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MOLARITY A measurement of the concentration of a solution Molarity (M) is equal to the moles of solute (n) per liter of

MOLARITY A measurement of the concentration of a solution Molarity (M) is equal to the moles of solute (n) per liter of solution M = n / V = mol / L. Calculate the molarity of a solution prepared by mixing 1.5 g of NaCl in 500.0 mL of water. First calculate the moles of solute:

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MOLARITY A measurement of the concentration of a solution Molarity (M) is equal to the moles of solute (n) per liter of

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  1. MOLARITY A measurement of the concentration of a solution Molarity (M) is equal to the moles of solute (n) per liter of solution M = n / V = mol / L Calculate the molarity of a solution prepared by mixing 1.5 g of NaCl in 500.0 mL of water. First calculate the moles of solute: 1.5 g NaCl (1 mole NaCl) = 0.0257 moles of NaCl 58.45 g NaCl Next convert mL to L: 0.500 L of solution Last, plug the appropriate values into the correct variables in the equation: M = n / V = 0.0257 moles / 0.500 L = 0.051 mol/L

  2. MOLARITY M = n / V = mol/ L How many grams of LiOH is needed to prepare 250.0 mL of a 1.25 M solution? First calculate the moles of solute needed: M = n / V, now rearrange to solve for n:n = MV n = (1.25 mol / L) (0.2500 L) = 0.3125 moles of solute needed Next calculate the molar mass of LiOH: 23.95 g/mol Last, use diminsional analysis to solve for mass: 0.3125 moles (23.95 g LiOH / 1 mol LiOH) = 7.48 g of LiOH

  3. MOLARITY M = n / V = mol/ L What is the molarity of hydroiodic acid if the solution is 47.0% HI by mass and has a density of 1.50 g/mL? First calculate the mass of solute in the 47.0% solution using the density. The 1.50 g/mL is the density of the solution but only 47.0% of the solution is the solute therefore: 47.0% of 1.50 g/mL = (0.470) (1.50 g/mL) = 0.705 g/mL density of solute Since molarity is given in moles per liter and not grams we must convert the g/mL to mol/mL using the molar mass. 0.705 g/mL (1 mole/ 128 g) = 0.00551 mol/mL Next convert mL to L: 0.00551 mol/mL (1000 mL/ 1L) = 5.51 mol/L = 5.51 M

  4. MOLARITY & DILUTION M1V1 = M2V2 The act of diluting a solution is to simply add more water (the solvent) thus leaving the amount of solute unchanged. Since the amount or moles of solute before dilution (nb) and the moles of solute after the dilution (na) are the same: nb = na And the moles for any solution can be calculated by n=MV A relationship can be established such that MbVb = nb = na= MaVa Or simply : MbVb = MaVa

  5. MOLARITY & Dilution Calculate the molarity of a solution prepared by diluting 25.0 mL of 0.05 M potassium iodide with 50.0 mL of water (the densities are similar). M1 = 0.05 mol/L M2 = ? V1 = 25.0 mL V2 = 50.0 + 25.0 = 75.0 mL M1V1 = M2V2 M1 V1 = M2 = (0.05 mol/L) (25.0 mL) = 0.0167 M of KI V2 75.0 mL

  6. MOLARITY & dilution Given a 6.00 M HCl solution, how would you prepare 250.0 mL of 0.150 M HCl? M1 = 6.00 mol/L M2 = 0.150 V1 = ? mL V2 = 250.0 mL M1V1 = M2V2 M2 V2 = V1 = (0.150 mol/L) (250.0 mL) = 6.25 mL of 6 M HCl M1 6.00 mol/L You would need 6.25 mL of the 6.00 M HCl reagent which would be added to about 100 mL of DI water in a 250.0 mL graduated cylinder then more water would be added to the mixture until the bottom of the menicus is at 250.0 mL. Mix well.

  7. PRACTICE PROBLEMS 2.4 M _________1. What is the concentration of 250.0 mL of 0.60 moles of HCl? _________ 2. What is the concentration of 35.0 mL of 0. 0556 moles of KCl? _________ 3. How many grams of KCl is needed to prepare 50.0 mL of a 0.10 M solution? _________ 4. How many milliliters of water must be added to 30.0 mL of 9.0 M KCl to make a solution that is 0.50 M KCl? _________ 5. What volume of 0.7690 M LiOH will contain 55.3 g of LiOH? _________ 6. How many liters of water must be added to 100.0 mL of 4.50 M HBr to make a solution that is 0.250 M HCl? 1.59 M 0.38 g 510 mL 3.00 L 1.80 L

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