solubility increase or decrease down group IIA

Answer 11

decrease (more precipitate)

Question 12

flame/solubility lab hazards

Answer 12

H2SO4 and bunsen burner

Question 13

what causes color differences in metal flame tests

Answer 13

Different metals have different electron structures → unique flame colors

Question 14

solubility reaction equation

Answer 14

M²⁺ (aq) + X²⁻ (aq) → MX (s) if MX is insoluble
M²⁺ = metal cation
X²⁻ = anion
MX (s) = solid precipitate if the salt is insoluble

Question 15

flame test procedure

Answer 15

spray blue flame with spray bottle containing metal and record flame color

Question 16

Solubility Test Procedure

Answer 16

1. Place 1 mL of each metal chloride in two sets of wells.
2. Add H₂SO₄ to one set and Na₂CO₃ to the other set
3. Record if a precipitate forms or if the solution remains clear

Question 17

unknown solution Identification Process

Answer 17

1. Do a flame test to identify the cation
2. do a solubility test to check for carbonate bubbles
3. Use solubility behavior trends to narrow down which cation is present.

Question 18

properties of solutions lab hazards

Answer 18

all acids and bases
esp: NaOH
HCl
NH3

Question 19

how to dispose of acids and bases

Answer 19

dump in sink and dilute with large volumes of water

Question 20

equipment used in properties of solutions lab (6)

Answer 20

graduated cylinders
stirring rod
litmus paper and alkacid paper
Conductivity probe and Vernier LabQuest
well plate
balance

Question 21

solution dilution equation

Answer 21

M₁V₁ = M₂V₂

Question 22

molarity equation

Answer 22

M=mol/L

Question 23

strong acid or base

Answer 23

strong electrolyte

Question 24

weak acid or base

Answer 24

weak electrolyte

Question 25

solution

Answer 25

aqueous mixture with 2 or more substances

Question 26

solvent

Answer 26

major component of a solution (usually water)

Question 27

solute

Answer 27

minor component of a solution (being added)

Question 28

solution lab procedure

Answer 28

Add ml acid or base to ml water use stirring rod to test acidity using alkacid and blue litmus paper

Question 29

non-electrolyte conductivity

Answer 29

0-100 μs

Question 30

weak electrolyte conductivity

Answer 30

100-8000 μs

Question 31

strong electrolyte conductivity

Answer 31

>8000 μs

Question 32

what compounds are strong electrolytes

Answer 32

NaOH, NaCl, HCl, H2SO4

Question 33

what compounds are weak electrolytes

Answer 33

NH3, HC2H3O2

Question 34

what compounds are non-electrolytes

Answer 34

C12H22O11, H2O

Question 35

titration lab hazards

Answer 35

HCl, NaOH, H2SO4

Question 36

Titration

Answer 36

A method to determine the concentration of an unknown solution by reacting it with a known volume and concentration of another solution.

Question 37

Neutralization

Answer 37

Reaction between an acid and a base to form water and a salt.

Question 38

Endpoint

Answer 38

The point in titration where the acid has been completely neutralized. Indicated by a color change.

Question 39

Indicator

Answer 39

A dye (e.g., phenolphthalein) that changes color to signal the endpoint.

Question 40

Molarity (M)

Answer 40

Moles of solute per liter of solution.

Question 41

titration lab procedure

Answer 41

1. rinse 2 burets with 5 ml of solution 2. fill one buret with H2SO4 and one with NaOH 3. add 10 ml of NaOH and phenolphthalein 4. Titrate with NaOH until solution is light pink or disappears after 30 seconds 5. calculate molarity

Question 42

Moles of HCl equation

Answer 42

mol HCl=mol NaOH×(mol HCl/mol NaOH)

Question 43

Molarity of Acid equation

Answer 43

M Acid= mol Acid/V Acid (M=mol/L) ​

Question 44

how to read a buret

Answer 44

from the top down to the nearest 0.01

Question 45

hazards of enthalpy lab

Answer 45

HCl, NaOH, and bleach (NaClO)

Question 46

what Cs to use for enthalpy calculations

Answer 46

4.184

Question 47

General Equation for Heat:

Answer 47

q=m⋅Cs⋅ΔT

Question 48

% error formula

Answer 48

|[experimental-theory]/theory|

Question 49

equipment used in enthalpy lab (4)

Answer 49

Styrofoam cup (calorimeter) Thermometer Graduated cylinders Beaker

Question 50

endothermic

Answer 50

absorbs heat into system

Question 51

exothermic

Answer 51

releases heat into surroundings

Question 52

enthalpy lab procedure

Answer 52

Mix 50.0 mL bleach (NaClO) + 50.0 mL Na₂SO₃ in calorimeter. Record temps as in Part One. Calculate

Question 53

ΔH per mol HCl

Answer 53

ΔH=q reaction in KJ/LR in moles

Question 54

bicarbonate lab hazards

Answer 54

HCl

Question 55

bicarbonate lab equipment (7)

Answer 55

Erlenmeyer flask Florence flask (for water displacement) plastic container Plastic weigh boat Graduated cylinder Thermometer Barometer

Question 56

ideal gas law

Answer 56

PV=nRT

Question 57

CO₂ pressure daltons law

Answer 57

PCO₂=Patm−PH₂O ​

Question 58

moles of CO₂

Answer 58

n=RT/PV ​

Question 59

% NaHCO₃ in the tablet

Answer 59

%NaHCO₃=(mass NaHCO₃/tablet mass)×100