Monthly Archives: June 2013

Uranium!!

Uranium is a silvery-white metallic chemical element in the actinide series of the periodic table, with symbol U and atomic number 92. A uranium atom has 92 protons and 92 electrons, of which 6 are valence electrons. Uranium is weakly radioactive because all its isotopes are unstable. The most common isotopes of uranium are uranium-238 (which has 146 neutrons) and uranium-235 (which has 143 neutrons). Its density is about 70% higher than that of lead, but not as dense as gold or tungsten. It occurs naturally in low concentrations of a few parts per million in soil, rock and water, and is commercially extracted from uranium-bearing minerals such as uraninite.

Cubes and cuboids of uranium photographed in the 1940s.
Image: U.S. Department of Energy (public domain).

 
Uranium was named after the planet Uranus, which had been discovered eight years prior to the discovery of uranium. Uranus was named in honour of the Greek god of the sky.
 
Uranium is more abundant and widespread than most people realise — it occurs in low levels in all rock, soil, and water, and is, for example, more abundant than silver. It is the largest element found on Earth in significant quantities. In the wild, nearly all uranium is the uranium-238 (99.27%) isotope, although there are trace amounts of naturally-occurring uranium-235 and even smaller amounts of uranium-234. Uranium is radioactive and decays by emitting alpha particles (two protons and two neutrons bound together). The half-life of uranium-238 is about 4.47 billion years and that of uranium-235 is 704 million years.
 
Before it was discovered that uranium is radioactive, it was widely used to colour glass, and pottery and glazes.
 
The atomic bomb, named “Little Boy”, that was dropped on Hiroshima Japan in 1945, contained 64 kg (140 lb) of highly-enriched U-235. This bomb had an explosive energy of 16 kilotonnes of TNT, it killed an estimated 90,000–166,000 people and destroyed roughly 50,000 buildings.
 
After enrichment, the barely radioactive U-238 remains behind. Known as depleted uranium, it is used as shielding for radioactive materials, or as “high-density penetrators” — which is military talk for dense pointy projectiles that smash holes through otherwise impenetrable objects.

 

Uraninite, also known as pitchblende, is the most common ore mined to extract uranium.

A person can be exposed to uranium (or its radioactive daughters such as radon) by inhaling dust in air or by ingesting contaminated water and food. The amount of uranium in air is usually very small; however, people who work in factories that process phosphate fertilizers, live near government facilities that made or tested nuclear weapons, live or work near a modern battlefield where depleted uranium weapons have been used, or live or work near a coal-fired power plant, facilities that mine or process uranium ore, or enrich uranium for reactor fuel, may have increased exposure to uranium.
 
Houses or structures that are over uranium deposits (either natural or man-made slag deposits) may have an increased incidence of exposure to radon gas.
 
Most ingested uranium is excreted during digestion. Only 0.5% is absorbed when insoluble forms of uranium, such as its oxide, are ingested, whereas absorption of the more soluble uranyl ion can be up to 5%. However, soluble uranium compounds tend to quickly pass through the body whereas insoluble uranium compounds, especially when inhaled by way of dust into the lungs, pose a more serious exposure hazard. After entering the bloodstream, the absorbed uranium tends to bioaccumulate and stay for many years in bone tissue because of uranium’s affinity for phosphates. Uranium is not absorbed through the skin, and alpha particles released by uranium cannot penetrate the skin.
 
Incorporated uranium becomes uranyl ions, which accumulate in bone, liver, kidney, and reproductive tissues. Uranium can be decontaminated from steel surfaces and aquifers.

To explore Uranium more visit the excellent articles below:-
http://www.guardian.co.uk/science/grrlscientist/2013/jun/21/1
http://en.wikipedia.org/wiki/Uranium

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Care and Storage pf pH Electrodes

The life of a pH electrode is not infinite. A number of factors affect the life span of a pH electrode. The higher the temperature that the electrode is used at, the more extreme the pH, how often the bulb dries out and needs to be rehydrated, how roughly it is used; all these factors and more shorten the life span of an electrode. An electrode that is well maintained and cared for can last up to 2 years, one that is not well maintained will not last as long, and one that is well maintained will not last significantly longer.

 

Storage of the pH electrode when not in use.

The pH electrode bulb needs to be moist at all times. When you are done with the electrode pour electrode storage solution into the cap that came with the electrode and put the cap over the bulb of the electrode. Keep the cap on until next use. If the electrode is being stored for a long time you may want to check the cap to be sure the storage solution is still in the cap and keeping the bulb moist. DO NOT STORE THE pH ELECTRODE IN DISTILLED WATER. Storing the pH electrode in distilled water will shorten the life of your pH electrode.

 

If you do not have electrode storage solution use pH 4 buffer solution. If you have neither electrode storage solution or pH 4 buffer solution you can use pH 7 buffer solution for a short time.

 

Rinsing the pH electrode between measurements.

You should rinse your pH electrode between measurements. This can be done with distilled water or rinsing with a sample of the next solution to be measured. Using both distilled water and then a sample of the next solution is also a good way to rinse the pH electrode between measurements.

 

pH electrode fill hole

Some pH electrodes have a fill hole for refreshing the electrolyte in the pH electrode; other pH electrodes do not have a fill hole. If your pH electrode has a fill hole the fill hole cap should be removed during calibration and use. This allows for the correct amount of reference electrolyte to flow into the sample. Replace the fill hole cap when done with the electrode at the end of the day

 

If bulb dries out, soak electrode bulb in pH 7

pH electrode bulbs should be keep moist at all times. When not in use the pH electrode bulb should be keep moist by pouring electrode storage solution in the cap provided. If the pH electrode bulb does dry out, soak it in pH 7 buffer for a couple of hours before calibrating or taking measurements.

 

Do not wipe the pH electrode with a cloth or any other type of material.

When you are done with the pH meter rinse off the electrode with distilled water, put storage solution in the cap, and put the cap on the end of the pH electrode as described above. If the electrode is wet do not dry it off, let the distilled water evaporate by itself.

 

Cleaning the pH electrode

The pH electrode needs to be cleaned in order to prevent build up of material on the surface of the glass bulb. How often it needs to be cleaned depends upon frequency of use and the material being tested. An electrode used on dark coloured and viscous material usually needs to be cleaned more often than an electrode used on clear thin material.  Material building up on the glass bulb of the electrode will cause the calibration of the electrode to be inaccurate and any subsequent reading to be inaccurate. Follow the instructions supplied with the electrode cleaning solution when cleaning the electrode bulb.
 
P&R Labpak supply a wide range of electrode storage solutions, buffers and other associated accessories from all major manufacturers including Hanna Instruments, Mettler Toledo, Sentek, Jenway, Schott, WTW etc…
 
Visit www.prlabs.co.uk or call us on 0870 034 2055.

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Laboratory Detergents

It’s important to make sure you choose the right detergent for your laboratory tasks whether they are for manual washing or for use in a washing machine.
 
As the sensitivity of analytical techniques has increased, the importance of stringent sample preparation and the quality and purity of the reagents are integral to getting good results. Even the best technique can be compromised by contaminated glassware or other lab utensils.

In the past, cleanliness was assured with toxic and aggressive products such as sodium hydroxide or Sulfo-chromic acid solutions that were very unpleasant to use. Fortunately lab detergents have come a long way. Today most labs have washing machines minimising effort and exposure to cleaning chemicals.

The issue now is ensuring that glassware is not contaminated with the detergent itself in the form of residues after cleaning. The detergent must be effective against contamination but not become a contaminant itself! A tall order when you consider the breadth of different tasks in specialised laboratories involving multiple types of contamination with various physical and chemical properties.
That’s the reason why the Labwash® Premium detergents range was developed in collaboration with experts. The range is extensive and includes good all round performance plus specialist products for specific requirements in different applications in pharma, petrochemicals, food industries, clinical labs etc..
Reliable processes are only possible with thorough, residue free cleaning and Labwash® delivers.
Excellent cleaning with no residues: Wide range of detergents suited to different cleaning tasks
High purity biodegradable ingredients: All raw materials fulfil the requirements of environmental protection.  Ecologically inert
High activity but low consumption: Labwash® Premium is concentrated but really efficient at low concentrations
Compatible with most materials: Labwash® Premium acts against contamination not the material being cleaned
1, 5, 10 and 20 l plastic packs: A wide range of packaging, easy to handle, adapted to your consumption
 
P&R Labpak are proud to offer this range of detergents to its customers.  We have a cross reference list to help customers choose which detergent is best suited for their needs if they want to swap from their existing brand so as to save money.
 
Why not visit our news page below and download the flyer detailing all the types available.
 
 
 
 

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What is a Soxhlet Extractor?

A Soxhlet extractor is a piece of laboratory apparatus invented in 1879 by Franz von Soxhlet. It was originally designed for the extraction of a lipid from a solid material. However, a Soxhlet extractor is not limited to the extraction of lipids. Typically, a Soxhlet extraction is only required where the desired compound has a limited solubility in a solvent, and the impurity is insoluble in that solvent. If the desired compound has a significant solubility in a solvent then a simple filtration can be used to separate the compound from the insoluble substance.

Normally a solid material containing some of the desired compound is placed inside a thimble made from thick filter paper, which is loaded into the main chamber of the Soxhlet extractor. The Soxhlet extractor is placed onto a flask containing the extraction solvent. The Soxhlet is then equipped with a condenser.

The solvent is heated to reflux. The solvent vapour travels up a distillation arm, and floods into the chamber housing the thimble of solid. The condenser ensures that any solvent vapour cools, and drips back down into the chamber housing the solid material.



The chamber containing the solid material slowly fills with warm solvent. Some of the desired compound will then dissolve in the warm solvent. When the Soxhlet chamber is almost full, the chamber is automatically emptied by a siphon side arm, with the solvent running back down to the distillation flask. The thimble ensures that the rapid motion of the solvent does not transport any solid material to the still pot. This cycle may be allowed to repeat many times, over hours or days.

During each cycle, a portion of the non-volatile compound dissolves in the solvent. After many cycles the desired compound is concentrated in the distillation flask. The advantage of this system is that instead of many portions of warm solvent being passed through the sample, just one batch of solvent is recycled.

After extraction the solvent is removed, typically by means of a rotary evaporator, yielding the extracted compound. The non-soluble portion of the extracted solid remains in the thimble, and is usually discarded.

For more information:-
http://en.wikipedia.org/wiki/Soxhlet_extractor
http://www.scilabware.com/Extraction-&-Fractionation/Soxhlet–Extraction/Soxhlet-complete-assemblies/p-51-52-208/
(Scilabware, Pyrex, Quickfit glassware available from P&R Labpak)

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