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THE MOLE

This guide provides essential insights into molarity, a critical concept in chemistry. Learn the basics of calculating molarity, including definitions, formulae, and step-by-step problem-solving methods. Discover how to determine the concentration of a solution, the significance of the molar mass from the periodic table, and how to carry out molarity calculations with examples. This is an essential resource for anyone studying chemistry, from beginners to advanced learners.

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THE MOLE

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  1. THE MOLE Molarity January 14, 2009 (adapted from Mrs. J’s website)

  2. Very Important to Know! • 1000 ml = 1 L • g/1 mol = molar mass = priodic table • Multiply  subscripts = yes Coefficients = NO

  3. substance being dissolved total combined volume A. Molarity • Concentration of a solution.

  4. A. Molarity 2M HCl What does this mean?

  5. MASS IN GRAMS MOLES NUMBER OF PARTICLES LITERS OF SOLUTION B. Molarity Calculations 6.02  1023 (particles/mol) molar mass (g/mol) Molarity (mol/L)

  6. Steps for Solving Molarity problems • Measure the mass or the mass will be given (in grams – g). This is the solute. • Determine the molar mass of the solute. • Where do you find molar mass? • What are the units and per how many moles? • Calculate the moles of the solute. • Add the water. This is the solvent and is also the volume of the molarity calculation. • Solute from step 1 dissolved insolvent from step 4 = solution • measurement’s final unit needs to be in Liters! • Molarity = mol solute / Liters of solution or M = mol / L

  7. M = B. Molarity Calculations • Find the molarity of a 250 mL solution containing 10.0 g of NaF. 10.0 g 1 mol 41.99 g = 0.238 mol NaF 0.238 mol 0.25 L = 0.95M NaF

  8. B. Molarity Calculations • How many grams of NaCl are required to make 0.500L of 0.25M NaCl? 0.500 L 0.25 mol 1 L 58.44 g 1 mol = 7.3 g NaCl

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