what is meant by molarity?
408650
a mole is the amount of a substance equal to its molecualr weight or 6.02 x 10^23 particles.  Molarity is the number of moles dissolved in a litre of solvent....if memory serves
40707
Definitions?  For inorganic chemistry?  You are going to have to give details.
244756
Volatilty in this context - its the aftermath of an explosive event.\n\nMeasured in terms of energetic force (joules, watts, amt of TNT, etc)\nDelivered = What should be the productive force by design\n\nWether Delivered = Actual is really applied semantics in my mine but only the supplier of the 'stuff' can explain.  Unless the supplier is trying to imput some accuracy into the calculation?  who knows?\n\ne.g.\nBombs(nuclear) - equivalent amount of TNT\nChemical reaction - equivalent energy released in joules/watts\n\nOther context where volatility is used :\n(no industry standard-consistent measurement methods)\n\nBoxing - power of the 'punch'\nInvestments - rate of rise N fall of prices
371216
Molarity is #moles/ volume in liters.\n\nFirst calculate the # of moles NaOH using the molecular weight (MW=40g/mole) of NaOH.\n\n#moles NaOH = weight NaOH/MW = 100g/(40g/mol)= 2.5moles\n\nNow calculate the molarity \n\nM= #moles NaOH/ volume = 2.5moles/20L = 0.125 Molar
134081
For liquids it is the volume of solute divided by the final volume after the solution.\nFor gaseous solute it is the volume at STP divided by the final solution volume.\nFor solid solutes v/v is not usually used.\nGenerally v/v is expressed in percent.
630251
Molarity is moles over volume(L) so covert the grams to moles. Do this by dividing the grams of your substance by the molar mass of the substance. \n58g/ 58g = 1 mole (Just a coincidence the two numbers are 58, they aren't always the same).\nThen divide moles by volume\n1 mole/ 1L and in this case the molarity is just 1.
851431
MASS / VOLUME\n that's way you measure it in g/mL
657532
Do you mean a reaction?  Some can be tracked by analytical methods.  Chemical equation has no meaning in this context.
377373
yes definetly the number of moles.
503503
In chemistry, concentration or Mass Percent is the measure of how much of a given substance there is mixed with another substance. This can apply to any sort of chemical mixture, but most frequently is used in relation to solutions, where it refers to the amount of solute dissolved in a solvent.\n\nTo concentrate a solution, one must add more solute, or reduce the amount of solvent (for instance, by selective evaporation). By contrast, to dilute a solution, one must add more solvent, or reduce the amount of solute.\n\nThere exists a concentration at which no further solute will dissolve in a solution. At this point, the solution is said to be saturated. If additional solute is added to a saturated solution, it will not dissolve. Instead, phase separation will occur, leading to either coexisting phases or a suspension. The point of saturation depends on many variables such as ambient temperature and the precise chemical nature of the solvent and solute.\n\nQualitative description\nOften in informal or non-technical language, concentration is descibed in a qualitative way, through the use of adjectives such as "dilute" or "weak" for solutions of relatively low concentration and of others like "concentrated" or "strong" for solutions of relatively high concentration. Those terms relate the amount of a substance in a mixture to the observable intensity of effects or properties caused by that substance. For example, a pratical rule is that that the more concentrated a chromatic solution is, the more intensely coloured it is.\n\nQuantitative notation\nFor scientifical or technical applications, a qualitative account of concentration is almost never sufficient, therefore Quantitative notations are needed to describe concentration. There are a number of different ways to quantitatively express concentration; the most common are listed below.\n\nNote: Many units of concentration require measurement of a substance's volume, which is variable depending on ambient temperature and pressure. Unless otherwise stated, all the following measurements are assumed to be at standard state temperature and pressure (that is, 25 degrees Celsius at 1 atmosphere or 101.325 kPa).\n\nMass percentage\nMass percentage denotes the mass of a substance in a mixture as a percentage of the mass of the entire mixture. For instance: if a bottle contains 40 grams of ethanol and 60 grams of water, then it contains 40% ethanol by mass. Commercial concentrated aqueous reagents such as acids and bases are often labeled in concentrations of weight percentage with the specific gravity also listed. In older texts and references this is sometimes referred to as weight-weight percentage (abbreviated as w/w).\n\nMass-volume percentage\nMass-volume percentage, (sometimes referred to as weight-volume percentage and often abbreviated as % m/v or % w/v) denotes the mass of a substance in a mixture as a percentage of the volume of the entire mixture. Mass-volume percentage is often used for solutions made from solid reagents. It is the mass of the solute in grams divided by the volume of solution in millilitres and multiplied by one hundred .\n\nVolume-volume percentage\nVolume-volume percentage or % (v/v) describes the volume of the solute in mL per 100 mL of the resulting solution. This is most useful when a liquid - liquid solution is being prepared. For example, beer is about 5% ethanol by volume. This means every 100 mL beer contains 5 mL ethanol (ethyl alcohol).\n\nMolarity\nMolarity (M) denotes the number of moles of a given substance per litre of solution. For instance: 4.0 litres of liquid, containing 2.0 moles of dissolved particles, constitutes a solution of 0.5 M. Such a solution may be described as "0.5 molar." (Working with moles can be highly advantageous, as they enable measurement of the absolute number of particles in a solution, irrespective of their weight and volume. This is often more useful when perform
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"Viscosity" is the degree to which a substance is fluid.\nIf a substance undergoes a decrease in viscosity when agitated, it is said to be "thixotropic."  The character of being thixotropic is called "thixotropy."
808705
Molarity of the solution = Number of moles of citric acid /1000 ml of solution\n\n= (250/192.1) moles of citric acid per 1000 ml of solution\n\n= 1.3014 M
890620
It is usually expressed as the concentration of the solute in water.  Phrased this way, one would say that the concentration of a given solute rises as you add more of it to a given amount of water.
960715
stoichiometry is \n\nCalculation of the quantities of reactants and products in a chemical reaction. \n\nThe quantitative relationship between reactants and products in a chemical reaction.
855791
There are a lot of items or writting related to these words. Permeability  is a measure of the ability of a material to transmit fluids. \n\nAbsorption, in chemistry, is a physical or chemical phenomenon or a process in which atoms, molecules, or ions enter some bulk phase - gas, liquid or solid material. \n\nthese two did not related to each other
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M (molarity) is defined as "mole per L (mole/L)" of solution\n\nglucose = C6H12O6, its molecular weight is 180.16g/mole (say about 180g/mole)\n\n1000mM = 1000mmole / L\n--> (1000mmole / L ) * (180g / mole)\n--> cancel out the "mole"\n--> 180000 mg/L\n\nsame logic for 970mM = 970mmole / L\n--> (970 mmole / L) * (180g / mole) = 174600 mg / L\n\nnote: you can leave the "m (milli)" there in your calculations, because, remember, "m" simply means 10^(-3), which is 0.001
928965
molarity  = moles / liters\n\nmoles = given mass / molecular mass\n\n10 g H2SO4 / 98 g per mole = about  0.1 moles\n\n0.1 moles / 1 L = 0.1 M solution