Sulfamic acid

Sulfamic acid
IUPAC name Sulfamic acid sulfamic acid
Another name Amide sulfuric acid
Identification information
CAS registration number	5329-14-6
It is an address number on a day	J43.594E
EINECS	226-218-8
United Nations / North America number	2967
RTECS number	WO5950000
Characteristic
Chemical formula	H3NSO3
Molar mass	97.10 g mol-1
The appearance	Colorless crystal
Density	2.15 g cm-3, solid
Melting point	205 degrees Celsius
The boiling point	The resolution
Solubility to water	14.689 g of / 100 g (0 degrees Celsius)
Acid dissociation constant pKa	0.99
Thermochemistry
Standard heat of formation ΔfHo	−674.9 kJ mol-1
The risk
Safe data sheet (outside link)	ICSC 0328
EU Index	016-026-00-0
R phrase	R36/38 R52/53
S phrase	S2 S26 S28 S61
Ignition point	Noninflammability
Associated material
Related material	Carbamic acid
I can put a case, the data without the special mention for normal temperature (25 degrees Celsius), the ordinary pressure (100 kPa).

The colorless solid that the sulfamic acid (スルファミン British: sulfamic acid) calls another name amide sulfuric acid, and a rational formula is referred to H₃N⁺SO₃^-. I dissolve in water well and show the relatively strong acidity. I am used to break down the surplus nitrite which remains behind when I dyed it with a diazo dye. A hydroxy group of the sulfuric acid substituted it for amino group.

Table of contents

Structure and reactive

The property of the sulfamic acid shows one of the zwitterion types which is tautomerism, a property as H₃N⁺SO₃^- as neutrality type H₂NSO₂(OH). The bond distance of sulfur and oxygen, sulfur and nitrogen is known each with 1.44, 1.77Å and shows that longer sulfur - oxygen has single bond, sulfur - nitrogen doubleness associativity [¹]. Furthermore, I understood that structure of H₃N⁺SO₃^- was important among four kinds of isomeric (neutrality type H₂NSO₂(OH), HN=SO(OH)₂, zwitterion type H₃N⁺SO₃^-, H₂N⁺=SO(OH)O^-) because it was shown that distance of 1.03Å included three hydrogen from nitrogen by an experiment of the neutron dispersion.

The sulfamic acid is acid dissociation constant Ka = 1.01 x 10^-1 with comparative strong acid. Because the solid is easy to get a pure article without showing absorbency, I am used as a standard material by acid base titration. I receive two phases of deprotonation in the ammonium solution and become dianion [HNSO₃]^2-.

The solid of the sulfamic acid melts at 205 degrees Celsius and I disintegrate at the higher temperature and change to water and sulfur trioxide, sulphur dioxide, nitrogen molecules.

There are urea and a common point at the point that amino group couples with 電子求引基 and generates an ammonium ion when, for example, I heat a water solution together.

Manufacturing method

It occurs because of a reaction of urea and the fuming sulphuric acid.

${\displaystyle \mathrm {CO(NH2)_{2}+H_{2}S_{2}O_{7}\rightarrow 2(NH_{2})HSO_{3}+CO_{2}}}$ 

Reaction

I produce nitrogen gas in response to nitrous acid.

${\displaystyle \mathrm {HNO_{2}+(NH_{2})HSO_{3}\rightarrow H_{2}SO_{4}+N_{2}+H_{2}O}}$ 

I am used for standardization to find the accurate density of sodium hydroxide solution.

${\displaystyle \mathrm {(NH_{2})HSO_{3}+NaOH\rightarrow (NH_{2})NaSO_{3}+H_{2}O}}$ 

Nitrous oxide occurs in response to work nitric acid as a reducing agent.

${\displaystyle \mathrm {HNO_{3}+(NH_{2})HSO_{3}\rightarrow H_{2}SO_{4}+N_{2}O+H_{2}O}}$ 

It is more than 80 degrees Celsius and is gradually hydrolyzed in cold water immediately and becomes hydrogen ammonium sulfate.

${\displaystyle \mathrm {(NH_{2})HSO_{3}+H_{2}O\ {\xrightarrow {80^{\circ }C}}\ NH_{4}HSO_{4}}}$ 

Use

 

Cyclamate

As for the sulfamic acid, the connection with the artificial sweetener is deep. Cyclamate which reacted sodium hydroxide, and was provided has been ever used many for a mixture of sulfamic acid and the cyclohexylamine as a cheap sweetener. Used acesulfame potassium is also an example of the artificial sweetener with sulfamic acid structure now.

In O- of the sulfamic acid or the N-substitution derivative, there is a thing used as an antibiotic, a reverse transcription inhibitor and a protease inhibitor, an anticancer agent (steroid sulfatase inhibitor, carbonic anhydrase inhibitor), an antiepileptic drug for HIV or antiobese medicine.

The sulfamic acid is used for washing of metal and ceramic as an acid cleaner. I am used as a rust last joke, scale miss in substitution for hydrochloric acid.

Raw materials of others, an esterification reaction and an acid catalysis, a pigment and the weed killer synthesis to push forward solidification of polymer (urethane resin, dentures stabilizer), nitrite production, the use as the additive to water system extinguishant are known.

Footnote

1. ^ J. W. Bats, P. Coppens, T. F. Koetzle (1977). "The Experimental Charge Density in Sulfur-Containing Molecules: A Study of the Deformation Electron Density in Sulfamic Acid at 78 K by X-ray and Neutron Diffraction." Acta Crystallographica B33. doi: 10.1107/S0567740877002568. 

References

Wiki media Commons has a category in conjunction with the sulfamic acid.

• MSDS
• General remarks: "Sulfamates and their therapeutic potential." Med. Res. Rev. 2005, 25, 186-228.
• General remarks: R. J. Cremlyn "An Introduction to Organosulfur Chemistry" John Wiley and Sons: Chichester, 1996. ISBN 0-471-95512-4
• General remarks: Greenwood, N. N.; Earnshaw, A. "Chemistry of the Elements, 2nd Edition" Oxford: Butterworth-Heinemann, 1997. ISBN 0-7506-3365-4

Outside link

• International Chemical Safety Card sulfamic acid - National Institute of Health Sciences

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