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Of these, the only ones that are conceptually reasonable to explain are "HClO" vs. Truong-Son N. Jan 10, Well, you should know seven of these at least roughly We explain after-the-fact that in general, a more electronegative central atom pulls electron density towards itself. As examples, "HI" is a stronger acid than "HBr" ; the primary reason is that "I" is larger than "Br"and makes a weaker bond with "H" there is a counteracting electronegativity trend, which is not significant here.

Thus, the "H"attached to an outer "O"gets less of it and thus the "O"-"H" bond is weakened. In direct contrast with "HCl" vs. Related questions How do I determine the molecular shape of a molecule? What is the lewis structure for co2? What is the lewis structure for hcn? How is vsepr used to classify molecules? What are the units used for the ideal gas law? How does Charle's law relate to breathing? What is the ideal gas law constant? How do you calculate the ideal gas law constant?

How do you find density in the ideal gas law? Does ideal gas law apply to liquids? Impact of this question views around the world. You can reuse this answer Creative Commons License.Perchloric acid.

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Simple Structure Advanced History. Comment on this record. Acido perclorico [Italian]. Hyperchloric acid. Perklorik asit [Turkish]. Waterstofperchloraat [Dutch]. Avoid heat. May form explosive peroxides. Incompatible with a wide variety of substances,including organic materials, alcohols, amines, strong acids, strongbases, acid anhydrides, finely powde red metals, strong reducing agents.

Contact with wood, paper and other celullose products may lead to explosion, as may contact with a variety of other organic and inorganic materials. Face shield for all but well-tried and predictable small-scale procedures. Click to predict properties on the Chemicalize site. Search ChemSpider: Compounds with the same molecular formula Compounds with the same skeleton Use this molecule in a structure search. Safety glasses, chemical resistant nitrile gloves.

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Axit pecloric

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Theoretical Properties.By using this website, you signify your acceptance of Terms and Conditions and Privacy Policy. Molar Mass, Molecular Weight and Elemental Composition Calculator Enter a chemical formula to calculate its molar mass and elemental composition:.

Molar mass of HClO4 is Computing molar mass molar weight To calculate molar mass of a chemical compound enter its formula and click 'Compute'. In chemical formula you may use: Any chemical element. Common compound names. Molar mass calculator also displays common compound name, Hill formula, elemental composition, mass percent composition, atomic percent compositions and allows to convert from weight to number of moles and vice versa.

Computing molecular weight molecular mass To calculate molecular weight of a chemical compound enter it's formula, specify its isotope mass number after each element in square brackets. Examples of molecular weight computations: C[14]O[16]2S[34]O[16]2. Definitions of molecular mass, molecular weight, molar mass and molar weight Molecular mass molecular weight is the mass of one molecule of a substance and is expressed in the unified atomic mass units u.

Weights of atoms and isotopes are from NIST article. Give us feedback about your experience with Molecular Weight Calculator.

hclo4

Related: Molecular weights of amino acids. Contact us. How to cite? Org online education free homework help chemistry problems questions and answers.They are not coincidentially equal.

HClO4 is an acid. Hint: if "H" is at the beginning of a chemical formula, the compound is probably an acid. HClO4 or perchloric acid is covalent, though the hydrogen-oxygen bond easily ionizes. A constant is not needed because HClO4 is a strong acid and will fully dissociate in solution. HClO4, or perchloric acid, is covalent. Click on the related link to see a structural formula for perchloric acid.

The name of HClO4 is perchloric acid. This is a type of inorganic compound. It is usually colorless and more acidic than nitric and sulfuric acids. Asked By Curt Eichmann. Asked By Leland Grant. Asked By Veronica Wilkinson. Asked By Daija Kreiger. Asked By Danika Abbott. Asked By Consuelo Hauck.

Asked By Roslyn Walter. All Rights Reserved. The material on this site can not be reproduced, distributed, transmitted, cached or otherwise used, except with prior written permission of Multiply.

hclo4

Ask Login. Asked by Wiki User. Top Answer. Wiki User Answered Perchloric acid and as the last part of the name suggests is an acid. Related Questions. How HClO4 formed? What is the name of the compound HClO4? Is HClO4 a salt? IS HClO4 a strong or weak acid? Is HClO4 a weak acid? What is the chemical formula HClO4?

Is HClO4 an electrolyte? Is HClO4 a strong acid? IS HClO4 an acid or a base? Does HClO4 ionic bond?

HClO4 Lewis Structure: How to Draw the Lewis Structure for HClO4

What is the conjugate acid of ClO4?When acids are added to aqueous salts of hypochlorous acid such as sodium hypochlorite in commercial bleach solutionthe resultant reaction is driven to the left, and chlorine gas is formed. Thus, the formation of stable hypochlorite bleaches is facilitated by dissolving chlorine gas into basic water solutions, such as sodium hydroxide. The acid can also be prepared by dissolving dichlorine monoxide in water; under standard aqueous conditions, anhydrous hypochlorous acid is currently impossible to prepare due to the readily reversible equilibrium between it and its anhydride: [14].

The presence of light or transition metal oxides of coppernickelor cobalt accelerates the exothermic decomposition into hydrochloric acid and oxygen : [14]. Salts of hypochlorous acid are called hypochlorites. One of the best-known hypochlorites is NaClOthe active ingredient in bleach. HOCl reacts with ammonia to form monochloramine :. HOCl can also react with organic aminesforming N -chloroamines. Hypochlorous acid reacts with a wide variety of biomolecules, including DNARNA[8] [15] [16] [17] fatty acid groups, cholesterol [18] [19] [20] [21] [22] [23] [24] [25] and proteins.

Knox et al. This is because HClO oxidises sulfhydryl groups, leading to the formation of disulfide bonds [32] that can result in crosslinking of proteins. The HClO mechanism of sulfhydryl oxidation is similar to that of monochloramineand may only be bacteriostatic, because once the residual chlorine is dissipated, some sulfhydryl function can be restored.

Sulfenic acids form disulfides with another protein sulfhydryl group, causing cross-linking and aggregation of proteins. Sulfinic acid and R—SO 3 H derivatives are produced only at high molar excesses of HClO, and disulfides are formed primarily at bacteriocidal levels. Hypochlorous acid reacts readily with amino acids that have amino group side-chains, with the chlorine from HClO displacing a hydrogen, resulting in an organic chloramine. Consistent with these results, it was later proposed that the chloramine undergoes a molecular rearrangement, releasing HCl and ammonia to form an aldehyde.

The sugar moieties are nonreactive and the DNA backbone is not broken. A second slower reaction that results in cleavage of the pyridine ring occurs when excess HClO is present. This reaction occurs by hydrolysis with addition of chlorine to one of the carbons and a hydroxyl to the other.

Molecular weight of HClO4

The resulting compound is a chlorohydrin. Disruption could occur if enough chlorohydrin is formed. InKnox et al.

He proposed that the active agent or agents diffuse across the cytoplasmic membrane to inactivate key sulfhydryl -containing enzymes in the glycolytic pathway. This group was also the first to note that chlorine solutions HOCl inhibit sulfhydryl enzymes.

Later studies have shown that, at bacteriocidal levels, the cytosol components do not react with HOCl.

hclo4

It has been further shown that loss of sulfhydryls does not correlate with inactivation. The uptake of radiolabeled substrates by both ATP hydrolysis and proton co-transport may be blocked by exposure to HOCl preceding loss of viability.

Venkobachar et al. Albrich et al.

hclo4

It was also observed that irreversible oxidation of cytochromes paralleled the loss of respiratory activity. One way of addressing the loss of oxygen uptake was by studying the effects of HOCl on succinate-dependent electron transport.In chemistry, the formula weight is a quantity computed by multiplying the atomic weight in atomic mass units of each element in a chemical formula by the number of atoms of that element present in the formula, then adding all of these products together.

A common request on this site is to convert grams to moles. To complete this calculation, you have to know what substance you are trying to convert.

The reason is that the molar mass of the substance affects the conversion. This site explains how to find molar mass. If the formula used in calculating molar mass is the molecular formula, the formula weight computed is the molecular weight. The percentage by weight of any atom or group of atoms in a compound can be computed by dividing the total weight of the atom or group of atoms in the formula by the formula weight and multiplying by We use the most common isotopes.

This is how to calculate molar mass average molecular weightwhich is based on isotropically weighted averages. This is not the same as molecular mass, which is the mass of a single molecule of well-defined isotopes. For bulk stoichiometric calculations, we are usually determining molar mass, which may also be called standard atomic weight or average atomic mass. Formula weights are especially useful in determining the relative weights of reagents and products in a chemical reaction.

HClO4 / ácido tetraoxoclórico (VII)

These relative weights computed from the chemical equation are sometimes called equation weights. Using the chemical formula of the compound and the periodic table of elements, we can add up the atomic weights and calculate molecular weight of the substance. When calculating molecular weight of a chemical compound, it tells us how many grams are in one mole of that substance.

The formula weight is simply the weight in atomic mass units of all the atoms in a given formula. Molecular weight of HClO4.Perchloric acid is a mineral acid with the formula HClO 4. Usually found as an aqueous solution, this colorless compound is a stronger acid than sulfuric acid and nitric acid.

Perchloric acid is useful for preparing perchlorate salts, especially ammonium perchloratean important rocket fuel component. Perchloric acid is dangerously corrosive and readily forms potentially explosive mixtures. Perchloric acid is produced industrially by two routes. Treatment of such solutions with hydrochloric acid gives perchloric acid, precipitating solid sodium chloride:. The concentrated acid can be purified by distillation. The alternative route, which is more direct and avoids salts, entails anodic oxidation of aqueous chlorine at a platinum electrode.

Treatment of barium perchlorate with sulfuric acid precipitates barium sulfateleaving perchloric acid. It can also be made by mixing nitric acid with ammonium perchlorate and boiling while adding hydrochloric acid. The reaction gives nitrous oxide and perchloric acid due to a concurrent reaction involving the ammonium ion and can be concentrated and purified significantly by boiling off the remaining nitric and hydrochloric acids.

Anhydrous perchloric acid is an unstable oily liquid at room temperature.

Hypochlorous acid

It forms at least five hydratesseveral of which have been characterized crystallographically. This form of the acid is stable indefinitely and is commercially available. Such solutions are hygroscopic. Thus, if left open to the air, concentrated perchloric acid dilutes itself by absorbing water from the air. Dehydration of perchloric acid gives the anhydride dichlorine heptoxide : [8]. Perchloric acid is mainly produced as a precursor to ammonium perchloratewhich is used in rocket fuel.

The growth in rocketry has led to increased production of perchloric acid. Several million kilograms are produced annually. Other acids of noncoordinating anionssuch as fluoroboric acid and hexafluorophosphoric acid are susceptible to hydrolysis, whereas perchloric acid is not. Despite hazards associated with the explosiveness of its salts, the acid is often preferred in certain syntheses. It is also used for electropolishing or etching of aluminium, molybdenum, and other metals. Given its strong oxidizing properties, perchloric acid is subject to extensive regulations.

Work conducted with perchloric acid must be conducted in fume hoods with a wash-down capability to prevent accumulation of oxidisers in the ductwork. The O'Connor Electro-Plating plant, 25 other buildings, and 40 automobiles were obliterated, and nearby homes were damaged.

The bath was being used to electro-polish aluminium furniture. In addition, organic compounds were added to the overheating bath when an iron rack was replaced with one coated with cellulose acetobutyrate Tenit-2 plastic. A few minutes later the bath exploded. From Wikipedia, the free encyclopedia. Perchloric acid. Hyperchloric acid [1]. CAS Number. Interactive image. PubChem CID. Chemical formula. Solubility in water.