Bewise Inc. www.tool-tool.com Reference
source from the internet.
硝酸鉀是鉀的硝酸鹽,
分子式KNO3。外觀為透明無色或白色粉末,無味,比重(水=1)為2.11。在水中的溶解度為13
g/100mL(因溫度而異,溫度越高溶解度越高,在其他化學物質之中,硝酸鉀溶解度變化是相當明顯的)。
潮解性較硝酸鈉為低,有冷卻刺
激鹽味。溶於水,稍溶於乙醇。
主要用途是製作火柴頭及煙火以及黑火藥、肥料、玻璃、燈蕊、醃
肉,此外煙草、冶金、分
析化學上亦常用之。
Potassium nitrate is a chemical compound
with the formula
KNO3. It occurs
as a mineral niter and
is a natural solid source of nitrogen. Its common
names include saltpetre (saltpeter in American English),
from Medieval Latin sal petræ: "stone salt" or possibly "Salt of Petra" and nitrate of
potash. The name Peru saltpetre or Chile saltpetre
(American Peru saltpeter or Chile saltpeter) refers not to
potassium nitrate but to a similar chemical sodium nitrate.
Major uses of potassium nitrate are in fertilizers, rocket propellants
and fireworks. When
used as a food additive in the European Union, the compound is referred
to as E252.
The
earliest known complete purification process for potassium nitrate was
outlined in 1270 by the Arab
chemist and engineer Hasan al-Rammah of Syria in his book al-Furusiyya
wa al-Manasib al-Harbiyya ('The Book of Military Horsemanship
and Ingenious War Devices'), where he first described the use of potassium
carbonate (in the form of wood ashes).
Into
the 19th century, niter-beds were prepared by mixing manure with either mortar
or wood ashes, common earth and organic materials such as straw to give
porosity to a compost pile typically 1.5×2×5 meters in size. The heap
was usually under a cover from the rain, kept moist with urine, turned
often to accelerate the decomposition and leached
with water after approximately one year. Dung-heaps were a particularly
common source: ammonia
from the decomposition of urea
and other nitrogenous materials would undergo bacterial oxidation to
produce various nitrates, primarily calcium nitrate, which could be
converted to potassium nitrate by the addition of potash from wood ashes.
A
variation on this process, using only urine, straw and wood ash, is
described by LeConte: Stale urine is placed in a container of straw hay
and is allowed to sour for many months, after which water is used to
wash the resulting chemical salts from the straw. The process is
completed by filtering the liquid through wood ashes and air-drying in
the sun.
During this period, the major natural sources of
potassium nitrate were the deposits crystallizing from cave walls and
the accumulations of bat
guano in caves. Traditionally guano was the source used in Laos for the manufacture of
gunpowder for Bang
Fai rockets.
During the 19th century and until around World War I,
potassium nitrate was produced on an industrial scale by the Birkeland–Eyde
process. Today practically all nitrates are produced from the
oxidation of ammonia
made by the Haber
process.
Potassium nitrate can be made by combining ammonium nitrate,
obtainable from instant cold packs, and potassium
hydroxide.
The reaction is shown here: NH4NO3
(aq) + KOH (aq) → NH3 (g) + KNO3 (aq) + H2O
(l)
As toxic ammonia
gas is produced, you should not do this indoors.
An alternative
way of producing potassium nitrate without a by-product of ammonia is to
combine ammonium
nitrate and potassium
chloride, easily obtained as a sodium-free salt substitute.
NH4NO3 (aq) + KCl (aq) → NH4Cl
(aq) + KNO3 (aq)
Potassium nitrate has an orthorhombic
crystal structure at room temperature, which transforms to a trigonal
system at 129 °C. Upon heating to temperatures above 560 °C, it
decomposes into potassium
nitrite, generating oxygen:
+ O2
Potassium nitrate is moderately soluble in
water, but its solubility increases with temperature (see infobox). The
aqueous solution is almost neutral, exhibiting pH 6.2 at 14 °C for a
10% solution of commercial powder. It is not very hygroscopic, absorbing
about 0.03% water in 80% relative humidity
over 50 days. It is insoluble in alcohol and is not poisonous; it can
react explosively with reducing agents, but it is not explosive on its
own.
Potassium nitrate is mainly used in fertilizers, as a
source of nitrogen and potassium – two of the macro nutrients
for plants. When used by itself, it has an NPK rating of
13-0-44. Potassium nitrate is also one of the three components of black powder, along
with powdered charcoal (substantially carbon) and sulfur, where it acts
as an oxidizer.
In the process of food preservation,
potassium nitrate has been a common ingredient of salted meat since the
Middle Ages, but
its use has been mostly discontinued due to inconsistent results
compared to more modern nitrate and nitrite compounds. Even so,
saltpetre is still used in some food applications, such as charcuterie and the
brine used to make corned
beef. Sodium
nitrate (and nitrite)
have mostly supplanted potassium nitrate's culinary usage, as they are
more reliable in preventing bacterial infection than saltpetre. All
three give cured salami
and corned beef their characteristic pink hue.
Potassium nitrate
is an efficient oxidizer, which produces a lilac flame upon burning due
to the presence of potassium. It is therefore used in amateur rocket
propellants and in several fireworks such as smoke bombs. It is
also added to pre-rolled cigarettes to maintain an even burn of the
tobacco.
Potassium nitrate is the main component (usually about
98%) of tree stump remover, as it accelerates the natural decomposition
of the stump. It is also commonly used in the heat treatment of metals
as a solvent in the post-wash. The oxidizing, water solubility and low
cost make it an ideal short-term rust inhibitor.
Potassium nitrate can be found in some toothpastes for
sensitive teeth.
Recently, the use of potassium nitrate in toothpastes for
treating sensitive teeth (dentine
hypersensitivity) has increased dramatically, even though studies to
this effect have been inconclusive.
Potassium nitrate
successfully combats high blood pressure and was once used as a
hypotensive. Other nitrates and nitrites such as glyceryl
trinitrate (nitroglycerin), amyl nitrite and isosorbide derivatives
are still used to relieve angina.
Potassium nitrate was once thought to induce impotence, and is
still falsely rumored to be in institutional food (such as military
fare) as an anaphrodisiac;
however, there is no scientific evidence for such properties.
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