wat is the difference between molar& molaritry?

Answer 1

Molar = UNIT of concentration = moles/L
Molarity = used when talking of Concentration
mole = 6.022×10^23 molecules of a substance

Answer 2

About $20

Answer 3

Molar (Physics) A body of matter as a whole, perceived apart from molecular or atomic properties.


Molarity
Another way of expressing concentration, the way that we will use most in this course, is called molarity. Molarity is the number of moles of solute dissolved in one liter of solution. The units, therefore are moles per liter, specifically it's moles of solute per liter of solution.

molarity =
moles of solute
liter of solution



Rather than writing out moles per liter, these units are abbreviated as M or M. We use a capital M with a line under it or a capital M written in italics. So when you see M or M it stands for molarity, and it means moles per liter (not just moles).

You must be very careful to distinguish between moles and molarity. "Moles" measures the amount or quantity of material you have; "molarity" measures the concentration of that material. So when you're given a problem or some information that says the concentration of the solution is 0.1 M that means that it has 0.1 mole for every liter of solution; it does not mean that it is 0.1 moles. Please be sure to make that distinction.

Answer 4

(Obvious dental joke side-stepped...)

They are the same concept. You merely use the words under slightly different grammatical contexts. Follow...

Molarity is the concept. Molarity describes concentration in terms of moles of solute per liter of solution.

You use the term "molar" when describing the actual solution. "Molar" or M is the UNIT of molarity. If a hydrochloric acid solution has a concentration of 5 moles HCl per liter of solution, then it is said to be "5 molar" or 5 M HCl.

Answer 5

Molar (Physics) A body of matter as a whole, perceived apart from molecular or atomic properties.
Molarity (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." This can be misinterpreted as "0.5 moles of solute per 1.0 liter of solvent" which assumes the solute has no volume and/or no volume change occurs on mixing the solute with the solvent. This is why preparation of a solution of known molarity involves adding an accurately weighed amount of solute to a volumetric flask, adding some solvent to dissolve it, then adding more solvent to fill to the volume mark. (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 performing stoichiometric calculations.). See molar solution for further information.

Although molarity is by far the most commonly used measure for concentration, particularly for dilute aqueous solutions, it does suffer from a number of disadvantages. Masses can be determined with great precision as balances are often very precise. Determining volume is often not as precise. In addition, a volume of a liquid changes with temperature so that the molarity also changes without adding or removing any mass. For non-dilute solutions another problem is that the molar volume of a substance is itself a function of concentration so that volume is not strictly additive.

The National Institute of Standards and Technology, the United States authority on measurement, considers the term molarity and the unit symbol M to be obsolete, and suggests instead the 'amount-of-substance concentration' (c) with units mol/m3 or other units used alongside the SI such as mol/L [1]. This recommendation has not been generally accepted in academia.


[edit] Molality
Molality (m) denotes the number of moles of a given substance per kilogram of solvent (not: solution). For instance: 2.0 kilograms of solvent, to which are added 1.0 moles of dissolved particles, constitutes a molality of 0.5 mol/kg. Such a solution may be described as "0.5 molal". The term molal solution is used as a shorthand for a "one molal solution", i.e. a solution which contains one mole of the solute per 1000 grams of the solvent.

The determination of molality only requires a good balance, because the masses of both solvent and solute can be obtained by weighing. Using a balance is often more precise than working with volumetric flasks burettes and pipettes. Another advantage of molality is that it does not change with the temperature as it deals with the mass of solvent, rather than the volume of solution. Volume typically increases with increase in temperature resulting in decrease in molarity. Molality of a solution is always constant irrespective of the physical conditions like temperature and pressure.

As for water a mass of 1000 grams corresponds roughly to a volume 1 litre at room temperature, molalities and molarities converge in value for dilute aqueous solutions at ambient conditions. For different solvents and different conditions this is not the case. This may cause confusion amongst people with insufficient training in the subject. In addition, some languages (for example, Japanese) have no different sounds for syllables RA and LA.

NIST considers the symbol m to be obsolete, and instead suggests the notation mB (and the use of SI units such as mol/kg). This recommendation has not been generally accepted in science.

Answer 6

molarity and molar are one and same thing
they both means
no of moles present in 1litre of solution
molarity = molar =
no, of moles of solute
-----------------------------
vol .solution in litres
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Answer 7

http://www.mpsomaha.org/mnhs/apchem/assignments/Problems/c4pp1.htm