Download - Chapter 13: Solutions
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Chapter 13: Solutions
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13.1: What is a Solution?
• Objectives:(1)Distinguish between solutions, suspensions,
and colloids.(2)Describe some techniques that chemists use
to separate mixtures.
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SuspensionSolution
Colloid
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Recall…
• Homogeneous mixture: A mixture has a uniform composition.
• Heterogeneous mixture: A mixture that does not have a uniform composition.
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Solution• Solution: A homogeneous mixture.
• Parts of a solution:– Solute: The substance that is dissolved in the solvent.– Solvent: The substance in which the solute is dissolved.
• Examples: Salt dissolves in water.– Salt is the solute.– Water is the solvent.
• Any solution in which water is the solvent is called an aqueous solution.
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Practice
• Identify the solute and solvent in each of the following solutions:
1.Sugar is dissolved in tea.
2. Calcium chloride is dissolved in water.
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Suspension
• Suspension:– Temporary heterogeneous mixture– The different parts of the mixture spontaneously
separate over time
• Examples:– Clay in water (clay settles to the bottom over time)– Sand in water (sand settles to the bottom over time)
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Colloid
• Colloid:– Stable heterogeneous mixture– Particles dispersed evenly but not dissolved– Particles suspended but do not settle– Scatter light
• Examples:– milk, gelatin desserts, whipped cream,
mayonnaise, fog
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Summary
• What is a solution?• What is the solute?• What is the solvent?• What is a suspension?• What is a colloid?• What are 6 methods for separating mixtures?
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13.2 Molarity
• Objective:(1) To calculate the concentration of a solution
in terms of molarity.
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Concentration
• Concentration: amount of solute in solution
• Can be measured in many different ways:– Molarity– Molality– Percent composition– Parts per million (ppm)
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Molarity
• Molarity = moles of solute liters of solution
• Example: 0.30 mol KBr are present in 0.40 L of solution.
• [KBr] = 0.30 mol = 0.75 M KBr 0.40 L
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Practice: Calculating Molarity
1. Calculate the molarity of a solution with 0.38 mol of copper (II) sulfate dissolved in 0.50 liters of solution.
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Practice: Calculating Molarity
Unfortunately, it doesn’t stay that easy…
2. What is the molarity of potassium chloride solution that has a volume of 400.0 mL and contains 85.0 g KCl?
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Practice: Calculating Molarity
3. Vinegar contains 5.0 g of acetic acid, CH3COOH, in 100.0 mL of solution. Calculate the molarity of acetic acid in vinegar.
4. If 18.25 g HCl is dissolved in enough water to make 500.0 mL of solution, what is the molarity of the HCl in solution?
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Practice: Calculating Molarity
5. If 20.0 g H2SO4 is dissolved in enough water to make 250.0 mL of solution, what is the molarity of the sulfuric acid solution?
6. A solution of silver nitrate contains 29.66 g of solute in 100.0 mL of solution. What is the molarity of the solution?
7. A solution of barium hydroxide contains 4.285 g of barium hydroxide in 100.0 mL of solution. What is the molarity of the solution?
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Practice: Solving for mass
8. What mass of KBr is present in 25 mL of 0.85 M solution of KBr?
9. What mass of NaCl is present in 430.0 mL of a 0.45 M NaCl solution?
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Stoichiometry and Molarity
1. An excess of zinc is added to 125 mL of 0.100 M HCl solution. What is the mass of zinc chloride formed? (hyrogen gas is also a product)
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Practice2. Commercial hydrochloric acid, HCl, is 12.0 M.
Calculate the mass of HCl in 250.0 mL of the solution.
3. What volume (in mL) of a 0.500 M solution of copper (II) sulfate is needed to react with an excess of aluminum to provide 11.0 g of copper?
4. Yellow CdS is prepared by reacting ammonium sulfide with cadmium nitrate. What mass of CdS can be prepared to mixing 2.50 L of 1.25 M cadmium nitrate solution with an excess of ammonium sulfide?
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13.3 Dilutions
• Objective:(1) To calculate the molarity of a diluted
solution.
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13.3 Dilutions
• The sulfuric acid we buy comes in 18M. • I need 4 M for my lab. • What should I do?
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13.3 Dilutions
• The sulfuric acid we buy comes in 18M. • I need 4 M for my lab. • What should I do?
DILUTE IT!!
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Dilutions
M1V1 = M2V2
I have 18.0 M sulfuric acid. I need 3.0 L of 4.0 M sulfuric acid. What volume of concentrated sulfuric acid should I use?
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Practice
1. What is the molarity of a solution that is made by diluting 50.00 mL of a 4.74 M solution of HCl to 250.0 mL?
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Practice
2. What volume should 1.19 mL of an 8.00 M acetic acid solution be diluted in order to obtain a final solution that is 1.50 M?
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Practice3. What is the molarity of a solution of ammonium
chloride prepared by diluting 50.0 mL of a 3.70 M ammonium chloride solution to 2.00 L?
4. What volume of water would be added to 16.5 mL of a 0.0813 M solution of sodium borate in order to get a 0.0200 M solution?
5. What volume of water would you add to 15.0 mL of a 6.77 M solution of nitric acid in order to get a 1.50 M solutions?
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13.4 Solubility Curves
• Objective:(1)To define saturated solution, unsaturated
solution, and supersaturated solution.(2)To read a solubility curve.(3)To analyze a solubility curve
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Solubility Curve
• Solubility Curve: tells us how much solute can be dissolved at a given temperature.
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Saturation• Saturated Solution: A solution that cannot dissolve
any more solute under the given conditions.
• Unsaturated Solution: A solution that contains less solute than a saturated solution and that is able to dissolve additional solute.
• Supersaturated Solution: A solution holding more dissolved solute than what is required to reach equilibrium at a given temperature.
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Solubility Curve
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Practice
1.) How many grams of NH4Cl must dissolve for NH4Cl to be saturated at 90⁰C?
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Practice
2.) How many grams of NH4Cl must dissolve in 500 g of H2O to be saturated at 90⁰C?
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Practice
3.)Which solute’s solubility changes the most with temperature?
4.) Which changes the least?
5.) Which solute (s) do not follow the “trend”?
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Practice
6.) How many grams of sodium nitrate will dissolve in 300 g of water 20⁰C?
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Practice
7.) 500 g of water is used to make a saturated solution of KCl at 10⁰C. How many more grams of KCl could be dissolved if the temperature was raised to 100⁰C?
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Practice
8.) A saturated solution of potassium nitrate in 200g of water at 50⁰C is cooled to 20⁰C. How much potassium nitrate will precipitate out of the solution?