This page lists examples of the orders of magnitude of molar concentration. Source values are parenthesized where unit conversions were performed.
M denotes the non-SI unit molar:
Factor (Molarity) | SI prefix | Value | Item |
---|---|---|---|
10−24 | yM | 1.66 yM | 1 elementary entity per litre [1] |
8.5 yM | airborne bacteria in the upper troposphere (5100/m3) [2] | ||
10−23 | |||
10−22 | |||
10−21 | zM | 3.6 zM | solar neutrinos on Earth (6.5×1010 /cm2⋅s) [3] |
10−20 | 12 zM | radon in ambient, outdoor air in the United States (0.4 pCi/L ≈ 7000/L) [4] | |
10−19 | 120 zM | indoor radon at the EPA's "action level" (4 pCi/L ≈ 70000/L) [5] | |
686 zM | cosmic microwave background photons in outer space (413/cm3) [6] | ||
10−18 | aM | ||
10−17 | |||
10−16 | |||
10−15 | fM | 2 fM | bacteria in surface seawater (1×109/L) [7] |
10−14 | 20 fM | virions in surface layer North Atlantic seawater (10×109/L) [8] | |
50–100 fM | gold in seawater [9] | ||
10−13 | |||
10−12 | pM | 7.51–9.80 pM | normal range for erythrocytes in blood in an adult male ((4.52–5.90)×1012/L) [10] [11] |
10−11 | 10–100 pM | gold in undersea hydrothermal fluids [9] | |
10−10 | 170 pM | upper bound for healthy insulin when fasting [12] | |
10−9 | nM | 5 nM | inhaled osmium tetroxide is immediately dangerous to life or health (1 mg Os/m3) [13] |
10−8 | |||
10−7 | 101 nM | hydronium and hydroxide ions in pure water at 25 °C (pKW = 13.99) [14] | |
10−6 | μM | ||
10−5 | |||
10−4 | 180–480 μM | normal range for uric acid in blood [10] | |
570 μM | inhaled carbon monoxide induces unconsciousness in 2–3 breaths and death in < 3 min (12800 ppm) [15] | ||
10−3 | mM | 0.32–32 mM | normal range of hydronium ions in stomach acid (pH 1.5–3.5) [16] |
5.5 mM | upper bound for healthy blood glucose when fasting [17] | ||
7.8 mM | upper bound for healthy blood glucose 2 hours after eating [17] | ||
10−2 | cM | 20 mM | neutrinos during a supernova, 1 AU from the core (1058 over 10 s) [18] |
44.6 mM | pure ideal gas at 0 °C and 101.325 kPa [19] | ||
10−1 | dM | 140 mM | sodium ions in blood plasma [10] |
480 mM | sodium ions in seawater [20] | ||
100 | M | 1 M | standard state concentration for defining thermodynamic activity [21] |
101 | daM | 17.5 M | pure (glacial) acetic acid (1.05 g/cm3) [22] |
40 M | pure solid hydrogen (86 g/L ) [23] | ||
55.5 M | pure water at 3.984 °C, temperature of its maximum density (1.0000 g/cm3) [24] | ||
102 | hM | 118.8 M | pure osmium at 20 °C (22.587 g/cm3) [25] |
140.5 M | pure copper at 25 °C (8.93 g/cm3) | ||
103 | kM | ||
104 | 24 kM | helium in the solar core (150 g/cm3 ⋅ 65%) [26] | |
105 | |||
106 | MM | ||
107 | |||
108 | 122.2 MM | nuclei in a white dwarf from a 3 M☉ progenitor star (106.349 g/cm3) [27] | |
109 | GM | ||
1010 | |||
1011 | |||
1012 | TM | ||
1013 | |||
1014 | |||
1015 | PM | ||
1016 | |||
1017 | 228 PM | nucleons in atomic nuclei (2.3×1017 kg/m3 = 1.37×1044/m3) [28] | |
1018 | EM | ||
... | |||
1077 | 3.9×1077 M | the Planck concentration (2.4×10104/m3), inverse of the Planck volume | |
Submultiples | Multiples | ||||
---|---|---|---|---|---|
Value | SI symbol | Name | Value | SI symbol | Name |
10−1 M | dM | decimolar | 101 M | daM | decamolar |
10−2 M | cM | centimolar | 102 M | hM | hectomolar |
10−3 M | mM | millimolar | 103 M | kM | kilomolar |
10−6 M | μM | micromolar | 106 M | MM | megamolar |
10−9 M | nM | nanomolar | 109 M | GM | gigamolar |
10−12 M | pM | picomolar | 1012 M | TM | teramolar |
10−15 M | fM | femtomolar | 1015 M | PM | petamolar |
10−18 M | aM | attomolar | 1018 M | EM | examolar |
10−21 M | zM | zeptomolar | 1021 M | ZM | zettamolar |
10−24 M | yM | yoctomolar | 1024 M | YM | yottamolar |
10−27 M | rM | rontomolar | 1027 M | RM | ronnamolar |
10−30 M | qM | quectomolar | 1030 M | QM | quettamolar |
11.04 g/l is the concentration of sodium ions in water in other words. That’s 1.09% sodium ion!
The concentration of hydronium ions in pire water is 1.9 micrograms per liter. That’s 1.9 parts per billion of hydronium.
The normal range for hemoglobin molecules is 254.36 grams per liter or 20.27% hemoglobin. The concentration of pure water is 1 kilogram per liter or 50% water. Glacial acetic acid is 1.05 kilograms per liter or 51.2% acetic acid.
An acid is a molecule or ion capable of either donating a proton (i.e. hydrogen ion, H+), known as a Brønsted–Lowry acid, or forming a covalent bond with an electron pair, known as a Lewis acid.
In chemistry, pH, also referred to as acidity or basicity, historically denotes "potential of hydrogen". It is a logarithmic scale used to specify the acidity or basicity of aqueous solutions. Acidic solutions are measured to have lower pH values than basic or alkaline solutions.
Radon is a chemical element; it has symbol Rn and atomic number 86. It is a radioactive noble gas and is colorless and odorless. Of the three naturally occurring radon isotopes, only radon-222 has a sufficiently long half-life for it to be released from the soil and rock, where it is generated. Radon isotopes are the immediate decay products of radium isotopes. Radon's most stable isotope, radon-222, has a half-life of only 3.8 days, making radon one of the rarest elements. Radon will be present on Earth for several billion more years, despite its half-life being a mere 3.8 days, because it is constantly being produced as a step in the decay chain of uranium-238, and that of thorium-232, each of which is an extremely abundant radioactive nuclide with a half-life of several billion years. The decay of radon produces many other short-lived nuclides, known as "radon daughters", ending at stable isotopes of lead. Radon-222 occurs in significant quantities as a step in the normal radioactive decay chain of uranium-238, also known as the uranium series, which slowly decays into a variety of radioactive nuclides and eventually decays into lead-206, which is stable. Radon-220 occurs in minute quantities as an intermediate step in the decay chain of thorium-232, also known as the thorium series, which eventually decays into lead-208, which is stable.
In chemistry, a salt or ionic compound is a chemical compound consisting of an ionic assembly of positively charged cations and negatively charged anions, which results in a neutral compound with no net electric charge. The constituent ions are held together by electrostatic forces termed ionic bonds.
Super-Kamiokande is a neutrino observatory located under Mount Ikeno near the city of Hida, Gifu Prefecture, Japan. It is operated by the Institute for Cosmic Ray Research, University of Tokyo with the help of an international team. It is located 1,000 m (3,300 ft) underground in the Mozumi Mine in Hida's Kamioka area. The observatory was designed to detect high-energy neutrinos, to search for proton decay, study solar and atmospheric neutrinos, and keep watch for supernovae in the Milky Way Galaxy.
In chemistry, hydronium (hydroxonium in traditional British English) is the common name for the cation [H3O]+, also written as H3O+, the type of oxonium ion produced by protonation of water. It is often viewed as the positive ion present when an Arrhenius acid is dissolved in water, as Arrhenius acid molecules in solution give up a proton (a positive hydrogen ion, H+) to the surrounding water molecules (H2O). In fact, acids must be surrounded by more than a single water molecule in order to ionize, yielding aqueous H+ and conjugate base. Three main structures for the aqueous proton have garnered experimental support: the Eigen cation, which is a tetrahydrate, H3O+(H2O)3, the Zundel cation, which is a symmetric dihydrate, H+(H2O)2, and the Stoyanov cation, an expanded Zundel cation, which is a hexahydrate: H+(H2O)2(H2O)4. Spectroscopic evidence from well-defined IR spectra overwhelmingly supports the Stoyanov cation as the predominant form. For this reason, it has been suggested that wherever possible, the symbol H+(aq) should be used instead of the hydronium ion.
The sulfate or sulphate ion is a polyatomic anion with the empirical formula SO2−4. Salts, acid derivatives, and peroxides of sulfate are widely used in industry. Sulfates occur widely in everyday life. Sulfates are salts of sulfuric acid and many are prepared from that acid.
Indoor air quality (IAQ) is the air quality within and around buildings and structures. Poor indoor air quality due to indoor air pollution is known to affect the health, comfort, and well-being of building occupants. It has also been linked to sick building syndrome, reduced productivity, and impaired learning in schools. Common pollutants of indoor air include: secondhand tobacco smoke, air pollutants from indoor combustion, radon, molds and other allergens, carbon monoxide, volatile organic compounds, legionella and other bacteria, asbestos fibers, carbon dioxide, ozone and particulates. Source control, filtration, and the use of ventilation to dilute contaminants are the primary methods for improving indoor air quality.
Chlordane, or chlordan, is an organochlorine compound that was used as a pesticide. It is a white solid. In the United States, chlordane was used for termite-treatment of approximately 30 million homes until it was banned in 1988. Chlordane was banned 10 years earlier for food crops like corn and citrus, and on lawns and domestic gardens.
Molar concentration (also called molarity, amount concentration or substance concentration) is a measure of the concentration of a chemical species, in particular, of a solute in a solution, in terms of amount of substance per unit volume of solution. In chemistry, the most commonly used unit for molarity is the number of moles per liter, having the unit symbol mol/L or mol/dm3 in SI units. A solution with a concentration of 1 mol/L is said to be 1 molar, commonly designated as 1 M or 1 M. Molarity is often depicted with square brackets around the substance of interest; for example, the molarity of the hydrogen ion is depicted as [H+].
The self-ionization of water (also autoionization of water, and autodissociation of water, or simply dissociation of water) is an ionization reaction in pure water or in an aqueous solution, in which a water molecule, H2O, deprotonates (loses the nucleus of one of its hydrogen atoms) to become a hydroxide ion, OH−. The hydrogen nucleus, H+, immediately protonates another water molecule to form a hydronium cation, H3O+. It is an example of autoprotolysis, and exemplifies the amphoteric nature of water.
In chemistry, the amount of substance (symbol n) in a given sample of matter is defined as a ratio (n = N/NA) between the number of elementary entities (N) and the Avogadro constant (NA). The entities are usually molecules, atoms, or ions of a specified kind. The particular substance sampled may be specified using a subscript, e.g., the amount of sodium chloride (NaCl) would be denoted as nNaCl. The unit of amount of substance in the International System of Units is the mole (symbol: mol), a base unit. Since 2019, the value of the Avogadro constant NA is defined to be exactly 6.02214076×1023 mol−1. Sometimes, the amount of substance is referred to as the chemical amount or, informally, as the "number of moles" in a given sample of matter.
Bromoform is an organic compound with the chemical formula CHBr3. It is a colorless liquid at room temperature, with a high refractive index and a very high density. Its sweet odor is similar to that of chloroform. It is one of the four haloforms, the others being fluoroform, chloroform, and iodoform. It is a brominated organic solvent. Currently its main use is as a laboratory reagent. It is very slightly soluble in water and is miscible with alcohol, benzene, chloroform, ether, petroleum ether, acetone and oils.
The ionic strength of a solution is a measure of the concentration of ions in that solution. Ionic compounds, when dissolved in water, dissociate into ions. The total electrolyte concentration in solution will affect important properties such as the dissociation constant or the solubility of different salts. One of the main characteristics of a solution with dissolved ions is the ionic strength. Ionic strength can be molar or molal and to avoid confusion the units should be stated explicitly. The concept of ionic strength was first introduced by Lewis and Randall in 1921 while describing the activity coefficients of strong electrolytes.
Osmotic concentration, formerly known as osmolarity, is the measure of solute concentration, defined as the number of osmoles (Osm) of solute per litre (L) of solution. The osmolarity of a solution is usually expressed as Osm/L, in the same way that the molarity of a solution is expressed as "M". Whereas molarity measures the number of moles of solute per unit volume of solution, osmolarity measures the number of osmoles of solute particles per unit volume of solution. This value allows the measurement of the osmotic pressure of a solution and the determination of how the solvent will diffuse across a semipermeable membrane (osmosis) separating two solutions of different osmotic concentration.
In chemistry and fluid mechanics, the volume fraction is defined as the volume of a constituent Vi divided by the volume of all constituents of the mixture V prior to mixing:
The molar conductivity of an electrolyte solution is defined as its conductivity divided by its molar concentration.
Acetic acid, systematically named ethanoic acid, is an acidic, colourless liquid and organic compound with the chemical formula CH3COOH. Vinegar is at least 4% acetic acid by volume, making acetic acid the main component of vinegar apart from water. It has been used, as a component of vinegar, throughout history from at least the third century BC.
The health effects of radon are harmful, and include an increased chance of lung cancer. Radon is a radioactive, colorless, odorless, tasteless noble gas, which has been studied by a number of scientific and medical bodies for its effects on health. A naturally-occurring gas formed as a decay product of radium, radon is one of the densest substances that remains a gas under normal conditions, and is considered to be a health hazard due to its radioactivity. Its most stable isotope, radon-222, has a half-life of 3.8 days. Due to its high radioactivity, it has been less well studied by chemists, but a few compounds are known.
In chemistry, the molar absorption coefficient or molar attenuation coefficient is a measurement of how strongly a chemical species absorbs, and thereby attenuates, light at a given wavelength. It is an intrinsic property of the species. The SI unit of molar absorption coefficient is the square metre per mole, but in practice, quantities are usually expressed in terms of M−1⋅cm−1 or L⋅mol−1⋅cm−1. In older literature, the cm2/mol is sometimes used; 1 M−1⋅cm−1 equals 1000 cm2/mol. The molar absorption coefficient is also known as the molar extinction coefficient and molar absorptivity, but the use of these alternative terms has been discouraged by the IUPAC.
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