#Molar mass of nacl plus

This used to be measured in atomic mass units (AMU) but is now typically expressed in Daltons (Da).

#Molar mass of nacl plus

Rearranging the equation is not necessary as the calculator tool will do this for you.Īs you are adding 58.44 g of NaCl to 2 L of water you could also express this value in terms of its concentrationĪtomic mass ( m a) – mass of one atom of that element which typically reflects the mass of the nucleus (protons plus neutrons). So, to make 2 liters of a 0.5 M solution of NaCl, you would need to add 58.44 g of NaCl. You need to make a 0.5 M solution of NaCl, having decided you want 2 liters how much NaCl should you add?įirst you must calculate the number of moles in this solution, by rearranging the equation Here, the solution being used is typically defined by its molar concentration ( M). The scenario in which most lab scientists will encounter this type of calculation is when making up solutions following a standard operating procedure (SOP) or a scientific paper.

Molarity ( M or mol/L) = Number of Moles (mol) / Volume (L)Įxample of molarity and concentration calculations Number of moles (mol) = Mass (g) / Molar Mass (g/mol)Ĭoncentration (g/L) = Mass (g) / Volume (L) To calculate molarity or to calculate related values (including volume, mass, molar mass and concentration) from molarity, the following equations are utilized. Provided some additional information is known, one value can be deduced from the other using the equations below. Whereas two solutions at the same concentration will have the same mass of the chemical per liter of solution but are therefore likely to have differing numbers of molecules of that chemical per liter. Two solutions that have the same molarity will have the same number of molecules of the chemical per liter but are likely to contain differing masses of that chemical per liter to achieve this. How does molarity relate to concentration? For sodium chloride (NaCl) they are in a ratio of 1:1 so the molar mass of NaCl is 22.99 + 35.45 = 58.44 g/mol.įor a compound like water (H 2O), 1 mole of hydrogen (H) is 1.008 g/mol and 1 mole of oxygen (O) is 15.9994 g/mol. One mole of sodium (Na) is 22.99 g, and 1 mole of chlorine is 35.45 g.

The molar mass is the mass in grams of 1 mole of a particular molecule. So, 1 mole of hydrogen gas (H 2) contains 6.02x10 23 molecules, and 1 mole of glucose (C 6H 12O 6.) also contains 6.02x10 23 molecules, but as H 2 is a much simpler molecule, 1 mole of H 2 will have a much smaller mass (the molar mass) than 1 mole of C 6H 12O 6. This equates to roughly 6.02x10 23, also referred to as Avogadro's Number. A 1 M solution is said to be “one molar”.Ī mole is the quantity of anything that has the same number of particles as 12 g of carbon-12. Molarity is the concentration of a solution in terms of the number of moles of the solute in 1 dm 3 (1 liter) of the solution.