suggested answers to in-text activities and...

New 21st Century Chemistry

Suggested answers to in-text activities and unit-end exercises

Topic 8 Unit 33

In-text activities

Internet Search & Presentation (page 207)

The aspirin story

The history of aspirin and other medicines dealing with pain, fever or inflammation reveals many

interesting points about scientific methodology and the interaction of people and society with

technology. One overriding theme that emerges when looking at the development of medicines is

the importance of sharing information and cooperation in research. Time and again discoveries in

one part of the world have been published, but not developed fully until another person reads and

uses the information in another time and place.

The textbook gives some detail of the history of the development of aspirin, but it is intended that

students find out more than what has been given to them.

Conditions that aspirin helps to relieve or cure

At over-the-counter dosage (one or two grams), it relieves fever and minor aches and pains. At

dosages three or four times higher, available by prescription only, it reduces swelling and is used to

treat gout, rheumatoid arthritis, and inflammatory ailments. Many people take low dosages (below

100 milligrams) daily for preventing recurrent stroke or heart attack. Recent studies found it

effective in reducing risks for colon and breast cancers. Evidence is accumulating for similar effects

in Alzheimer and other diseases.

However, aspirin can irritate the stomach and in some cases cause ulcer and internal bleeding.

Alternative treatments for pain relief are available: paracetamol and ibuprofen.

Making aspirin soluble

One problem with aspirin is that it is not particularly soluble in cold, or even warm, water (e.g. 36

°C – the temperature of the human body).

A medicine tablet works far better if it is water-soluble, because it then enters the bloodstream more

rapidly. One way of making the aspirin ‘soluble’ is to convert it to one of its salts, e.g. the sodium

salt. As this product is ionic, it would be much more water-soluble than the parent covalent acid –

aspirin itself.

Suggested answers to in-text activities and unit-end exercises 1 © Jing Kung. All rights reserved.Topic 8 Unit 33


Clinical trials

A new medicine has to demonstrate its safety, quality and efficacy through a series of rigorous

clinical trials in order to obtain a licence and be available to the general public.

Clinical trials are conducted in phases. The trials at each phase have a different purpose and help

scientists answer different questions.

• In Phase I trials, researchers test an experimental drug in a small group of people (20 – 80) for

the first time to evaluate its safety, determine a safe dosage range, and identify side effects.

• In Phase II trials, the experimental study drug is given to a larger group of people (100 – 300) to

see if it is effective and to further evaluate its safety.

• In Phase III trials, the experimental study drug is given to large groups of people (1 000 – 3 000)

to confirm its effectiveness, monitor side effects, compare it with commonly used treatments,

and collect information that will allow the experimental drug to be used safely.

• In Phase IV trials, post marketing studies delineate additional information including the drug’s

risks, benefits, and optimal use.

References:

http://www.creatingtechnology.org/biomed/aspirin.htm

http://docbrown.info/page04/OilProducts15.htm

http://www.abpi.org.uk//publications/briefings/clinical_brief.pdf

http://clinicaltrials.gov/ct2/info/understand


Soap-making by ancient people

Soap making is one of the oldest known organic chemical reactions. Soaps are formed by the

reaction of fats or oils with an alkali. It is possible that the process could have been discovered in

prehistoric times when animal fat from cooking meat dripped onto wood ash (which is alkaline)

producing a crude soap. Archaeologists once found evidence that the Babylonians were making

soap around 3000 BC. Soap making was probably introduced to Europe by the Phoenicians around

600 BC.

The Romans also produced soap. The word soap in many languages is derived from a famous

Roman legend. According to this legend women who washed clothes in the stream below Sapo Hill

noticed how much easier they were to clean than in other streams. It seemed that the ashes and fats

from sacrificial fires in temples on Sapo Hill mixed together to produce soap which was washed

down from the hill. A soap-making factory, complete with soap moulds and bars of soap, was

discovered in the ruins of Pompeii. With the fall of the Roman Empire, soap making declined and

soap was used mostly for cleaning clothes and textiles rather than for personal bathing.

Commercial production of soap in Europe

Soapmakers’ guilds began to spring up in Europe during the seventeenth century. Southern

European countries, such as Italy, Spain, and France were early production centers for soap.



The English began soapcrafting during the twelfth century. Unfortunately, soap was heavily taxed

as a luxury item, and so it was only readily available to the rich. In 1853, when the English soap tax

was repealed, a boom in the soap trade coincided with a change in the social attitudes toward

personal cleanliness.

In America, soap was made by women producing it out of their homes seasonally. The commercial

production of soap did not start until the early 1600s when enterprising soapmakers from England

began arriving in the New World.

Scientific advancements and soap-making

Scientific advancements that affected the soapmaking trade began with Nicholas Leblanc, a French

chemist who patented a process for making an alkali from common salt in 1791. His process

allowed for the inexpensive production of soda ash.

In the early 1800s, Michel Chevreul's significant discoveries about the relationship of fats,

glycerine, and fatty acids laid the groundwork for the chemistry of soaps and fats.

During the mid 1800s, Belgian chemist Ernest Solvay discovered the ammonia process that

improved the methods for extracting soda ash from common salt. This increased the availability and

quality of soda ash for soap making.

As a result of the scientific achievements, soap became a popular and easy-to-obtain commodity.

Production of soapless detergents

Soapless detergents use materials called surfactants which dissolve greases; detergent effects of

certain synthetic surfactants were first noted in 1913 by A Reychler, a Belgian chemist. During

World War I the Germans used soapless detergents as an alternative to soap but after that war their

uses were largely confined to industrial processes.

After World War II the U.S. aviation fuel plants changed over to making tetrapropene, used in

household detergents, causing a fast growth of household use in the late 1940s. The first product

was a ‘soapless shampoo’. Up to the 1960s they were more expensive than traditional soaps but

they could be used with hard or soft water equally well.

In the late 1960s biological detergents, containing enzymes and better suited to dissolve protein

stains such as egg stains, were introduced in the U.S..

References:

http://inventors.about.com/library/inventors/blsoap.htm

http://www.harvestsoaps.com/history_of_soap.htm

http://www.soapmakingfun.com/making-homemade-soap/history-of-soap-making.shtml

http://www.sappohill.com/soaphistory.html

http://www.worldlingo.com/ma/enwiki/en/Detergent

http://www.igg.org.uk/gansg/12-linind/soap.htm



Checkpoint (page 225)

1 CH3(CH2)14CH2— is a non-polar group which can dissolve in grease.

is a polar group which can dissolve in water.

2 a) Detergent I

b)

c) Before shaking an oil-water mixture, the hydrocarbon ‘tails’ of detergent particles are

soluble in the oil and the anionic ‘heads’ are soluble in the water.

Upon shaking, oil droplets form. Each droplet is surrounded by detergent particles with the

anionic ‘heads’ in the water.

Repulsion between the anionic heads prevents the oil droplets from coming together again.

Thus, the oil droplets remain suspended in the water. An emulsion is formed.

d) Detergent I functions well in hard water.

When detergent II is added to hard water, scum forms.

A lot of the detergent is needed to get a lather.

e) Not suitable

Sea water contains a lot of metal ions, such as magnesium ions and calcium ions.

Detergent II will react with the metal ions to form scum and hence reduce the effectiveness

of the detergent.


1



2 a)

b) Carboxyl group; hydroxyl group


1 a) Ester functional group; carbon-carbon double bond

b)

c) X is formed from an unsaturated carboxylic acid.

It is a liquid at room temperature as its molecules cannot pack together closely due to the

presence of cis double bonds.

2 a) First gently heat, while stirring, a mixture of fat and concentrated sodium hydroxide solution

for about 20 minutes. Most of the soap formed dissolves in the reaction mixture.

Then add concentrated sodium chloride solution to the mixture. The soap separates from the

solution and floats on the surface.



Obtain the soap by filtration. Then wash the soap with a little distilled water and allow to

dry.

b)

c) Saponification


a) Amine functional group, carboxyl group, amide functional group, ester functional group

b)


Saccharin

Saccharin was discovered over a century ago and has been used as a non-caloric sweetener in foods

and beverages for more than 100 years. Saccharin contributes no calories to the diet because it is not

metabolized by the human body. (It is excreted in the same form as ingested.)

Uses of saccharin

Saccharin is useful for people trying to control their weight. Saccharin may assist in weight

management, control of blood glucose and prevention of dental caries.

Saccharin is appropriate for medical and nutrition therapy for people with diabetes, and dietetic

professionals may incorporate saccharin into the individualized meal plans of their patients who

have diabetes.



References:

http://www.saccharin.org/pdf/sach_broch_final_406.pdf

http://chemistry.about.com/od/factsstructures/ig/Chemical-Structures---S/Saccharin.htm

Sucrose

Sucrose or table sugar is obtained from sugar cane or sugar beets.

Sucrose is made from glucose and fructose units. The glucose and fructose units are joined by a

glycosidic linkage.

Uses of sucrose

Sucrose and its co-products lend themselves to possibilities in many areas:

• fine chemicals;

• pharmaceuticals;

• polymers;

• building and structural materials;

• fermentation or enzyme substrate for chemicals production;

• new food products and sweeteners;

• making biodiesel / ethanol;

• transformation of cane or beet plant to make other products.

References:

http://www.spriinc.org/buton10bftpp.html

http://www.elmhurst.edu/~chm/vchembook/546sucrose.html

Cellulose

Cellulose is a natural polymer of the β-glucose monomer. Two b-glucose monomer molecules can

link together via an oxygen atom at the first carbon atom (C1) of one unit and the fourth carbon



atom (C4) of the next. A water molecule is released. This is a condensation reaction. The link

between the two glucose units is called a glycosidic linkage.

Uses of cellulose

Cellulose has been used to make paper since the Chinese first invented the process around AD 100.

Cellulose is separated from wood by a pulping process that grinds woodchips under flowing water.

The pulp that remains is then washed, bleached and poured over a vibrating mesh. When the water

finally drains from the pulp, what remains is an interlocking web of fibres that, when dried, pressed,

and smoothed, becomes a sheet of paper.

Cellulose is the major constituent of textiles made from cotton, linen and other plant fibres.

Cellulose can also be processed and chemically modified to make plastics, photographic film, and

rayon. Cellulose derivatives can be used as adhesives, explosives, thickening agents in food, and

moisture-proof coatings. Historically, cellulose made some of the first synthetic polymers like

cellulose nitrate, cellulose acetate, ethyl cellulose and rayon.

References:

http://www.scienceclarified.com/Ca-Ch/Cellulose.html

http://en.wikipedia.org/wiki/Cellulose

http://web1.caryacademy.org/chemistry/rushin/StudentProjects/CompoundWebSites/2000/Cellulose

/uses.htm

Starch

The main sources of starch are the cereal crops, rice, maize, wheat and the root crop potatoes.

Starch is composed of a mixture of two substances: amylose, an essentially linear polysaccharide,

and amylopectin, a highly branched polysaccharide. Both forms of starch are polymers of a-glucose.

Natural starches contain 10 – 20% amylose and 80 – 90% amylopectin.

Amylose typically consists of more than 1 000 glucose units link together via oxygen atoms

between the first carbon atom (C1) of one unit and the fourth carbon atom (C4) of the next. The link

between glucose units is called a glycosidic linkage.



Chains of glucose units with such glycosidic linkages tend to assume a helical arrangement.

Amylopectin has a structure similar to that of amylose, with the exception that in amylopectin the

chains are branched. Branching takes place between C6 of one glucose unit and C1 of another and

occurs at intervals of 20 – 25 glucose units.

These two molecules are assembled together to form a semi-crystalline starch granule. The granule

also contains small amounts of lipid and phosphate. The exact proportions of these molecules and

the size of the granule vary between species.

Examples of use of starchFood and

drinksAnimal

feedAgriculture Plastic Pharmacy Building Textile Paper Various

mayonnaise pellets seed coating biodegradable plastic

tablets mineral fibre

warp corrugated board

oil drilling

baby food by-product fertilizer dusting powder

gypsum board

fabrics cardboard water treatment

bread concrete yarns paper glue



soft drinksmeat

productsconfectionerySource: International Starch Institute, Aarhus, Denmark

References:

http://www.starch.dk/

http://jxb.oxfordjournals.org/cgi/content/full/54/382/451

Cholesterol

Cholesterol is a waxy, fat-like compound that belongs to a major class of lipids called steroids. It's

found in many foods, in the bloodstream and in all the body’s cells.

Cholesterol comes from two sources: the body and food. The liver and other cells in the body make

about 75% of blood cholesterol. The other 25% comes from food.

Functions of cholesterol

Cholesterol is essential for

• formation and maintenance of cell membranes (helps the cell to resist changes in temperature

and protects and insulates nerve fibres);

• formation of sex hormones;

• production of bile salts, which help to digest food;

• conversion into vitamin D in the skin when exposed to sunlight.

‘ Good’ and ‘bad’ cholesterol

Cholesterol cannot dissolve in the blood. It has to be transported to and from the cells by carriers

called lipoproteins. Lipoproteins consist of protein, cholesterol, triglycerides and phospholipids.

The density of these lipoproteins is determined by the amount of protein in the molecule. The terms

‘good’ and ‘bad’ cholesterol refer to high density lipoproteins (HDL) and low density lipoproteins

(LDL) respectively.

When too much LDL (bad) cholesterol circulates in the blood, it can slowly build up in the inner

walls of the arteries that feed the heart and brain. Together with other substances, it can form

plaque, a thick, hard deposit that can narrow the arteries and make them less flexible. This condition



is known as atherosclerosis. If a clot forms and blocks a narrowed artery, heart attack or stroke can

result.

About one-fourth to one-third of blood cholesterol is carried by high-density lipoprotein (HDL).

HDL cholesterol is known as ‘good’ cholesterol, because high levels of HDL seem to protect

against heart attack. Low levels of HDL also increase the risk of heart disease.

Medical experts think that HDL tends to carry cholesterol away from the arteries and back to the

liver. Some experts believe that HDL removes excess cholesterol from arterial plaque, slowing its

buildup.

References:

http://health.howstuffworks.com/cholesterol1.htm

http://www.americanheart.org/presenter.jhtml?identifier=512

http://www.scientificpsychic.com/health/lipoproteins-LDL-HDL.html

Insulin

Glucose provides energy to all of the cells in the body. The cells take in glucose from the blood and

break it down for energy. The glucose in the blood comes from food.

When a person eats food, glucose gets absorbed from the intestines and distributed by the

bloodstream to all of the cells in the body. The body tries to keep a constant supply of glucose for

the cells by maintaining a constant glucose concentration in the blood. So, when there is an

oversupply of glucose, the body stores the excess in the liver and muscles by making glycogen, long

chains of glucose. When glucose is in short supply, the body mobilizes glucose from stored

glycogen and / or stimulates the person to eat food.

To maintain a constant blood-glucose level, the body relies on two hormones produced in the

pancreas that have opposite actions: insulin and glucagon.

Insulin consists of two polypeptide chains, an A chain and a B chain, joined together by disulphide

bonds. The smaller of the two chains is referred to as the A chain and is 21 amino acids long in

humans. The second chain is referred to as the B chain and is 30 amino acids long in humans.



Source: http://www.chemistryexplained.com/Hy-Kr/Insulin.html

Functions of insulin

Insulin is required by almost all of the body’s cells, but its major targets are liver cells, fat cells and

muscle cells. For these cells, insulin does the following:

• stimulates the liver and muscle cells to store glucose in glycogen;

• stimulates the fat cells to form fats from fatty acids and glycerol;

• stimulates the liver and muscle cells to make proteins from amino acids;

• inhibits the liver and kidney cells from making glucose from intermediate compounds of

metabolic pathways (gluconeogenesis).

Diabetes

Diabetes is classified into three types: Type 1, Type 2 and gestational diabetes.

Type 1 is caused by a lack of insulin. This type is found in 5 – 10% of diabetics and usually occurs

in children or adolescents.

Type 2 occurs when the body does not respond or cannot use its own insulin. Type 2 occurs in 90 –

95% of diabetics and usually occurs in adults over the age of 40, most often between the ages of 50

and 60.

Gestational diabetes can occur in some pregnant women and is similar to Type 2 diabetes. During

pregnancy, several hormones partially block the actions of insulin, thereby making the woman less

sensitive to her own insulin.

References:

http://health.howstuffworks.com/diabetes1.htm



http://www.vivo.colostate.edu/hbooks/pathphys/endocrine/pancreas/insulin_struct.html

http://www.providence.edu/chm/kcornely/Case%204_%20The%20structure%20of%20insulin.pdf

Casein

Milk is a complex biological fluid with high amount of proteins, lipid and minerals. The function of

milk is to supply nutrients such as essential amino acids required for the growth of the newborn.

Originally, milk proteins were believed to be a simple homogeneous protein, but about a century or

more ago, milk proteins were divided into two broad classes. The first fraction, which is about 80%

of the protein in bovine milk, is called casein. The second fraction, which makes up about 20% of

protein, is referred to as whey protein, serum protein or non-casein nitrogen.

Casein exists in milk in complex groups of molecules that are called ‘micelles’.

A typical micelle contains on the order of 104 polypeptide chains of four basic types, together with

about 3 x 103 microgranules of an amorphous calcium phosphate. The micelles are polydisperse in

size and variable in composition.

Due to the importance of casein and casein micelles for the functional behaviour of dairy products,

the nature and structure of casein micelles have been studied extensively, but the exact structure of

casein micelles is still under debate.

Various models for casein micelle structure have been proposed. Most of the proposed models fall

into three general categories: coat-core, subunit (sub-micelles), and internal structure models.

Functions of casein

The casein micelle is an important and characteristic macromolecular assembly of mammalian

biology, occurring in all milks that have been examined in sufficient detail. Its functions, insofar as

they are known, are to form a coagulum in the stomach of the nursling, allowing the slow release of

nutrients down the digestive tract, and to act as a means of transporting calcium and phosphate in a

readily assimilable form from mother to young. As well as providing a source of amino acids,

enzymatic cleavage of casein polypeptide chains can produce various types of biologically active

peptides.

Another recent speculation is that casein has a role in protecting the mammary gland against ectopic

calcification, a hazard that is common to all tissue in contact with supersaturated calcium solutions.

References:

http://www.nzic.org.nz/ChemProcesses/dairy/3E.pdf

http://books.google.com.hk/books?

id=9H_gemXpEWQC&pg=PA63&lpg=PA63&dq=structure+of+CASEIN&source=bl&ots=mxmH

460AUp&sig=M-EfF2UOtYlYE9E6L-MUH3YTQzw&hl=zh-

TW&ei=KaL8S_T7N4uTkAWGi9iMBw&sa=X&oi=book_result&ct=result&resnum=10&ved=0C

DcQ6AEwCTge#v=onepage&q=structure%20of%20CASEIN&f=true

http://rdo.psu.ac.th/sjst/journal/27-1-pdf/19casein-micelle.pdf



Unit-end exercises (pages 255 – 267)

Answers for the HKCEE (Paper 1) and HKALE questions are not provided.

1 a) i) B

ii) A

b)

2 When we add a detergent solution to a table cloth stained with grease, the hydrocarbon ‘tails’ of

the detergent particles dissolve in the grease. The anionic ‘heads’ of the detergent particles are

insoluble in the grease and remain outside.

The surrounding water molecules attract the anionic ‘heads’ and lift the grease off the surface.

By stirring, the grease (which carries the dirt particles) breaks up into tiny droplets suspended in

the water. These tiny droplets cannot come together again due to the repulsion between the

anionic ‘heads’ of detergent particles on their surfaces. An emulsion forms.

Rinsing washes away the greasy suspension, and leaves the surface clean.

3 a) A hexane-1,6-dioic acid

B hexane-1,6-diamine

b) Condensation polymerization

c)

4 a)

b) i)

ii) Condensation polymerization

c) Fibres used to make clothes

Bottles for carbonated drinks



d) By the hydrolysis of the ester linkage by enzymes or microorganisms

5 Carbonyl group

Hydroxyl group

6 B

7 B

8 B

9 B

10 B (1) X is a condensation polymer.

(2) X is formed from the condensation polymerization of two different monomers.

11 —

12 —

13 —

14 a) Little / no lather

Scum

b) Add dilute nitric acid followed by silver nitrate solution.

A white precipitate forms.

c) There are several ions that would give a colour flame.

15 a) Ester functional group; carbon-carbon double bond

b) i) Saponification

ii) First gently heat, while stirring, a mixture of vegetable oil and concentrated sodium

hydroxide solution for about 20 minutes. Most of the soap formed dissolves in the

reaction mixture.

Then add concentrated sodium chloride solution to the mixture. The soap separates from

the solution and floats on the surface.

Obtain the soap by filtration. Then wash the soap with a little distilled water and allow to

dry.

c) Hydrogenation of vegetable oils

d) Hydrocarbons from petroleum, concentrated sulphuric acid and sodium hydroxide



e) Bacteria use up oxygen in the water during the decomposition of detergents. This makes the

water of some streams, rivers and seas smell badly due to oxygen depletion.

16 a)

b) When the soap is added to hard water, scum forms.

The scum forms because the calcium and magnesium ions in hard water react with the soap,

giving an insoluble product that floats on the water.

c) Washing soda reacts with calcium ions and magnesium ions in hard water to form insoluble

carbonates, thus removing the hardness of water.

17 a) i) Carbon and hydrogen

ii)



iii) Permanent dipole-permanent dipole attractions

iv) Reflux glycerol and carboxylic acid in the presence of concentrated sulphuric acid.

b) i) Hydrogen bonding is the attraction between the hydrogen atom attached to an oxygen

atom and the lone pair on another oxygen atom.

ii) Glycerol is soluble in water because its molecules can form many hydrogen bonds with

water molecules.

The boiling point of a compound depends on the strength of its intermolecular

attractions.

Strong hydrogen bonds exist in glycerol.

Hence a lot of heat is needed to separate the glycerol molecules during boiling.

Thus glycerol has a relatively high boiling point.

c) i) Propene

ii) Petroleum

iii) Substitution

iv) Sodium hydroxide solution

v)

vi) Number of moles of compound A =

= 0.71 mol

Theoretical yield of glycerol = 0.71 mol x 92.0 g mol–1

= 65 g


30 g42 g mol–1


Percentage yield of glycerol = x 100%

= 3%

18 a) Monomer molecules join together repeatedly to form polymer molecules.

Small water molecules are formed during the reaction.

b)

c)

19 a)

b) i)

(any one of the hydrogen bonds is acceptable)

ii) Strong hydrogen bonds hold the polymer chains and water molecules together.

c) i) Permanent dipole-permanent dipole attractions exist between chains of the polymer

derived from compound A while hydrogen bonds exist between chains of the polymer

derived from compound B.

Hence chains of the polymer derived from compound A can slide past one another more

easily.

Thus the polymer is more flexible.


2 g65 g


ii)

iii) No

The polymer does not contain carbon-carbon double bond.

20 a) Any one of the following:

• To improve the quality.

• To reduce cost.

• The demand is greater than the nature can supply.

b)

c) i) butane-1,4-diamine

ii) Any two of the following:

• Lower melting point

• Lower strength

• Lower rigidity

d) i) Number of repeating units =

= 151

ii) Amide functional group

iii) The number of hydrogen bonds per unit length of polymer chain of Stanyl is greater than

that of nylon-6,6.

Hence more heat is needed to overcome the forces between the polymer chains of

Stanyl, enabling the chains to move over one another.

e) i)


3 x 104

198.0


ii)

(any one of the hydrogen bonds is acceptable)

21 a) Number of moles of CO2 produced by 0.10 g of Z =

= 2.2 x 10–3 mol

Mass of C in 0.10 g of Z = 2.2 x 10–3 mol x 12.0 g mol–1

= 0.026 g

Mass of H in 0.10 g of Z = 0.020 g x

= 2.2 x 10–3 g

Mass of O in 0.10 g of Z = (0.10 – 0.026 – 2.2 x 10–3) g

= 0.072 g

the empirical formula of Z is CHO2.


53 cm3

24 000 cm3 mol–1

2.0 g mol–1

18.0 g mol–1


b) Let (CHO2)n be the molecular formula of Z.

Molar mass of Z= n(12.0 + 1.0 + 2 x 16.0) g mol–1

= 90.0 g mol–1

n = 2

∴ the molecular formula of Z is C2H2O4.

c) Number of moles of 0.900 g of Z =

= 0.0100 mol

Number of moles of NaOH required for complete neutralization

= 1.00 mol dm–3 x dm3

= 0.0200 mol

0.0100 mole of Z requires 0.0200 mole of NaOH for complete neutralization.

i.e. 1 mole of Z requires 2 moles of NaOH for complete neutralization.

It can be deduced that Z should contain two –COOH groups.

the structural formula of Z is .

d) W CH2=CH2

X BrCH2CH2Br

Y HOCH2CH2OH

e) C20H42 C18H38 + C2H4

22

23 —

24 —

25 —


0.900 g90.0 g mol–1

20.01 000

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