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Understanding Moles and Avogadro's Number in Chemistry

A mole is a fundamental unit in chemistry used to count entities such as atoms, molecules, or particles. Represented by Avogadro's number (6.02 x 10²³), one mole corresponds to approximately this number of entities. Similar to a dozen representing 12 items, a mole can quantify various substances, from atoms to apples. Understanding moles is crucial for calculations of mass and molarity, the concentration of solutions. This guide explains the significance of moles in chemistry and how to prepare solutions accurately using molarity concepts.

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Understanding Moles and Avogadro's Number in Chemistry

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  1. WHAT IS A MOLE? Image from: http://www.animationlibrary.com/sc/163/Other_Rodents/?page=7 Info modified from: http://genchem.chem.wisc.edu/sstutorial/FunChem.htm

  2. COUNTING ATOMS • Atoms are too small to count individually • Use a counting unit called Avogadro's number • Avogadro's number = 6.02 X 1023 atoms

  3. WHAT IS A MOLE? Just as an amount of 12 is described by the term dozen, Avogadro's number is described by the term mole. A dozen eggs is 12 eggs; a mole of atoms is 6.02 X 1023 atoms. http://images.jupiterimages.com/common/detail/84/83/23048384.jpg http://www.animationlibrary.com/sc/163/Other_Rodents/?page=7

  4. Avogadro's number can be used to count anything. You could have a mole of apples or a mole of Ping-Pong balls. You can get some idea of the magnitude of Avogadro's number by considering that a mole of Ping-Pong balls would cover the surface of the Earth with a layer approximately 60 miles thick. http://farm1.static.flickr.com/34/123891179_3c553b3dba.jpg

  5. Equally important:one mole of a substance has a mass in grams equal to the formula weight of that substance. • EX: one mole of glucose (C6H12O6) • contains 6.02 X 1023 molecules of glucose • has a mass in grams equal to 180 g (12 X 6 + 1.0 X 12 + 16 X 6 ) http://www1.istockphoto.com/file_thumbview_approve/3055983/2/istockphoto_3055983_sugar_pile.jpg

  6. MOLARITY =a measure of concentration of a solution given in moles/L Example: A 1.0 M solution of glucose is made by dissolving 180 g of glucose in enough water to equal 1 L How would you make a 0.5 M glucose solution? a 0.1 M glucose solution?

  7. THINK ABOUT IT? If you ADD 180 g of glucose TO 1 L of water, do you have a 1 M solution? YOU WILL END UP WITH MORE THAN 1 L of SOLUTION + http://www1.istockphoto.com/file_thumbview_approve/3055983/2/istockphoto_3055983_sugar_pile.jpg http://www.a3bs.com/imagelibrary/U14205/mechanics/U14205_graduated-cylinder-100-ml.jpg http://mrsdlovesscience.com/measure.html

  8. VOLUMETRIC FLASK • Add your sugar • Fill up to 1 L mark →

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