The compound is used for various purposes like Purifying water Making lubricating substances Making barium-rich chemicals Skin contact, inhalation or ingestion of this material can cause dangerous health hazards.
July Introduction Many of the dazzling bursts of color that light up the night sky on the Fourth of July are brought to you compliments of chlorine chemistry. Barium chloride, BaCl2, responsible for the glittering green bursts, is this month's featured chlorine compound.
But, barium chloride is much more than a pretty flash in the sky. The chemical element barium is a heavy, soft, silvery-white metal that, like the element chlorine, always occurs combined in nature.
Due to their reactivity, barium and chlorine form compounds naturally. The most common form of barium in nature is the salt barium sulfate, BaSO4, also known as the mineral barite. It is also the chief ore of barium. Barium chloride, another barium salt, can be manufactured by reacting barium sulfate with hydrochloric acid, HCl: Notice that barium and hydrogen switch "chemical partners" between the reactants side and the products side of the equation.
This type of reaction is known as a double-replacement reaction, and it may be represented in a fun, cartoon way as: Sulfate Detective Barium chloride has several important functions, but one very familiar to chemists is the role of "sulfate detective.
These negatively charged units are known as negatively charged ions, or anions. The key to barium chloride's role in tracking down sulfates is the simple fact that barium chloride dissolves in water while barium sulfate hardly dissolves in water at all.
Presented with a water-based liquid of unknown chemistry, a chemist might add barium chloride to the solution and watch for the appearance of a thick, white "precipitate" of barium sulfate, indicating the presence of sulfate. Although the term "precipitate" sounds as though it might be raining in a beaker, a precipitate is simply a solid that forms in a liquid solution as a result of a chemical reaction.
Because it is practically undissolvable in the liquid of the solution, the precipitate becomes visible. A chemical precipitate first turns a liquid cloudy and eventually, due to gravity, the cloudiness clears as the solid settles down to the bottom of the vessel.
Other Roles for Barium Chloride Besides being an important indicator chemical, barium chloride can be a starting chemical for barium and chlorine production. It is also used in manufacturing aluminum alloys, in pigments and dyes and as a water softener.
Taking Advantage of Barium's Physical Properties Barium, the name for the element of atomic number 56 on the Periodic Table of the Elementscomes from the Greek word "barys," meaning "heavy.
The same number of electrons balance the electrical charge. Barium's compounds are heavy and dense. Barium sulfate, for example, is used in x-ray examinations to image the human digestive system. The patient drinks a "barium milkshake," a slurry of barium sulfate which fills the digestive tract and provides an obstacle by virtue of its many electrons to x-rays.
In blocking the path of x-rays, barium outlines the tract, permitting doctors to identify problem areas.
Barium sulfate's high density also plays an important role in oil exploration. It is added to "drilling mud," a slurry added to drill holes to control the pressure on underground oil and gas reserves. Barium sulfate helps reduce the risk of blow-out-an escape of oil and gas from the drill hole.
Blow-outs can result in fire and explosion. The following chemical reaction is an example of a single replacement reaction involving potassium Kchlorine Cl and iodine I: How does this reaction differ from a double replacement reaction?
Make a cartoon representation of a single replacement reaction. Make a list of the metal chloride compounds that are used in fireworks and the colors they produce. For a list of previous "Chlorine Compound of the Month" features, click here. News View our resource center to find press releases, testimonies, infographics and more.Consider the reaction between hydrochloric acid and sodium hydroxide; HCl (aq) + NaOH (aq)> To write the products we combine the anion of the acid with the cation of the base and write the correct formula following the principle of electroneutrality.
The other product is water.
Molecular equation: HCl (aq) + NaOH (aq)> NaCl (aq) + H 2 O (l) So the molecular form of the equation is shown above. Barium hydroxide is a chemical compound with the chemical formula Ba(OH) 2 (H 2 O) x.
The monohydrate (x =1), known as baryta or baryta-water, is one of the principal compounds of barium. This white granular monohydrate is the usual commercial form.
Syllabus-specification CONTENT INDEX of revision summary notes. Note: a C after the learning objective indicates it is for Edexcel GCSE Chemistry ONLY, NOT for Combined Science.
Revision summaries for Edexcel GCSE Chemistry Paper 1 Chemistry 1 . Mar 28, · Reaction between barium hydroxide and sulfuric acid?
My text book says that the reaction between barium hydroxide and aqueous sulfuric acid to form barium sulphate and water would not work.
It offers no further plombier-nemours.com: Resolved. Dec 04, · Sulfuric acid, H2SO4, is an acid, and barium hydroxide, Ba(OH)2, is a base. When you mix the two, a neutralization reaction occurs that forms water and a salt.
The equation is:Status: Resolved. Precipitation reactions can be represented using several types of chemical equations: complete-formula equations (also known as "molecular" equations), complete ionic equations, and net ionic equations.
Each provides a different perspective on the chemicals involved in the reaction.