Epsom Spa Epsom and Ewell History Explorer Epsom Spa A modern day photo of Epsom Wells From the early seventeenth century, places in Britain were promoted as spas. People flocked to places where such waters were readily available and inns and taverns were required to put up the visitors, while diversions and entertainments for the visitors usually developed as well. One of the earliest of these places was Epsom. Tradition told how the healing powers of the waters were discovered in 1618 or thereabouts. A villager called Henry Wicker was looking after animals on Epsom Common in a dry summer, when there was a shortage of water for cattle. He found a trickle of water in the hollow hoofprint of a cow, and dug a square hole about it before taking the animals home for the night. Returning the next day he found the hole that he had made was full and running over with clear water. But his cattle, however thirsty, would not drink from it because of its mineral taste. Wicker tried the water himself, and was the first person in history to experience the effects of Epsom salts. Enthusiastically, he set about promoting the waters as a medicine.

By the Commonwealth period, Epsom already had some of the attractions of a spa town. In 1656, gentlemen from as far away as Rutland and Cornwall were coming to spend a week at Epsom, usually in August when it was most popular. An artist's impression of Epsom Common with an early well building After the Restoration of Charles II a Dutch visitor, William Schellinks, came to the Wells. 'Epsom' he wrote, 'is a very famous and much visited place, very pleasant, and that because of the water which lies not far from there in a valley, which is much drunk for health reasons, having purgative powers, being sent in stoneware jars throughout the land, being a spring, and is with a wall around enclosing a raised well, and the ground paved with bricks. It has in the middle an opening in the ground for the water flow. This well stands at the rear of a small house in which there are some small rooms, and many people come there to drink, also to shelter from the sun. The practice of the drinking of the water is early in the morning and from then until 8, 9, 10 o'clock.

It is drunk on an empty stomach from stoneware mugs holding about one pint. Some drink ten, twelve, even fifteen or sixteen pints in one journey, but everyone as much as he can take. And one must then go for a walk, works extraordinarily excellent, with various funny results. Gentlemen and ladies have their separate meeting places, putting down sentinels in the shrub in every direction. It has happened that the well is drunk empty three times in a morning, in hot and dry summers when the water has more strength. And the people who observe this come then in such crowds that the village which is fairly large and can spread at least 300 beds, is still too small and the people are forced to look for lodgings in the neighbourhood. Some stay there on doctor's orders for several weeks continuously in the middle of the summer, drinking daily from this water, and many people take after the drinking some hot meat broth or ale.' A painting of the well building in 1795 In the late 1600s the well was housed in a little building on the Common but a new Lord of the Manor, John Parkhurst, took over in 1707 and had better premises built.

The Wells were located in a large light brick built room .There was a coffee house, two rooms for 'gameing' and shops selling' sweetmeates' and 'fruite'. Detail from the 1866 survey OS Map - Click image to enlarge 1692 two London goldsmiths acquired the bowling green site on the corner of South Street and the High Street, and erected premises known as the New Tavern and Assembly Rooms, subsequently Waterloo House. This provided facilities for dining, dancing, gambling and meeting people; there was also a coffeehouse opening onto the street, and in the gardens at the back was the bowling green and a cockpit. The bowling green and cockpit have long gone but the original building has been acquired by Wetherspoons and the name 'The Assembly Rooms' restored. Around 1699 a second well was sunk to the west of the town, on land owned by a Mr. Symonds. This was near the public house to the west of South Street, known since at least 1755 as the Magpie but renamed Symonds Well in 1996.

The discovery that water laden with Epsom salts could be found nearer the town inspired a local entrepreneur, John Livingstone, an apothecary who had recently moved into the town. A hand tinted line drawing of the well buildings taken from a book by Henry Pownall on the history of Epsom c.1825 After he had discovered that the mineral waters could be obtained to the west of the town, he started buying property in the area: first a little land near Symonds Well, and later some larger plots in 'Shoulder of Mutton Close', which lay between the present West Street, High Street and South Street. He started building there and in 1707 advertised his development as the New Wells, to be opened that Easter. 'There are Shops now to be Let at the said Wells for a Bookseller, Pictures, Haberdasher of Hats, Shoomaker, Fishmonger and Butcher, with Conveniences for several other Trades. It is design'd that a very good Consort of Musick shall attend and play there Morning and Evening during the Season and nothing will be demanded for the Waters drank there'.

The gaming and dancing were to take place in a new Assembly Room - the third to be provided in Epsom, following the ones on the Common and in Waterloo House. Like the New Tavern complex, which was just on the other side of South Street, Livingstone's New Wells had a bowling green, gardens, and a coffeehouse next door (now the Albion). These stood on the rising ground behind the so-called Old Manor House in West Street, and were entered from an alley still to be seen alongside the Albion Hotel. Livingstone's enterprises must have prospered, since he was later able to give the land in East Street on which almshouses for 12 poor widows were built. This may have been intended to secure his reputation, because there were rumours of sharp practice about some of Livingstone's dealings. After opening the New Wells, he rented the site of the Old Wells on the Common, and although he ran both sites for a few years, he then closed down the earlier site - thus eliminating the main competition to his own facilities. But the public did not seem to mind: they were too busy enjoying the social life in the heart of the town.

The Height of the Fashionable Spa A drawing of Epsom High Street showing the Assembly Rooms on the right and the white painted old clock house left of centre. c.1837 Image courtesy of Surrey Libraries and is held in the Epsom & Ewell Local And Family History Centre Collection ((External Links open in a new window) Celia Fiennes (1662-1741) travelled to improve her health, visiting many spa towns. She wrote that in the summer 'Monday is the highday in Epsom' - Monday was in fact the ordinary day for the kinds of recreation not permitted on Sunday, until the later invention of the weekend. There is 'raceing of boyes, or rabbets, or piggs; in the evening the Company meete in the Greenes, first in Upper Green, many steps up, where are Gentlemen bowling, Ladyes walking, the benches round to sitt, there are little shopps, and a gameing or danceing-roome; the same man at the Wells keepes it, sells coffee there also'. The Upper Green was Livingstone's establishment at the New Wells.

Then the company move to the Lower Green at Waterloo House 'not far off, just in the heart of the town, its a much neater Green and warmer, the whole side of this is a very large roome with large sashe windows to the Green with cusheons in the windows and seates all along; there are two hazard-boards; at the end is a Milliner and China shop'. All the length of this building on the street ward was a kind of colonnade formed by a row of trees, cut and plaited together by the skill of local gardeners. Another visitor was the Count von Uffenbach, who came over from Germany in 1710. First he visited the old Wells, but was not impressed - they were a good quarter hour's walk from the town in a mediocre house adjoining a short covered passage where you walked up and down when drinking. The water was drunk from small nasty stoneware beakers, four to six at a time (about six pints). You did this for three days in succession; then rested a bit and repeated this a second and third time, altogether nine times. Some were purged, others vomited.

Things were altogether more pleasant at the New Wells in the town, where there is also a bowling green, billiards room and coffeehouse, but the water tasted just the same. It was not just visitors who were impressed by Epsom. The writer John Toland, who was looking for retired lodgings after an eventful career as a spy and theologian, took summer lodgings at Woodcote when the first quality houses were being built there, between 1710 to 1718. He was full of praises for Epsom; it reminded him of the civilised towns where he had stayed in Holland, rather than the crude English countryside. The place was much frequented for its most healthy air and excellent mineral waters, and he described it as full of convenient houses in the latest style built for the entertainment of strangers, set in a beautiful countryside, with tree shaded side walks where you may meet the people you expect at the Exchange or St. James' Park. The two bowling greens at Waterloo house and the New Wells kept up a friendly competition with each other, and there was music playing most of the day.

A fairer circle of people was never seen in the continental spas of the time than could be admired on the High Green or Long Room, where a young man can easily find a blooming beauty. Doctors, instead of prescribing the waters for the vapours or the spleen, told their patients to get involved instead in the entertainments and enjoy themselves in the shops, the taverns, inns and coffeehouses, 'which latter for social virtue are equalled by few'. Coffeehouses were still a novelty then, and very fashionable. An early photograph of Epsom High Street with the Assembly Rooms with railings on the left. c.1890 Image courtesy of Surrey Libraries and is held in the Epsom & Ewell Local And Family History Centre Collection ((External Links open in a new window) Epsom's position as a Spa was always under threat. Other sites were soon developing, with better facilities. Bath and Tunbridge both had the patronage of Catherine de Braganza and the vogue for Bath became almost universal. Places near London were looked down on, whatever the qualities of their water, and those that were further away had a better social cachet.

Daniel Defoe said 'the nobility and gentry go to Tunbridge, the merchants and rich citizens to Epsom ... the common people chiefly to Dulwich and Streatham'. Epsom had another disadvantage - its water supply was limited and the scraping of the bottom often made it cloudy. There were also suspicions of dilution. Celia Fiennes on her first visit says: 'its not a quick spring and very often is dranke drye, and to make up the defficiency the people do often carry water from common wells to fill this in a morning (this they have been found out in) which makes the water weake and of little operation'. It is not surprising that Epsom could not compete with places where there was an abundance of water - like Bath, Buxton, Cheltenham, Harrogate, Leamington, Malvern, Tenbury, Woodhall, to name but a few, mostly discovered long after Epsom had started the fashion. Starting with Nehemiah Grew in 1695, chemists had established what gave Epsom's water its medicinal quality, and Epsom Salts were soon cheaply available over their counters.

This meant that there was no longer any need to go to the town for them, especially as the quantities of water from the two Epsom Wells were never large enough for manufacturing on any scale. With Livingstone's death in 1727, Epsom lost its most successful marketing director and the decline set in. By 1738, an updated edition of Defoe's tour cut out his enthusiastic description of the entertainments, saying that Epsom used to be frequented a few years ago on account of the mineral waters, but is now a town of fine houses, retreats for London merchants. The assembly rooms and other public buildings had fallen into decay, and only one house remained occupied at the Old Wells, from which a man and his wife carried the water in bottles to adjacent places. It is clear from a manorial survey of 1755 that the entertainment centres had all closed down by that date, their greens becoming yards for smiths or coopers. Many of the lodging houses took on the appearance of slum tenements, as their rooms were let out permanently to workmen and their families.

Local people did not know who to blame, although by the 1760s there was a vigorous tradition that Livingstone, far from having founded the Spa, had helped to ruin it by adulterating the waters. This was rather unfair, if only because the waters had never been the main reason for coming to the town. Commercially, Epsom did not suffer too much from the loss of the Spa, since the early eighteenth century had seen many houses built for the gentry in Woodcote, and these continued to provide employment for the locals. It may be that these resident clergy and stockholders actively discouraged further use of the Spa facilities, suspecting that they might appeal to a lower-class market like those at Hampstead or Islington, and so lower the tone of the town. At some stage in the early 20th century the well was capped But many visitors had realised the attractions of Epsom as a place to live. It was so near to London, and so healthy; besides, there were the Downs nearby, with the attraction of horseracing. The streets contained many fine houses of gentry and London merchants, some of whom commuted daily to London.

Of all this the New tavern coffeehouse and long room survive- a fine building of the late 17th century on the south end of the High Street. It had, and still has, sash windows - still a bit of a novelty at the time. By 1755 the property had become disused: it was divided up, at first into houses, and then converted into shops. A series of drapers, beginning with Baileys in the early 19th century, and followed by Oldridge and Wheelers, ran a high class establishment here, while the original pleasure grounds were used by blacksmiths and as a furniture yard - after a spell as a car park, this area is now built over by the Ashley Centre. The main building was substantially conserved and rebuilt by Elys in 1952: they retained original features, such as the archway for the central carriage drive, through which vehicles would pass to drop off visitors in comfort within the building. , More recently the building has reverted to its old name, 'The Assembly Rooms', and a similar use to that of its original purpose, a place where individual's can obtain refreshment.

The well head is revealed during the 1990's building work to replace the well cap This article is taken from an account written by Jeremy Harte, Curator of Bourne Hall Museum who based his account on some original research of Maurice Exwood. Images: Unless otherwise indicated all images are courtesy of Jeremy Harte, Curator, Bourne Hall Museum . Epsom Salts Epsom Salts Millions of people the world over must have asked at the chemist for Epsom Salts, and used it with recognisable effect, without knowing anything about the place that gave it its name. Nehemiah Grew established the name in his book on the 'bitter purging salts', as he named them, in 1695. The quantities of water from the two Epsom Wells were never large enough for manufacturing on any scale. He was granted a Royal patent for 'The Way of Makeing the Salt of the Purging Waters perfectly fine... very cheape'. This meant that he had the exclusive right to manufacture Epsom Salts. Grew set up this manufacture at Acton Well where he hoped to make 20,000 lbs. per year at a substantial profit.

But Francis Moult, a chemist who had published the unauthorised translation from Latin of Grew's book, claimed that he had been manufacturing and selling the salts for years. He was using the water of Shooter's Hill Well and undercut Grew's price. In 1754 bottled Epsom water was being sold at the 'Mineral Water Warehouse' in Fleet Street, as well as Epsom Salts. These were also available from Morris' coffee house at Epsom (now the Albion Hotel). As early as 1723 the Royal Society had a report from John Brown that it was being manufactured from the bitterns left after crystallisation of common salt from seawater at Portsmouth, Leamington and Newcastle - in other words, as a by-product of manufacture of common salt. John Brown tested these products and compared them with the real thing, which he obtained from his friend Mr Hyet, an apothecary at Epsom. Mr Hyet was asked to boil down some water from the well in the town - another confirmation from chemists that Livingstone's well produced the real product.

Epsom Salts, which the Encyclopaedia Britannica calls Epsomite - or hydrated magnesium sulphate, to give it its scientific name (MgSO4·7H2O) - are also found naturally in mines and limestone caves. So despite the limited supply of water from Epsom's wells, Epsom Salts will never be in short supply. Epsom Salts are still sold, under that name, not just for the traditional purpose but as an ingredient for other useful medicaments and they are included in some rose fertilisers. This article is taken from an account written by Jeremy Harte, Curator of Bourne Hall Museum Ashtead's Mineral Spring: Magnesium, Chemical Element - water, uses, elements, examples, metal, gas, number, name PRONUNCIATION mag-NEE-zee-um Large amounts of magnesium are used to make alloys. An alloy is made by melting or mixing two or more metals. The mixture has properties different from those of the individual metals. Magnesium alloys are quite light, yet very strong. This property makes them useful in the construction of airplanes and space-craft.

About 70 percent of the magnesium compounds produced in the United States are used in the manufacture of refractory materials. A refractory material is one that can withstand very high temperatures by reflecting heat. Refractory materials are used to line the ovens that maintain high temperatures. The remaining 30 percent of magnesium compounds are used in agriculture, construction, industrial, and chemical operations. Discovery and naming Compounds of magnesium are very abundant in the Earth. Dolomite, or calcium magnesium carbonate (CaMg(CO 3 2 , is an example. Dolomite has been used as a building material for centuries. Another well-known magnesium compound is Epsom salts, or magnesium sulfate (MgSO 4 . Epsom salts are known for their soothing qualities, most notably when added to a bath. (See accompanying sidebar.) The allure of Epsom salts P erhaps the best know magnesium compound is magnesium sulfate (MgSO 4 ). It is popularly known as Epson salts. One of the earliest stories about Epsom salts dates back to 1618. The town of Epsom, in Surrey, England, was suffering from a severe drought.

A farmer named Henry Wicker brought his cattle to drink from a water hole on the town commons (central park). But the cattle would not drink the water. Wicker was surprised because he knew they were very thirsty. He tasted the water himself and found that it was very bitter. The bitterness was due to magnesium sulfate in the water. This compound became known as Epsom salts. People soon learned that soaking in the natural waters that contained Epsom salts made them feel better. The salts seemed to have properties that soothed the body. Before long, soaking in these waters became very popular. Today, Epsom salts are used in bath water. They relax sore muscles and remove rough skin. Many people believe the salts have the same relaxing effect as hot springs. Some gardeners even believe that sprinkling Epsom salts in the garden helps flowers and vegetables grow! Careful studies of magnesium and its compounds began in the middle 1700s. Scottish physician and chemist Joseph Black (1728-99) carried out some of the earliest experiments on magnesium compounds. He reported on his research in an article that became famous. Black is sometimes given credit for "discovering" magnesium because of his work with the element.

By 1800, chemists knew that magnesium was an element. But no one had been able to prepare pure magnesium metal. Magnesium holds very tightly to other elements in its compounds. No one had found a way to break the bonds between magnesium and these other elements. In 1808, English chemist Humphry Davy (1778-1829) solved the problem by passing an electric current through molten (melted) magnesium oxide (MgO). The current caused the compound to break apart, forming magnesium metal and oxygen gas: Davy used this method to discover a number of other elements. (See sidebar on Davy in the calcium entry in Volume 1.) Like magnesium, these elements form compounds that are very difficult to break apart. An electric current provides the energy to break these compounds down into their elements. The name magnesium goes back many centuries. It was selected in honor of a region in Greece known as Magnesia. The region contains large supplies of magnesium compounds. Physical properties Magnesium is a moderately hard, silvery-white metal. It is the lightest of all structural metals. These metals are strong enough to be used to build buildings, bridges, automobiles, and airplanes.

Magnesium is easily fabricated. Fabrication means shaping, molding, bending, cutting, and working with a metal. Metals must be fabricated before they can be turned into useful products. Metals that are strong, tough, or hard are not easily fabricated. They must be converted to an alloy. A metal that is more easily fabricated (such as magnesium) is combined with them. The melting point of magnesium is 651°C (1,200°F) and its boiling point is 1,100°C (2,000°F). Its density is 1.738 grams per cubic centimeter. At high temperatures, magnesium bums with a blinding white light. Chemical properties Magnesium is a fairly active metal. It reacts slowly with cold water and more rapidly with hot water. It combines with oxygen at room temperature to form a thin skin of magnesium oxide. It burns with a blinding white light at higher temperatures. Magnesium reacts with most acids and with some alkalis. An alkali is a chemical with properties opposite those of an acid. Sodium hydroxide (common lye such as Drano) and lime-water are examples of alkalis.

Magnesium also combines easily with many non-metals, including nitrogen, sulfur, phosphorus, chlorine, fluorine, bromine, and iodine. It also reacts readily with a number of compounds, such as carbon monoxide (CO), carbon dioxide (CO 2 , sulfur dioxide (SO 2 , and nitric oxide (NO). Occurrence in nature The abundance of magnesium in the Earth's crust is estimated to be about 2.1 percent. That makes it the sixth most common element in the earth. It also occurs in seawater. A cubic mile of seawater is estimated to contain up to six million tons of magnesium. There are many naturally occurring minerals of magnesium. Some of the most important are dolomite; magnesite, or magnesium carbonate (MgCO 3 ; carnallite, or potassium magnesium chloride (KMgCl 3 ; and epsomite, or magnesium sulfate (MgSO 4 . The largest producer of magnesium ores is Turkey. Other large producers are North Korea, China, Slovakia, Austria, and Russia. The amount of magnesium produced in the United States is not reported in order to protect trade secrets.

Magnesium produced in the United States comes from three sources: seawater, brine, and mines. Seawater is processed to obtain magnesium by companies in California, Delaware, Florida, and Texas. Magnesium is obtained from brine in Michigan and Utah. Brine is water that is even saltier than seawater. Finally, some magnesium compounds are taken from mines in Nevada, North Carolina, and Washington. Isotopes There are three naturally occurring isotopes of magnesium: magnesium-24, magnesium-25, and magnesium-26. Isotopes are two or more forms of an element. Isotopes differ from each other according to their mass number. The number written to the right of the element's name is the mass number. The mass number represents the number of protons plus neutrons in the nucleus of an atom of the element. The number of protons determines the element, but the number of neutrons in the atom of any one element can vary. Each variation is an isotope. One radioactive isotope of magnesium, magnesium-28, also exists. A radioactive isotope is one that breaks apart and gives off some form of radiation. Radioactive isotopes are produced when very small particles are fired at atoms.

These particles stick in the atoms and make them radioactive. Magnesium-28 has no important commercial uses. Extraction Magnesium is prepared by one of two methods. The first method is similar to the method used by Davy in 1808. An electric current is passed through molten (melted) magnesium chloride: Magnesium alloys are often used in the production of skis. The second method involves reacting magnesium oxide with ferrosilicon. Ferrosilicon is an alloy of iron and silicon. When magnesium oxide and ferrosilicon react, free magnesium metal is formed. Uses Although most cameras now use electronic flashes, magnesium metal is often contained in cameras that use flash bulbs. A thin strip of magnesium metal is inside the bulb. When the Magnesium alloys are used in power tools, such as the reciprocating saw shown here. flash is ignited, the magnesium strip catches fire. It burns with a very bright white light. The light from the bulb illuminates a scene for the photograph. A common use of magnesium metal is in fireworks. Most firework displays include some brilliant flashes of very white light. Those flashes are produced by the burning of magnesium metal. Magnesium is commonly alloyed with other metals.

Magnesium and aluminum, for instance, are two metals that combine to form alloys that are very strong and resistant to corrosion (rust). But they weigh much less than steel alloys with similar properties. Strength and low density are important properties in the manufacture of airplanes, automobiles, metal luggage, ladders, shovels and other gardening equipment, racing bikes, skis, race cars, cameras, and power tools. A typical magnesium alloy contains about 90 percent magnesium, 2 to 9 percent aluminum, and small amounts of zinc and manganese. Compounds The largest single use of magnesium compounds is in refractories.

Other magnesium compounds are used in the following categories: medicine: pain killer and fever reducer (magnesium acetylsalicylate); antacid to neutralize stomach acid (magnesium hydroxide; magnesium phosphate; magnesium silicate); laxative to loosen the bowels (magnesium carbonate; magnesium chloride; magnesium citrate; magnesium hydroxide; magnesium lactate; magnesium phosphate); antiseptic to kill germs (magnesium borate; magnesium salicylate; magnesium sulfate); sedative to help one get sleep (magnesium bromide) production of glass and ceramics: magnesium fluoride; magnesium oxide mothproofing of textiles: magnesium hexafluorosilicate fireproofing wood for construction: magnesium phosphate manufacture of paper: magnesium sulfite Health effects Magnesium is essential for good health in both plants and animals. It forms part of the chlorophyll molecule found in all green plants. Chlorophyll is the molecule in green plants that controls the conversion of carbon dioxide and water to carbohydrates, such as starch and sugar. Plants that do not get enough magnesium cannot make enough chlorophyll. Their leaves develop yellowish blotches as a result. Magnesium is found in many enzymes in both plants and animals.

An enzyme is a catalyst in a living organism. It speeds up the rate at which certain changes take place in the body. Enzymes are essential in order for living cells to function properly. It is difficult not to get enough magnesium in one's daily diet. It is found in nuts, cereals, seafoods, and green vegetables. Most people have no problem getting the 300 to 400 milligrams of magnesium recommended in the daily diet. Magnesium forms part of the chlorophyll molecule found in all green plants. A lack of magnesium can occur, however. For example, alcoholics and children in poor countries sometimes develop a magnesium deficiency. In such cases, magnesium deficiency may cause a person to become easily upset or overly aggressive. On the other hand, it is also possible to be exposed to too much magnesium. For example, inhaling magnesium powder can produce irritation of the throat and eyes, resulting in a fever. In large doses, magnesium can cause damage to muscles and nerves. It can eventually result in loss of feeling and paralysis (inability to move parts of the body). Such conditions are rare. They are likely to occur only among people who have to work with magnesium metal on a regular basis.

Also read article about Magnesium from Wikipedia User Contributions: Cochise College P The term Epsom salt was coined by Grew who in 1695 named the mineral found in the bitter saline spring waters after the nearest town to its vicinity, Epsom, in Surrey, England. He also had acquired a royal patented for the collection and sale of the mineral compound. In addition, the name of the town was also derived from Ebbaï¿½s ham, Ebba was a Saxon landowner. So, what is Epsom salt? Epsomï¿½s salt, or its mineral name, Epsomite, which occurs naturally as heptahydrous magnesium sulfate mineral, a hydrated form of Magnesium Sulfate (MgSO4). Its chemical compound is magnesium, sulfur, oxygen, with seven water molecules, and the chemical formula is (MgSO4 7H2O). Epsom Salt Magnesium sulfate in its unaltered state is called anhydrous magnesium sulfate, which means having no water. Its physical appearance is that of a white powdery material. What environment does it form?

Epsom Salt, or Bitter salts, forms as a powdery, fibrous or globular crust growing as efflorescence, (flowering out), on cave walls, sulfide, coal, and metal mines from saline springs, or depositions of sulfur and magnesium-rich water due to mining operations. Salt deposits also occur among hot springs. Epsomite formations are mostly found in arid regions located in dry caves and alike which inhibits the dissolution of the mineral due to its hydrophilic personality, i.e., water soluble. It also been noticed among volcanoesï¿½ fumaroles such as Mt. Vesuvius in Italy. Epsomite also occurs in South Africa as unusual marine salt deposits that form in sedimentary beds. HOW DO EPSOM SALT CRYSTALS FORM? The forming of Epsom salt crystals is a straightforward process. A source of water is needed like a hot springs. The springs needs to be hot enough to fully dissolve the magnesium sulfate, that is, an increase of temperature also increases the amount of space between each molecule. This will create a condition of saturation is when all available space between molecules has been filled.

Later as the water cools the space decreases forcing the molecules together at which time it causes the crystals to form and separate from the water. To reference this topic along with an experiment in the process of how crystals grow view the following: H:\GEOLOGY\How Do Epsom Salt Crystals Form eHow_com.mht How is Epsom Salt obtained? Originally, Epsom salt was obtained by boiling down the mineral waters at Epsom, England; afterwards the mineral was acquired from sea water using the same methods. Ironically this method has not changed except for the material from which Epsom salt is prepared. Besides the usual sources that Epsom salt is obtained it is also prepared from other sources such as Kieserite mineral and Dolomite. Magnesium Sulfate, Epsom salt, is obtained by dissolving the mineral in water at 200oF (90oC) then allow the solution to cool thereby the process of filtration the crystals are removed. Another source is dolomite. Since Dolomite belongs to a group known as Salts, and consists of the elements calcium, magnesium, carbon, and oxygen in which it takes the form of carbonate of calcium and magnesium.

Dolomite is a suitable source to obtain Epsom salt because it consists of magnesium, sulfur, and oxygen. The process of extraction is similar. LOCATIONS EPSOM SALT IS FOUND Epsomite was found as crusts produced by thermal springs in Epsom, Surrey, England, which is the locality it is named after. It occurs in certain areas in the Sahara Desert of Africa, the desert of Central Australia, and the Atacama Desert of Chile, where it sometimes forms thick beds. In the U.S., it occurs in the saline lake beds on Kruger Mountain, near Oroville, Okanogan Co, Washington, and in the Carlsbad Caverns of New Mexico. Other occurrences are the Kalkar quarry, Santa Cruz Co., California; the White Caps mine in Manhattan, Nye Co., Nevada; Majuba Hill mine, Pershing Co., Nevada; and Bisbee, Cochise Co., Arizona. Color: Colorless, white with pale shades of pink and green. Luster: Glassy Taste: Bitter-salt Soluble in Water: Dehydrates readily in dry air but accepts moisture in humid conditions.

A fact that is a detriment to most collection specimens as they may absorb water from the air and deteriorate overtime. Fracture: Conchoidal Cleavage: Perfect in one direction and distinct in two other directions. Heat: Hydrates loses water molecules when heated: Heptahydrate loses one molecule of water at room temperature, 4 molecules of water @ 70oC (160oF), 6 molecules of water @150oC (300oF), and 7 molecule of water above 200oC (400oF). USES OF EPSOM SALT General It is used in agriculture and gardening in order to reduce the magnesium deficiency in the soil. Making bath salts. Industry, uses it in the anhydrous form. Using ï¿½ cup of Epsom salts in warm water to soak feet. A gentle exfoliation of the skin. Using 2 cups in a warm bath for better relaxation. Hair Conditioner, it adds volume to the hair. Aids in eliminating skin ailments. Medicinal Occasional constipation, taken orally as a laxative.

Arthritic pain relief and Osteoporosis make a solution of warm salts and apply it to the needed areas. Pregnant women issues, injected prevents premature birth and aids in reducing high blood pressure. The areas that Epsom salt can be used is astonishing and just too numerous to list them all, and the secret to its value? Is that Epsom salt is artificially made salt of magnesium and is forever trying to rid itself of the sulfur and join with its original partner, carbon. Because of this affinity for carbon it readily exchanges sulfur for carbon when possible. Hence this is the human bodyï¿½s cure-all because since the body takes in forms of carbons in the forms of food stuffs and breathable air it then becomes a crude form of carbon. The magnesium dumps the sulfur and connects with the carbon units thus facilitating excretion of waste products from the bodyï¿½s systems. Epsom salt truly is a Miracle Mineral. How to Find Us - Epsom United Reformed Church How to Find Us The Memory Project How to Find Us Epsom is located some 15 miles (24 km) south-west of London along the A24 London-Dorking road.

It owes its fame to two events: the discovery of health-giving waters in the seventeenth Century, which led to Epsom Salts (hydrated Magnesium Sulphate) and to its popularity as a Spa for the Court of King Charles II and others, and the founding of a race for 3yr-old horses on Epsom Downs, known as the Derby. Epsom, with the neighbouring town of Ewell, is a Borough, having received its charter in 1937. Population is around 60,000. Its name is variously said to be derived from ‘the home of Ebba’, rumoured to have been a local Anglo-Saxon Princess, hence Ebbisham, an old name for Epsom still used locally for street names and a Sports Centre; alternatively, from a water source which ran down the line of Church Street, unconnected with the Wells, that appears at intervals, always inconveniently, i.e., ebbing and flowing, at the north-eastern end of the High Street. Our Church is located in Church Street, directly opposite the Police Station, just a little north of the junction with Worple Road.

This street is well-named, being the location of three churches: our Church; Epsom Baptist Church, which about 50 metres from its junction with the High Street; and the part-15th Century Epsom Parish Church of St Martin of Tours, some two hundred metres south of our Church. Address of the church: Magnesium Compound - Magnesium Stearate Manufacturer from Mumbai Magnesium Compound Magnesium compound Magnesium Compound Leading Manufacturer of Magnesium Stearate, Magnesium Metal Powder, Magnesium Metal Turning, Magnesium Metal Ribbon, Magnesium Acetate and Magnesium Carbonate Light from Mumbai. Request Callback Magnesium Stearate Approx Price: Rs 375 / 500 Gram(s) We are engaged in offering a comprehensive range of Magnesium Stearate that is a perfect composition of chemicals. Furthermore, our range of stearate is extensively used as diluents by our clients. This stearate is hugely in demand as this is widely used for formulating, medical tablets, capsules and various types of powders. Yes!

I am Interested Approx Price: Rs 240 / 100 Gram(s) Facilitated with huge industrial expertise and understanding, we are providing Magnesium Metal Powder. Features: Hygienically processed Longer shelf life Magnesium is an alkaline earth metal that has the symbol Mg in the periodic table of elements. Magnesium is a fairly strong, silvery-white, light-weight metal (one third lighter than aluminum) that slightly tarnishes when exposed to air. In a powder, this metal heats and ignites when exposed to moisture and burns with a white flame. It is difficult to ignite in bulk, though it is easy to light if it is shaved into thin strips. Once ignited, it is difficult to extinguish. Magnesium is a brilliant white metal, which is relatively soft. It is one of the more abundant elements, there being 23000 ppm in the earth’s crust. As a powder, magnesium is extremely reactive, but as a solid it oxidises slowly in air and reacts slowly in water. It does not occur naturally, but is found in combination with other elements in minerals such as magnesite (MgCO3, primarily) and dolomite (the double carbonate of magnesium and calcium).

As with other elements in groups 1 and 2 of the periodic table, it can be produced by electrolysis of the molten halide. Magnesium is very chemically active, it takes the place of hydrogen in boiling water and a great number of metals can be produced by thermic reduction of its salts and oxidized forms with magnesium. It joins together with most non-metals and almost every acid. Magnesium reacts only slightly or not at all with most of the alkalis and many organic substances, like hydrocarbons, aldehides, alcohols, phenols, amines, esters and most of the oils. Used as a catalyst, magnesium promotes organic reactions of condensation, reduction, addition and dehalogenation. It was used for a long time for synthesizing special and complex organic components by the well-known Grignard reaction. The main ingredients of the alloys are: aluminum, manganese, zircon, zinc, rare-earth metals and thorium. Magnesium compounds are used as refractory material in furnace linings for producing metals (iron and steel, nonferrous metals), glass, and cement.

With a density of only two thirds of the aluminum’s, it has countless applications in cases where weight reducing is important, i.e. in aeroplane and missile construction. It also has many useful chemical and metallurgic properties, which make it appropriate for many other non-structural applications. Magnesium components are widely used in industry and agriculture. Other uses include: removal of sulphur form iron and steel, photoengraved plates in the printing industry; reducing agent for the production of pure and other metals from their salts; flashlight photography, flares, and pyrotechnics. Magnesium is the eighth most abundant element and constitutes about 2% af the Earth’s crust by weight, and it is the third most plentiful element dissolved in seawater. It’s very abundant in nature, and it’s found in important quantities in many rocky minerals, like dolomite, magnetite, olivine and serpentine. It’s also found in seawater, underground brines and salty layers. It’s the third most abundant structural metal in the earth’s crust, only exceeded by aluminum and iron. Yes! I am Interested Chip size: 0. 2mmx1.

5mm Packing: Well Air Tight packed in Paper Fibre Drums, Each drum Containing 25 Kgs. Expiry Date: -The Material will work fine till 8 months if kept air tight. It will expire within 3 months if exposed to air. Magnesium is 33% lighter than aluminum, 60% lighter than titanium, and 75% lighter than steel. Yet for many applications it’s stronger per unit volume than all three of those structural metals. It is also an extremely versatile metal. Besides its basic functions as a component in aluminum alloys, titanium, and steel production, magnesium can also be cast into various mechanical parts and replace aluminum alloys for virtually anything you want to make lighter and stronger. Magnesium usage is not just limited to the automotive sector. It is also generating a lot of buzz in the sports sector. It has taken high performance to a whole new level. Not only is magnesium light-weight, durable, and stronger than aluminum, but it also absorbs 16 times more shock and vibrations, making it the ideal metal that gives competitive sports that extra edge. Many motorcycle and mountain bike manufacturers have incorporated magnesium in their premium designs for years while new innovations used in the sports sectors are generating additional attention.

Skiers, snowboarders and even ice skaters now find some of their equipment made out of magnesium as it provides much better stability at higher speeds. It is also transforming the sport of golf, where drivers made with a magnesium crown are lighter with better weight distribution to allow golfers to deliver longer and more powerful drives. Many magnesium advantages are used in world economic because they can’t be realized using other materials and comparable manufacturing processes. When the die casting process reaches such a high state of perfection, there is a tendency for some to think of future progress in terms of purification. Such thinking isn’t always true. There are many things that have to be done to realize all these suggestions and aims – bigger and better casting machines, improved finishing techniques, casting of metals that have not yet been practical and so on. Yes! I am Interested Ask For Price Magnesium Acetate Anhydrous magnesium acetate has the chemical formula Mg(C2H3O2)2 and in its hydrated form, magnesium acetate tetrahydrate, it has the chemical formula Mg(CH3COO)2 • 4H2O. In this compound magnesium has an oxidation state of 2+.

Magnesium acetate is the magnesium salt of acetic acid.It is deliquescent and upon heating, it decomposes to form magnesium oxide.Magnesium acetate is commonly used as a source of magnesium in biological reactions. Yes! I am Interested Ask For Price Magnesium Carbonate Light Magnesium carbonate, MgCO3, is an inorganic salt that is a white solid. Several hydrated and basic forms of magnesium carbonate also exist as minerals. Yes! I am Interested Ask For Price Magnesium Chloride Magnesium chloride is the name for the chemical compounds with the formulas MgCl2 and its various hydrates MgCl2(H2O)x. These salts are typical ionic halides, being highly soluble in water. The hydrated magnesium chloride can be extracted from brine or sea water. In North America, magnesium chloride is produced primarily from Great Salt Lake brine. It is extracted in a similar process from the Dead Sea in the Jordan valley. Magnesium chloride, as the natural mineral bischofite, is also extracted (via solution mining) out of ancient seabeds; for example, the Zechstein seabed in northwest Europe. Some magnesium chloride is made from solar evaporation of seawater.

Anhydrous magnesium chloride is the principal precursor to magnesium metal, which is produced on a large scale. Hydrated magnesium chloride is the form most readily available. Yes! I am Interested Ask For Price Magnesium Citrate Magnesium citrate (1:1) (1 magnesium atom per citrate molecule), called below by the common but ambiguous name magnesium citrate (which can also mean magnesium citrate (3:2)), is a magnesium preparation in salt form with citric acid. It is a chemical agent used medicinally as a saline laxative and to completely empty the bowel prior to a major surgery or colonoscopy. It is available without a prescription, both as a generic and under the brand names Citromag and Citroma. It is also used in the pill form as a magnesium dietary supplement. It contains 11.3% magnesium by weight. Compared to magnesium citrate (3:2), it is much more water soluble, less alkaline, and contains 29.9% less magnesium by weight. Yes! I am Interested Ask For Price Magnesium Fluoride Magnesium fluoride is an inorganic compound with the formula MgF2.

The compound is a white crystalline salt and is transparent over a wide range of wavelengths, with commercial uses in optics that are also used in space telescopes. It occurs naturally as the rare mineral sellaite Yes! I am Interested Ask For Price Magnesium Hydroxide Magnesium hydroxide is an inorganic compound with the chemical formula of hydrated Mg(OH)2. As a suspension in water, it is often called milk of magnesia because of its milk-like appearance. The solid mineral form of magnesium hydroxide is known as brucite Yes! I am Interested Ask For Price Magnesium Nitrate Magnesium nitrate is a hygroscopic salt with the formula Mg(NO3)2. In air, it quickly forms the hexahydrate with the formula Mg(NO3)2·6H2O (and molar weight of 256.41 g/mol). It is very soluble in both water and ethanol Yes!

I am Interested Magnesium Oxide Light Approx Price: Rs 350 / 500 grams Magnesium oxide (MgO), or magnesia, is a white hygroscopic solid mineral that occurs naturally as periclase and is a source of magnesium (see also oxide). It has an empirical formula of MgO and consists of a lattice of Mg2+ ions and O2− ions held together by ionic bonding. Magnesium hydroxide forms in the presence of water (MgO + H2O → Mg(OH)2), but it can be reversed by heating it to separate moisture Yes! I am Interested Ask For Price Magnesium Oxide Heavy Magnesium oxide (MgO), or magnesia, is a white hygroscopic solid mineral that occurs naturally as periclase and is a source of magnesium (see also oxide). It has an empirical formula of MgO and consists of a lattice of Mg2+ ions and O2− ions held together by ionic bonding. Magnesium hydroxide forms in the presence of water (MgO + H2O → Mg(OH)2), but it can be reversed by heating it to separate moisture Yes!

I am Interested Ask For Price Magnesium Phosphate Magnesium phosphate is a general term for salts of magnesium and phosphate appearing in three forms: Monomagnesium phosphate (Mg(H2PO4)2)Dimagnesium phosphate (MgHPO4)Magnesium phosphate tribasic (Mg3(PO4)2)Various forms have been used as laxatives and antacids Yes! I am Interested Ask For Price Magnesium Sulphate Heptahydrate Magnesium sulfate (or magnesium sulphate) is an inorganic salt (chemical compound) containing magnesium, sulfur and oxygen, with the formula MgSO4. It is often encountered as the heptahydrate sulfate mineral epsomite (MgSO4·7H2O), commonly called Epsom salt, taking its name from a bitter saline spring in Epsom in Surrey, England, where the salt was produced from the springs that arise where the porous chalk of the North Downs meets non-porous London clay. Yes! I am Interested Ask For Price Magnesium Sulphate Dried Magnesium sulfate (or magnesium sulphate) is an inorganic salt (chemical compound) containing magnesium, sulfur and oxygen, with the formula MgSO4.

It is often encountered as the heptahydrate sulfate mineral epsomite (MgSO4·7H2O), commonly called Epsom salt, taking its name from a bitter saline spring in Epsom in Surrey, England, where the salt was produced from the springs that arise where the porous chalk of the North Downs meets non-porous London clay. Yes! I am Interested Ask For Price Magnesium Trisilicate Magnesium trisilicate is an inorganic compound that is used as a food additive. The additive is often employed by fast food chains to absorb fatty acids and remove impurities that form in edible oils during the frying process Yes! I am Interested Tell Us What You Are Looking For? Website: Epsom Epsom 18.04 km2 (6.97 sq mi) Population Epsom () is a market town in Surrey , England, 13.6 miles (21.9 km) south south-west of London , located between Ashtead and Ewell . The town straddles chalk downland ( Epsom Downs ) and the upper Thanet Formation .

Epsom Downs Racecourse holds The Derby , now a generic name for sports competitions in English-speaking countries. The town also gives its name to Epsom salts , extracted from mineral waters there. Epsom is the source of the Hogsmill River and includes the semi-rural Horton and Langley Vale. Contents 14 External links History Epsom is famous for the Epsom Downs Racecourse which hosts the Epsom Derby; painting by Théodore Géricault , 1821. Lord Rosebery Epsom lies within the Copthorne hundred used for periodic, strategic meetings of the wealthy and powerful in Anglo Saxon England , and later having a Hundred Court . The name of Epsom is early recorded as forms of Ebba’s ham (home or perhaps manor ). [2] Ebba was a Saxon landowner. Many Spring line settlements by springs in Anglo-Saxon England were founded at the foot of dry valleys such as here and Effingham , Bookham , Cheam , Sutton , Carshalton , Croydon and Bromley . A relic from this period is a 7th-century brooch found in Epsom and now in the British Museum .

Chertsey Abbey , whose ownership of the main manor of Ebbisham was confirmed by King Athelstan in 933, asserted during its Middle Ages existence that Frithwald and Bishop Erkenwald granted it 20 mansas of land in Epsom in 727. [2] Epsom appears in Domesday Book of 1086 as Evesham, held by Chertsey Abbey . Its domesday assets were: 11 hides ; 2 churches, 2 mills worth 10 shillings , 18 ploughs , 24 acres (97,000 m2) of meadow , woodland worth 20 hogs ; altogether it rendered £17 per year to its overlords. [3] The town at the time of Domesday Book had 38 households (and 6 serfs noteworthy enough to be recorded as assets), some of them in a nucleated village near the parish church of which there were two. [4] At various dates in the Middle Ages manors were founded by subinfeudation at Epsom Court, Horton , Woodcote, Brettgrave and Langley Vale .

[2] Under Henry VIII and Queen Mary the manor passed to the Carew then related Darcy families. It passed via the Mynne, Buckle and Parkhurst families to Sir Charles Kemys Tynte and after his death to Sir Joseph Mawbey . By the end of the Georgian period , Epsom was known as a spa town . Remnants of this are its water pump and multiple exhibits in the town’s museum. There were entertainments at the Assembly Rooms (built c. 1690 and now a pub). A green-buffered housing estate has now been built upon the wells in the south-west of the town. Epsom salts are named after the town. Epsom salt ( magnesium sulphate ) was originally prepared by boiling down mineral waters which sprung at Epsom. What was in the Middle Ages the town pond has become the town’s market . Within the centuries-old boundaries is Epsom Downs Racecourse which features two of the five English Classic horse races; The Derby and The Oaks, which were first run in 1780 and 1779 respectively.

On 4 June 1913, Emily Davison , a militant women’s suffrage activist, stepped in front of King George V ‘s horse running in the Derby, sustaining fatal injuries. The British Prime Minister and first chairman of the London County Council , Lord Rosebery , was sent down (expelled) from the University of Oxford in 1869 for buying a racehorse and entering it in the Derby − it finished last. Lord Rosebery remained closely associated with the town throughout his life, leaving land to the borough, commemorated in the names of Rosebery Park and Rosebery School . A house was also named after him at Epsom College , one of Britain’s public schools in Epsom. The New Student’s Reference Work of 1914 describes Epsom: [5] “ Ep′som, a small town market of Surrey, England, fifteen miles southwest of London. The springs which made Epsom so fashionable a resort in the latter half of the 17th century, gave name to the Epsom salt, formerly made from them. The church, rebuilt in 1824, contains monuments by Flaxman and Chantrey .

On Banstead Downs, one and a half miles south of the town, the most famous horse-races of the world are held yearly on Derby day. The grand stand was built in 1829–30 at a cost of $100,000, and seats 7,500 spectators. Population, 10,915. ” Town Hall, The Parade St Martin of Tours Church, Epsom Epsom Clock Tower was built in 1847, replacing the watchhouse which stood from the 17th century, and was built to 70 feet of red and suffolk brick, with heraldic lions of Caen Stone at the four corners of the tower base. A bell was added in 1867. By 1902 the lions had been replaced by lanterns, (which were replaced by the current globe lights in 1920) and the toilet buildings added either side of the tower.

[6] Owing partly to its position and transport infrastructure in the London commuter belt allowing easy access to the Greater London conurbation to the north and the rolling Surrey countryside to the south, the borough of Epsom and Ewell was named in August 2005 by Channel 4 ‘s Location, Location, Location as the “Best Place to Live” in the United Kingdom, and ranked at numbers 8 and 3 in subsequent years. [7] [8] The Epsom Playhouse was opened in 1984 and is run by Epsom and Ewell Borough council. [9] The Ashley Centre , a shopping mall, was built in the early 1980s and subsequently parts of the high street were pedestrianised as part of the construction of the town’s one-way system. In the 1990s, a large multiplex Odeon cinema was built in Upper High Street.

The late 1990s saw the development of the Ebbisham Centre (not to be confused with the nearby early 18th century Ebbisham House), a community service based development, including a doctors’ surgery, Epsom Library, a cafe and a health and fitness centre. The Derby Square expanded and includes a number of franchise chain pubs/bars. The University for the Creative Arts has one of its five campuses in Epsom. Laine Theatre Arts , an independent performing arts college, is based in the town. Students have included Victoria Beckham . Leisure facilities in and around the town include a leisure centre (the Rainbow Centre) on East Street; Epsom Downs Racecourse ; the Odeon cinema; and the Horton Park Children’s Farm. Major employers in the town include Epsom and Ewell Borough Council and WS Atkins . As part of Epsom and Ewell, the town is twinned with Chantilly in northern France. Epsom and Ewell was ranked in the top ten of the Halifax Quality of Life Survey 2011. [10] Sport and leisure Epsom has a Non-League football club Epsom & Ewell F.C.

who currently share a ground with Merstham F.C. , as they sold their original ground off West Street. They are currently looking to move back into the Epsom area. [11] Geography Soil and elevation The town is bisected in two in terms of soil: the north of the town is on gravel and sand deposited around the London Clay of most of London as the Thanet Formation , whereas the south-east of the town is on uneroded chalk slopes: Epsom Downs refers to these slopes reaching up to wide plateau (on which sit the formerly water-scarce settlements: Box Hill , Walton on the Hill , Tadworth and Kingswood, Surrey ) and covers 990 acres (400 ha) of what is in traditional terms and in technical terms, part of the area of the settlement, called Epsom Downs. [2] In terms of topsoil, the northern soil is free draining, slightly acid but base-rich soils, producing extremely fertile pastures and deciduous woodland.

The southern soil is of two types: shallow, lime-rich soil over chalk or limestone of the escarpment slightly acid, loamy and clayey soils with impeded drainage soil [12] The town’s clustered bulk is at 35m to 70m (above Ordnance Datum , mean sea level) and slopes incrementally from south and all other directions (to a lesser extent) towards the centre-north. The racecourse and Langley Vale parts of Epsom rise to high points of 140m and form a drainage divide between tributaries of the Thames flowing north and towards the Mole Gap south-west.

[13] Nearest settlements Horton Hospital [16] (1903) Long Grove Hospital [17] (1907, an exact duplicate of Horton Hospital to save construction time) West Park Hospital [18] (construction started 1912, used as a military hospital from 1916 and officially opened in 1921) The hospitals were built in close proximity to each other on a 1,096-acre (4.44 km2) estate on part of Epsom Common , which the London County Council bought to solve the overcrowding problems experienced in its other hospitals. The hospitals shared a central ‘engineering works’ next to Long Grove, which supplied all five institutions with water and electricity and were served by the private Horton Light Railway . Today, of the former hospitals, three have been largely redeveloped for housing (Horton, The Manor and Long Grove Hospital) and two are in the process of being redeveloped while retaining limited NHS services including day care and a cottage hospital. [19] The surrounding land has now become the Horton Country Park and is also home to the Hobbledown Children’s Farm.

[20] Localities Epsom is contiguous apart from the neighbourhoods or localities below. Horton Horton covers the slightly elevated westernmost part of the borough. Suburban and rural, it is centred on Horton Lane, a wide road with gentle bends, 1.5 miles (2.4 km) in length with a 40 mph speed limit one of two routes between Chessington (including Hook) and the West Ewell-Epsom conurbation as an alternative route to Hook Road (the B284). It was a manor of the parish and remains a hamlet of the town as well as not qualifying for post town status. The place-name Horton is a common one in England. It derives from Old English horu ‘dirt’ and tūn ‘settlement, farm, estate’, presumably meaning ‘farm on muddy soil’. [21] Formerly around it were a group of psychiatric hospitals which served London and Surrey, forming a socially distanced community and pre-dated the United Kingdom’s shift to care in the community mental health treatments which commenced in the early 20th century.

Horton’s amenities include: Hobbledown children’s adventure park and farm Epsom Polo Club Langley Vale This locality is a sloped, developed network of streets, surrounded by steep farmland and the racecourse. Transport Remains of Epsom Town railway station Epsom railway station has frequent rail services to London and other local towns. The town’s other station, Epsom Town, was closed in 1929; although most of the listed buildings remain. The station is of historic interest being the arrival point for Queen Victoria and her entourage prior to taking a carriage up to Epsom Downs. Two other railway lines were built to serve the Epsom Downs Racecourse , with termini at Epsom Downs and Tattenham Corner . The Horton Light Railway was built around 1905, as a branch from the main line near Ewell West Station, to deliver building materials to the mental hospitals (see above) being built on what is now Horton Country Park. Bus Bus services connect Epsom to neighbouring areas and a regular service connects with the London Underground at Morden . Some bus services are commercial, some run with the support of Surrey County Council, and others under contract to London Buses .

Coach company Epsom Coaches and their bus division Quality Line are based in the town. Road The A24 passes through the centre of the town. The M25 motorway can be joined at Junction 9 Leatherhead , via the A24 south. The B280 runs from Epsom (West Hill) through Malden Rushett (A243) to Oxshott . Education Epsom College

Question: Which town in Surrey gives its name to the common form of Hydrated Magnesium Sulphate?
Answer: EPSOM