Experimental report subject inorganic chemistry

Experiment 2: Reaction of alkaline earth metal and water Take 2 tubes and add in each tube 2 ml of water, a little Mg powder, and 1 drop of phenolphthalein.. Hydrogen in test tube 2 is m

VIETNAM NATIONAL UNIVERSITY, HO CHI MINH CITY

HO CHI MINH UNIVERSITY OF TECHNOLOGY FACULTY OF CHEMICAL ENGINEERING

EXPERIMENTAL REPORT Subject: Inorganic Chemistry

Instructor: Nguyễn Tu n Anh ấ

Classcode : CC04-VC02

GROUP 8:

1 Nguy n Th Minh Ng ễ ị ọc 2052187

2 Tr n Tu n Nguyên ầ ấ 2053281

3 Lâm Tuy t Nhi ế 2053300

Ho Chi Minh City, January 8 2022

UNIT 2: ALKALINE EARTH METAL (IIA)

I EXPERIMENTAL RESULTS

Experiment 1: Flame color test

on an alcohol lamp The flame has an orange-red color

Perform similarly with:

Explain the phenomenon: The metal ion of the salt absorbs energy from the flame, the electrons in the outermost shell are excited to a higher energy level So when it returns to the ground state, it will emit radiation with wavelengths in the specific visible region that represents each metal ion and has a different color

When igniting alkaline earth metal cations (in compounds with suitable anions) the flame has a characteristic color In the main subgroup of group IIA, when going from top to bottom, the specific color of the flame will change from red to yellow, which means the energy increases gradually due

to the increasing atomic radius, and the electrons easily move to a higher energy level

Experiment 2: Reaction of alkaline earth metal and water

Take 2 tubes and add in each tube 2 ml of water, a little Mg powder, and 1 drop of phenolphthalein

Air bubbles appear more The color is darker pink and spread throughout

Explain the phenomenon:

-Mg and water

decreases Therefore the reaction (1) occurs faster, and more air bubbles are released

solution fades to loss of color, and more gas is released Then the pink color reappears

Explain the phenomenon:

making the reaction (1) more intense and the gas released more

Mg(OH)2 + NH Cl MgCl + NH4 2 3± + H2O

Because Mg(OH)2 is dissolved, the balance (2) is shifted to the right, reducing OH- leading to phenolphthalein color loss

and OH- is produced by reaction (2)

Alkali-earth metals are weakly reactive with water at room temperature, but react strongly when heated or with a suitable catalyst

• Tube 1: React with acid (HCl) The precipitate dissolves, and the solution becomes transparent

• Tube 2: React with base (NaOH) No phenomenon occurs

solution with an unpleasant odor

b) Preparation and properties of alkaline earth metal hydroxide

-2³

Hydroxides of alkaline earth metals are basic By reacting their soluble salts with alkali metals, it is possible to prepare hydroxides of alkaline earth metals Experiment 4: Solubility of sulfate alkaline earth metal salt

completely consistent with their solubility product constants

The solubility of hydroxides and sulfate salts from Mg to Ba is the opposite because, for sulfate salts, the activation energy of the cation is greater than the lattice energy

water decreases, and the hydrate energy decreases, so the solubility decreases from

Mg to Ba

Experiment 5: Determine the water hardness

Pipette 10ml of hard water solution into 250ml erlen Then, add distilled water to obtain the total volume of 100ml Add 5 ml of pH 10 buffer and about 7 drops of ERIO-T indicator Shake well and titrate with ETDA 0.02N solution until the indicator changes from purple-red to light blue Perform the titration twice

Vsample = 10 ml

CN ETDA = 0.02 N

Experiment 6: Soften the hard water

calcium hydroxide slurry Boil mixture in 3 minutes and filter to remove the precipitate Use this mixture (10ml) to titrate with a similar procedure as experiment

5

Vsample = 50 ml

UNIT 6: HYDROGEN-OXYGEN- SULFUR

I EXPERIMENTAL RESULTS

Experiment 1: Preparation of hydrogen gas

Install the air collection system

Put 3 zinc beads in a test tube, then add 5ml concentrated HCl solution Collect the gas produced with a small test tube filled with water upside down in a small basin filled with water Zinc gradually dissolves, creates many bubbles, and generates a lot of heat

Because hydrogen reacts with oxygen mixed in the test tube and the gas pipeline, there is an explosion Initially, the amount of oxygen was more, so there was a loud explosion

2 H + O 2 2 ⎯³ t

H2O

The steam formed meets the cold glass and condenses

Hydrogen can be produced by the reactions of active metal with a strong acid

is approximate 2:1, the explosion is the biggest

Experiment 2: Activity of hydrogen molecules and hydrogen atom

well and divide into 3 tubes

Tube 1: Used as a standard tube

Tube 2: Let the hydrogen gas flow through The color of the solution fades but does not disappear

Hydrogen in test tube 2 is molecular hydrogen without strong reducing properties,

so it does not react with KMnO4 The solution is a little pale because in the solution when there is still a new hydrogen atom, not yet combined into a molecule Tube 3: Add some zinc particles Zinc dissolves, bubbles appear, the solution pales and becomes transparent

The newly born hydrogen is atomic hydrogen, which is a strong reducing agent, so

it reacts with KmnO4 to discolor the solution The gas is produced when unreacted atomic hydrogen combines to form molecular hydrogen

2 Atomic hydrogen has a stronger reducing property than molecular hydrogen

Experiment 3: Preparation of oxygen gas

the air collection system Heat the test tube and collect the escaping gas in the filled layer upside down in the water bath

water-2 KClO 3⎯ ³MnO 2⎯,t

Experiment 4: Property of oxygen gas

- Take a little of burning Sulphur in the first tube of oxygen It bursts into blue flame

violet-Sulfur has a strong affinity with oxygen So it can burn in the air with the violet-blue flame

- Insert a glowing splint into the second tube of oxygen It bursts into flame The reaction is strongly exothermic

The tube that has a large amount of oxygen will increase the rate of reaction

At a high temperature, carbon has a strong reducing property Thus, it reacts strongly with oxygen

CO2±

- Heat the copper wire and insert it into the third tube of oxygen

The black layer is due to copper being oxidized by oxygen, forming copper (II) oxide

2 I + H- 2O2 + 2 H I + 2 H O +÷ 2 2

a toothpick The solution is effervescent, with gas escaping The coals become brighter when being put into the tube, which proves that there is oxygen

Experiment 6: Reaction of Sulfur (S) and Copper (Cu)

Put 1g sulfur in a porcelain bowl, bring to a boil Use tongs to put the heated copper wire into the mouth of the upper porcelain cup The copper wire turns black, with white smoke rising

Cu(s) +S(g) CuS(s) ² (black)

White smoke is caused by evaporating sulfur

Sulfur has strong oxidizing properties at high temperatures

The sulfur acts as an oxidizing agent in the above reaction

Experiment 7: Reduction of thiosulfate salt

1:2) The solution is colorless Then it turns turbid

Sulfur makes the solution cloudy

sulfur-II ANSWER THE QUESTIONS

1 Compare the activity of hydrogen molecules and atom Explain? Write the

Atomic hydrogen is a stronger reducing agent than molecular hydrogen The newly born hydrogen is atomic hydrogen with strong reducing properties, so this compound reacts with KMnO4 to make a colorless solution Gas is produced when unreacted atomic hydrogen combines to form molecular hydrogen

2O

2 The important reaction of Oxygen

An important reaction of oxygen is oxidation, especially the combustion reactions

C + O CO 2² 2

C H O6 12 6 + 6 O 6 CO + 6 H O 2² 2 2

peroxide in a cool, dark place, open only when needed And when opened, keep the original brown bottle, which is designed to limit the light in to decompose it faster

4 Write the electron equation to demonstrate the reduction and oxidation of Sulfur For example?

The electronic equations showing the oxidizing properties of Sulfur:

S0 + 2e S ³

2-The electronic equations showing the reducing properties of Sulfur:

so Thiosulfate is a strong reducing agent and readily decomposes in acidic forming environments

sulfur-Oxidation number of S in Thiosulfate is +2

UNIT 8: Cu Ag - Au METAL (IB) –

I EXPERIMENTAL RESULTS

to react with all the amount of CuO

Heat the mixture until CuO is empty, filter the mixture if Cu still remains Concentrate the mixture until crystal seed appearance (without stirring)

vacuum filter (without using water in the filter process)

droplets of NaOH 2M until precipitation appearance Filter to keep precipitation A

a) Tube 1: Heat carefully

Heating copper hydroxide produces copper oxide, CuO, a black solid:

The mixture (left) is concentrated and CuSO 4 5H 2 O (right).

Cu(OH)2 (s) ² CuO (s) + H O (l) 2

b) Tube 2: Add high concentration HCl and heat carefully (with stirring)

CuCl2 + Cl -² [CuCl4]2-

c) Tube 3: Add 4ml NaOH 40% and heat

The precipitate dissolves and turns into a blue-purple-coloured solution

Experiment 5: Reaction of CuSO4 and AgNO3 with KI

Prepare 2 tubes:

Add drop by drop KI solution into 2 tubes and heat them

• Tube 1: A yellow precipitate forms Then it turns into earth-brown color

• Tube 2: A yellow precipitate forms The color remains after being heated

Experiment 6: Property of the precipitation

Prepare 2 tubes:

Add drop by drop NaOH 2M solution into 2 tubes and heat them

Tube with CuSO (left) and AgNO (right) afterwards 4 3

CuSO4 + NaOH ² Cu(OH) ³ + Na2 2SO4

• Tube 2: A brown precipitate forms (AgOH)

Collect the precipitation and separate it into 4 tubes (each precipitation in 2 tubes)

green solution

• Tube 1.2 (reacting with NH4OH): the precipitate slowly dissolves and becomes a blue solution

• Tube 2.1 (reacting with HNO3): the precipitate dissolves and turns into a white solution AgOH is unstable and easily dissolves in water:

Metals from Group IB are amphoteric but weak, easy to create complex substances with ammonia solution

Experiment 7: Property of the Silver salt

• Tube 1: Add 10 droplets NaCl 0.1M solution A white precipitate forms

• Tube 1: The precipitate dissolves to create a colorless solution

• Tube 2: The precipitate partially dissolves

• Tube 3: The precipitate hardly dissolves

The colors of the precipitates become darker from Cl to I The dissolubility decreases from AgCl, AgBr to AgI because of increasing anion radius Experiment 8: Silver mirror reaction

10% solution, a precipitate appears then gradually dissolves

Then, add 5 droplets of HCHO 40% solution and heat the tube at 50 C A white Āprecipitate forms

II ANSWER THE QUESTIONS

1 Why do metals in groups IA and IB have different properties despite a similar outer layer structure with one electron?

Although the metals in groups IA and IB have a similar outer layer structure with one electron, their properties are very different The reason is that the barrier effect of IB metals is weaker than that of IA metals, leading to their higher first ionization energy Consequently, the IB metals are less active than the IA metals

2 Cu preparation from malachite equations?

A white precipitate appears after adding

5 droplets of HCHO 40% solution

UNIT 10: CHROMIUM

I EXPERIMENTAL RESULTS

Add drop by drop the diluted NaOH solution into 2 tubes Collect the precipitation

by centrifugation

• Tube 1: Reaction with the dilute acid

• Tube 2: Reaction with the excess of dilute NaOH solution

Experiment 5: Equilibrium between chromate and dichromate

ions

Add drop by drop NaOH 2N solution into the tube until its color changes The color

H+ + OH H-³ 2O

The equilibrium of chromate and dichromate ion: 2CrO + 2H42- + ⇄ Cr2O72- + H O 2

water, it forms an orange solution The colors come from the negative ions:

equilibrium with each other in an aqueous solution

Experiment 6: Solubility of chromate salt

0.5N

Pb(NO )3 2 + K2CrO4 ³ PbCrO4 ÿ + 2KNO 3

with silver nitrate, a brown-red precipitate of silver chromate is formed along with potassium nitrate

each tube Tube (1) partially dissolves, tube (2) dissolves fast, tube (4) and (5) hardly dissolves

2-Tube 1 (leftmost) to tube 5 (rightmost)

Tube 1 (leftmost) to tube 5 (rightmost) after adding 1ml CH 3 COOH

CrO4 + 2H Cr⇄ 2O7 + H O 2

Chromates (CrO42-) are usually insoluble Exceptions include Na2CrO4, K2CrO4, (NH4)2CrO4, and MgCrO4

UNIT 12: TRANSITION METAL (GROUP VIIIB)

Fe Co Ni – –

I EXPERIMENTAL RESULTS

Experiment 1: Preparation of Mohr salt (NH₄)₂Fe(SO₄)₂·6H₂O

Hydrogen The solution is black

The solution was black because Fe was contaminated

Boil in a fume hood until the iron completely dissolves, the solution turns

of the solution constant

Filter the solution

Cool and allow to crystallize at room temperature Vacuum filtration obtains a

The Mohr salt solution reacts with:

- Diluted KMnO / H4 2SO4: The solution has a color of light yellow

add 2-3 drops of 0.5N KI, dark purple precipitate appears

• Tube 1: 2 drops 0.01N NH SCN solution The solution turns to blood 4red

color appears

When shaking, the liquid becomes turbid and bright blue due to the dispersion of the blue precipitate through the liquid The color of cobalt (II) hydroxide quickly changes from blue to pink The pink material also can be written as hydrous

• Tube 1: Heat and place in the air The color of the precipitate changes to dark chocolate-brown

chocolate-brown

tubes An apple-green precipitate appears

-2 (apple-green)

• Tube 1: Place in air The color of the precipitate does not change

• Tube 2: Add some droplets of H2O2 3% solution The color of the precipitate changes to black

The stability of divalent compounds increases, stability of trivalent compounds decreases from Fe to Ni

▪ Tube 1.1: React with concentrated HCl solution ² The precipitate is dissolved, producing colorless solution

appears

Divide the precipitate into two parts

▪ Tube 2.1: React with concentrated HCl solution ² The precipitate is dissolved, forming yellow solution

The dispersion of the blue precipitate through the liquid causes the liquid to

become turbid and vivid blue when shaken Cobalt (II) hydroxide rapidly changes color from blue to pink

-2Divide the precipitate into two parts

▪ Tube 3.1: React with concentrated HCl solution ² The precipitate is dissolved, forming reddish-pink solution

appears

-2 (apple-green)Divide the precipitate into two parts

▪ Tube 4.1: React with concentrated HCl solution ² The precipitate is dissolved, forming brown solution

in the alkaline solutions

2

b) The Tsugaep reaction of Nickel

complex solution

-2 (green)

Add 1 droplet of dimethylglyoxime in tube A rose-red precipitate appears

The complex has a square shape, is electrically neutral, weakly acidic, and basic So

will cause the precipitate to dissolve immediately This reaction is used for the

Experiment 5: Properties of Co and Ni compounds 2+ 2+

precipitate appears then dissolves to create the liquid that is brown at the top, pink at the bottom, blue in the middle When shaking, the solution turns brown

creating the blue color in the middle of the liquid

• Tube 2: Add the concentrated HCl solution to excess A blue solution appears