Solutions.

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Solutions

Quantitative Expressions of Concentration Percent by mass Percent by volume Molarity Molality Dilution of solutions

Percent by Mass Percent by mass gives the mass of solute per mass units of solution Percent solute=mass of solute x 100% mass of solution Mass of solution = mass of solute + mass of solvent

Percent by Mass Problems Calculate the % by mass of a NaCl solution made by adding 50 g of NaCl to 100 mL of water. Calculate the mass of NaCl contained in 200. g of a 6.00% solution of NaCl A 6.00% solution of NaCl contains 40.0 g of NaCl. Calculate the mass of the solution.

Percent by Volume Percent by volume gives the volume of solute per volume units of solution Percent solute=volume of solute x 100% volume of solution volume of solution = volume of solute + volume of solvent

Percent by Volume Problems What is the % by volume of a solution that is made by adding 25 mL of acetone to 100 mL of water? A 6% solution of vinegar contains 3.0 mL of HC2H3O2. Calculate the volume of water that was added.

Molarity Molarity-the moles of solute pervolume of solution in liters. M = molarity = moles of solute liters of solution (solution = solvent + solute)

A solution of NaCl has a molarity of 1 (1M). What does this mean? 1 mole of NaCl is dissolved in enough water to make 1 L. 1 mole = 58 g NaCl A 1M solution of NaCl contains 58 g of NaCl dissolved in 1 liter of water. How much salt is dissolved in a 2M solution? 116 g How much salt is dissolved in a 6 M solution? 348 g Which is more concentrated?

Molarity Problems Calculate the molarity of a solution prepared by dissolving 11.5 g of solid NaOH in enough water to make 1.50 L of solution. Calculate the mass of Ba(OH)2 required to prepare 2.50 L of a 0.0600 M solution of Ba(OH)2.

Molality Molality-the number of moles of solute per kilogram of solvent Molality = moles of solute kilogram of solvent

Review What is the molarity? What is the mass percent? What is the % by volume?

Dilution of Solutions Dilution occurs when more solvent is added to a solution without changing the amount of solute that is present. M1V1 = M2V2 For safety purposes when in a lab setting, concentrated solutions of acids and bases are always added slowly to water.

Dilution Problems How many mL of 18.0 M H2SO4 are required to prepare 1.00 L of a 0.900 M solution of H2SO4?