2Solution Concentration The concentration of a solution is a measure of how much solute is dissolved in a specific amount of solvent or solutionConcentrations can be measured qualitatively and quantitatively.Qualitatively using the words:1- concentrated: contains a large amount of solute.2- dilute: contains a small amount of solute
3Concentration Description Types of MixturesQuantitatively using one of the following concentration ratiosConcentration DescriptionRatioPercent by massmass of solute × 100mass of solutionPercent by volumevolume of solute × 100volume of solutionMolaritymoles of soluteliter of solutionMolalitykilogram of solventMole fractionmoles of solute + moles of solvent
4percent by mass:Q1: In order to maintain a sodium chloride (NaCl) concentration similar to ocean water, an aquarium must contain 3.6 g NaCl per g of water. What is the percent by mass of NaCl in the solution?3.5%Q2: You have g of a bleach solution. The percent by mass of the solute sodium hypochlorite (NaOCl) is 3.62%. How many grams of NaOCl are in the solution?54.3gQ3: The percent by mass of calcium chloride in a solution is found to be 2.65%. If 50.0 g of calcium chloride is used, what is the mass of the solution? g
5Percent by volumeQ1: What is the percent by volume of ethanol in a solution that contains 35 mL of ethanol dissolved in 155 mL of water?18%Q2: What is the percent by volume of isopropyl alcohol in a solution that contains 24 mL of isopropyl alcohol in 1.1 L of water? 2.1%Q3: If 18 mL of methanol is used to make an aqueous solution that is 15% methanol by volume, how many milliliters of solution is produced? 120 mL
6MolarityQ1: A mL intravenous (IV) solution contains 5.10 g of glucose (C6 H12O6). What is the molarity of this solution? The molar masses are, C=12’H=1’O=16 g/mol of glucose MQ2: Calculate the molarity of 1.60 L of a solution containing 1.55 g of dissolved KBr. (K=39,Br=80) MQ3: How much calcium hydroxide (Ca(OH )2), in grams, is needed to produce 1.5 L of a 0.25M solution? (Ca=40,O=16,H=1).28g
7Step 3: Distilled water is added to the flask to bring the solution level up to the calibration mark Step Step Step3How to prepare an accurate solution?Step 1: The mass of the solute is measured.Step 2: The solute is placed in a volumetric flask of the correct volume.
8QuestionsQ1: How many grams of CaCl2 would be dissolved in 1.0 L of a 0.10M solution of CaCl? 11gQ2: How many grams of CaC l2 should be dissolved in mL of water to make a 0.20M solution of CaC l?11g
9Dilution Equationconcentrated solution can be diluted by adding solvent. The number of moles of solute does not change when a concentrated solution is diluted.Dilution Equation:M1 V 1 = M2 V 2M1 and V1 represent the molarity and volume of the stock solution, and M2 and V2 represent the molarity and volume of the dilute solution.
10QuestionsQ1: What volume, in milliliters, of 2.00M calcium chloride (CaC l ) stock solution would you use to make 0.50 L of 0.300M calcium chloride solution? 75mlQ2: If 0.5 L of 5M stock solution of HCl is diluted to make 2 L of solution, how much HCl, in grams, was in the solution? 91.15g
11MolalityQ1: In the lab, a student adds 4.5 g of sodium chloride (NaCl) to g of water. Calculate the molality of the solution. 0.77mol/KgQ2: What is the molality of a solution containing 10.0 g of N a2SO4 dissolved in g of water? mQ3: How much (Ba (OH)2), in grams, is needed to make a 1.00m aqueous solution? 171g
12Mole fractionMole fraction: the ratio of the number of moles of solute in solution to the total number of moles of solute and solvent.Q1: What is the mole fraction of NaOH in an aqueous solution that contains 22.8% NaOH by mass? 0.118If the mole fraction of sulfuric acid ( H2SO4) in an aqueous solution is 0.325, how much water, in grams, is in 100 mL of the solution?43.8%
13QuestionsQ1:Explain the similarities and differences between a 1M solution of NaOH and a 1m solution of NaOH.Both solutions contain NaOH (solute) dissolved in water (solvent). The 1m solution contains 1 mole of NaOH per kilogram of water; the 1M solution contains 1 mole of NaOH per liter of solution.