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Solution Concentration (Molarity)

Solution Concentration (Molarity). Concentration. a measure of the amount of solute that is dissolved in a given quantity of solvent unit of measurement is Molarity (M) which is moles/liter can be dilute or concentrated. moles solute. Molarity. =. liters of solution. Molarity.

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Solution Concentration (Molarity)

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  1. Solution Concentration (Molarity)

  2. Concentration • a measure of the amount of solute that is dissolved in a given quantity of solvent • unit of measurement is Molarity (M) which is moles/liter • can be dilute or concentrated

  3. moles solute Molarity = liters of solution Molarity • The number of moles of solute dissolved in one liter of solution

  4. 1.0 L of water was used to make 1.0 L of solution. Notice the water left over. 1.0L of water would be too much.

  5. Making a known molar solution top off to 1 liter

  6. PROBLEM: Dissolve 5.00 g of NiCl2•6 H2O in enough water to make 250 mL of solution. Calculate the Molarity. Step 1: Calculate moles of NiCl2• 6H2O in 5 g of NiCl2• 6H2O 1.0 L = 1000 mL .25 L = 250 mL Step 2: Calculate Molarity

  7. USING MOLARITY What mass of oxalic acid, H2C2O4, is required to make 250 mL of a 0.0500 M solution? Step 1: Change mL to L. 250 mL/1000 = 0.250 L Step 2: Calculate. moles = (0.0500 M) (0.250 L) = 0.0125 moles H2C2O4 Step 3: Convert moles to grams. (0.0125 mol H2C2O4) (90.00 g) = 1.13 g 1 mol H2C2O4 M = moles/V  moles = M•V

  8. Learning Check How many grams of NaOH are required to prepare 400 mL of 3.0 M NaOH solution? 1) 12 g 2) 48 g 3) 300 g

  9. Making Dilutions • diluting a solution reduces the number of moles of solute per unit volume, but the total number of moles of solute in the solution does not change • therefore, as Volume increases, Molarity decreases • Molarity (M) = moles of solute liters of solution (V) becomes: M1 V1 = M2 V2

  10. How many milliliters of a 2.00M MgSO4 solution must be diluted with water to prepare 100 ml of a 0.400 M MgSO4 solution? M1V1 = M2 V2

  11. air lead

  12. Percent Solutions • another way to quantitatively describe the concentration of a solution (two ways): • the ratio of the volume of the solute to the volume of the solution • % V = volume of solute / volume of solution x 100% • 85 mL of ethanol diluted with water to a total solution volume of 250mL • 85 mL/250 mL (100%) = 34% ethanol by volume • the ratio of the mass of the solute to the mass of the solution • % M = mass of solute / mass of solution x 100% • 56 g NaCl in a 2000 g NaCl solution • 56g/2000g (100%) = 2.8% salt by mass

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