Mole: Difference between revisions
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Moles are the units used to measure the concentration of a chemical in a solution. | Moles are the units used to measure the concentration of a chemical in a solution. | ||
A mole, in chemical terms, should not be confused with a small brown furry animal that can dig up your lawn. Nor with Molarity( denoted by M) which is a measure of concentration of a chemical species/substance in moles per unit volume, commonly per litre (Mol/L) | A mole, in chemical terms, should not be confused with a small brown furry animal that can dig up your lawn. Nor with Molarity( denoted by M) which is a measure of concentration of a chemical species/substance in moles per unit volume, commonly per litre (Mol/L). | ||
The numbers of moles in a sample can be calculated as follows: | |||
Number of Moles = Mass of the Sample (g) / Relative Formula (or Atomic) Mass | |||
For example, the mass of 1 mole of sodium chloride (NaCl) is 58.44g. | |||
Revision as of 16:24, 11 November 2012
A mole is a measure of chemical mass which is defined by the unit 6.022x1023 atoms of carbon-12. This value is also known as Avagadro's Constant.
Moles are the units used to measure the concentration of a chemical in a solution.
A mole, in chemical terms, should not be confused with a small brown furry animal that can dig up your lawn. Nor with Molarity( denoted by M) which is a measure of concentration of a chemical species/substance in moles per unit volume, commonly per litre (Mol/L).
The numbers of moles in a sample can be calculated as follows:
Number of Moles = Mass of the Sample (g) / Relative Formula (or Atomic) Mass
For example, the mass of 1 mole of sodium chloride (NaCl) is 58.44g.